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Chemistry

Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson

Chapter 15

Equilibria of Other Reaction Classes - all with Video Answers

Educators

Chapter Questions

03:18

Problem 1

Complete the changes in concentrations for each of the following reactions:
(a) $\begin{aligned} \operatorname{AgI}(s) \longrightarrow & \mathrm{Ag}^{+}(a q)+\mathrm{I}^{-}(a q) \\ x & \end{aligned}$
(b) $\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q)$
(c) $^{\mathrm{Mg}(\mathrm{OH})_{2}(s)} \longrightarrow \mathrm{Mg}^{2+}(a q)+2 \mathrm{OH}^{-}(a q)$
(d) $\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s) \longrightarrow 3 \mathrm{Mg}^{2+}(a q)+2 \mathrm{PO}_{4}^{3-}(a q)$
(e) $\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{3} \mathrm{OH}(s) \longrightarrow 5 \mathrm{Ca}^{2+}(a q)+3 \mathrm{PO}_{4}^{3-}(a q)+\mathrm{OH}^{-}(a q)$

Rikhil Makwana
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01:49

Problem 2

Complete the changes in concentrations for each of the following reactions:
(a) $\operatorname{BaSO}_{4}(s) \longrightarrow \mathrm{Ba}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$
(b) $A \mathrm{g}_{2} \mathrm{SO}_{4}(s) \longrightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$
(c) $\operatorname{Al}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{OH}^{-}(a q)$
(d) $\operatorname{Pb}(\mathrm{OH}) \mathrm{Cl}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+\mathrm{OH}^{-}(a q)+\mathrm{Cl}^{-}(a q)$
(e) $\mathrm{Ca}_{3}\left(\mathrm{AsO}_{4}\right)_{2}(s) \longrightarrow 3 \mathrm{Ca}^{2+}(a q)+2 \mathrm{AsO}_{4}^{3-}(a q)$

Eric Ferrara
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01:16

Problem 3

How do the concentrations of $\mathrm{Ag}^{+}$ and $\mathrm{CrO}_{4}^{2-}$ in a saturated solution above 1.0 $\mathrm{g}$ of solid $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ change when 100 $\mathrm{g}$ of solid $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ is added to the system? Explain.

Rikhil Makwana
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01:19

Problem 4

How do the concentrations of $\mathrm{Pb}^{2+}$ and $\mathrm{S}^{2-}$ change when $\mathrm{K}_{2} \mathrm{S}$ is added to a saturated solution of PbS?

Eric Ferrara
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01:28

Problem 5

What additional information do we need to answer the following question: How is the equilibrium of solid silver bromide with a saturated solution of its ions affected when the temperature is raised?

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03:00

Problem 6

Which of the following slightly soluble compounds has a solubility greater than that calculated from its
solubility product because of hydrolysis of the anion present: $\mathrm{CoSO}_{3}, \mathrm{Cul}, \mathrm{PbCO}_{3}, \mathrm{PbCl}_{2}, \mathrm{Tl}_{2} \mathrm{S}, \mathrm{KClO}_{4} ?$

Eric Ferrara
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04:33

Problem 7

Which of the following slightly soluble compounds has a solubility greater than that calculated from its
solubility product because of hydrolysis of the anion present: $\mathrm{AgCl}, \mathrm{BaSO}_{4}, \mathrm{CaF}_{2}, \mathrm{Hg}_{2} \mathrm{I}_{2}, \mathrm{MnCO}_{3}, \mathrm{ZnS}, \mathrm{PbS} ?$

Rikhil Makwana
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02:29

Problem 8

Write the ionic equation for dissolution and the solubility product $\left(K_{\mathrm{sp}}\right)$ expression for each of the following slightly soluble ionic compounds:
(a) $\mathrm{PbCl}_{2}$
(b) $\mathrm{Ag}_{2} \mathrm{S}$
(c) $\mathrm{Sr}_{3}\left(\mathrm{PO}_{4}\right)_{2}$
(d) $\mathrm{SrSO}_{4}$

Eric Ferrara
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03:07

Problem 9

Write the ionic equation for the dissolution and the $K_{\mathrm{sp}}$ expression for each of the following slightly soluble ionic compounds:
(a) $\mathrm{LaF}_{3}$
(b) $\mathrm{CaCO}_{3}$
(c) $\mathrm{Ag}_{2} \mathrm{SO}_{4}$
(d) $\mathrm{Pb}(\mathrm{OH})_{2}$

Rikhil Makwana
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05:02

Problem 10

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives
solubilities of the following compounds in grams per 100 $\mathrm{mL}$ of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
(a) BaSiF_ $, 0.026 \mathrm{g} / 100 \mathrm{mL}$ (contains $\mathrm{SiF}_{6}^{2-} \mathrm{ions} )$
(b) $\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{4}, 1.5 \times 10^{-2} \mathrm{g} / 100 \mathrm{mL}$
(c) $\mathrm{Gd}_{2}\left(\mathrm{SO}_{4}\right)_{3}, 3.98 \mathrm{g} / 100 \mathrm{mL}$
(d) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{PtBr}_{6}, 0.59 \mathrm{g} / 100 \mathrm{mL}$ (contains $\mathrm{PtBr}_{6}^{2-} \mathrm{ions} )$

Eric Ferrara
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10:08

Problem 11

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.
(a) BaSeO, 0.0118 g/100 mL
(b) $\mathrm{Ba}\left(\mathrm{BrO}_{3}\right)_{2} \cdot \mathrm{H}_{2} \mathrm{O}, 0.30 \mathrm{g} / 100 \mathrm{mL}$
(c) $\mathrm{NH}_{4} \mathrm{Mg} \mathrm{AsO}_{4} \cdot 6 \mathrm{H}_{2} \mathrm{O}, 0.038 \mathrm{g} / 100 \mathrm{mL}$
(d) $\mathrm{La}_{2}\left(\mathrm{MoO}_{4}\right)_{3}, 0.00179 \mathrm{g} / 100 \mathrm{mL}$

Rikhil Makwana
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00:35

Problem 12

Use solubility products and predict which of the following salts is the most soluble, in terms of moles per liter, in pure water: $\mathrm{CaF}_{2}, \mathrm{Hg}_{2} \mathrm{Cl}_{2}, \mathrm{PbI}_{2},$ or $\mathrm{Sn}(\mathrm{OH})_{2}$ .

Eric Ferrara
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05:43

Problem 13

Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) $\mathrm{KHC}_{4} \mathrm{H}_{4} \mathrm{O}_{6}$
(b) $\mathrm{PbI}_{2}$
(c) $\mathrm{Ag}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right],$ a salt containing the $\mathrm{Fe}(\mathrm{CN})_{4}-$ ion
(d) $\mathrm{Hg}_{2} \mathrm{I}_{2}$

Rikhil Makwana
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04:05

Problem 14

Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) $\mathrm{Ag}_{2} \mathrm{SO}_{4}$
(b) $\mathrm{PbBr}_{2}$
(c) AgI
(d) $\mathrm{CaC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O}$

Eric Ferrara
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07:56

Problem 15

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected.
(a) $\operatorname{AgCl}(s)$ in 0.025$M \mathrm{NaCl}$
(b) $\mathrm{CaF}_{2}(s)$ in 0.00133 $\mathrm{M} \mathrm{KF}$
(c) $\mathrm{Ag}_{2} \mathrm{SO}_{4}(s)$ in 0.500 $\mathrm{L}$ of a solution containing 19.50 $\mathrm{g}$ of $\mathrm{K}_{2} \mathrm{SO}_{4}$
(d) $\mathrm{Zn}(\mathrm{OH})_{2}(s)$ in a solution buffered at a pH of 11.45

Aadit Sharma
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06:26

Problem 16

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected.
(a) $\operatorname{TICl}(s)$ in 1.250$M \mathrm{HCl}$
(b) $\operatorname{PbI}_{2}(s)$ in 0.0355$M \mathrm{CaI}_{2}$
(c) $\mathrm{Ag}_{2} \mathrm{CrO}_{4}(s)$ in 0.225 $\mathrm{L}$ of a solution containing 0.856 $\mathrm{g}$ of $\mathrm{K}_{2} \mathrm{CrO}_{4}$
(d) $\mathrm{Cd}(\mathrm{OH})_{2}(s)$ in a solution buffered at a pH of 10.995

Eric Ferrara
Eric Ferrara
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06:26

Problem 17

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions.
(a) $\operatorname{TICl}(s)$ in 0.025$M \mathrm{TINO}_{3}$
(b) $\mathrm{BaF}_{2}(s)$ in 0.0313 $\mathrm{M} \mathrm{KF}$
(c) $\mathrm{MgC}_{2} \mathrm{O}_{4}$ in 2.250 $\mathrm{L}$ of a solution containing 8.156 $\mathrm{g}$ of $\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$
(d) $\mathrm{Ca}(\mathrm{OH})_{2}(s)$ in an unbuffered solution initially with a pH of 12.700

Eric Ferrara
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02:23

Problem 18

Explain why the changes in concentrations of the common ions in Exercise 15.17 can be neglected.

Adriano Chikande
Adriano Chikande
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02:23

Problem 19

Explain why the changes in concentrations of the common ions in Exercise 15.18 cannot be neglected.

Adriano Chikande
Adriano Chikande
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01:35

Problem 20

Calculate the solubility of aluminum hydroxide, Al(OH), in a solution buffered at pH 11.00 .

Eric Ferrara
Eric Ferrara
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08:39

Problem 21

Refer to Appendix J for solubility products for calcium salts. Determine which of the calcium salts listed is most soluble in moles per liter and which is most soluble in grams per liter.

Aadit Sharma
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01:40

Problem 22

Most barium compounds are very poisonous; however, barium sulfate is often administered internally as an aid in the X-ray examination of the lower intestinal tract (Figure 15.4$)$ . This use of BaSO $_{4}$ is possible bessible because of its low solubility. Calculate the molar solubility of BaSO_ and the mass of barium present in 1.00 $\mathrm{L}$ of water saturated with BaSO.

Eric Ferrara
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02:15

Problem 23

Public Health Service standards for drinking water set a maximum of 250 $\mathrm{mg} / \mathrm{L}\left(2.60 \times 10^{-3} \mathrm{M}\right)$ of $\mathrm{SO}_{4}^{2-}$ because of its cathartic action ( it is a laxative). Does natural water that is saturated with CaSO, $\left(" g y p^{\prime \prime} \text { water }\right)$ as a result or passing through soil containing gypsum, $\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}$ , meet these standards? What is the concentration of $\mathrm{SO}_{4}^{2-}$ in such water?

Rikhil Makwana
Rikhil Makwana
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03:19

Problem 24

Perform the following calculations:
(a) Calculate $\left[\mathrm{Ag}^{+}\right]$ in a saturated aqueous solution of AgBr.
(b) What will $\left[\mathrm{Ag}^{+}\right]$ be when enough $\mathrm{KBr}$ has been added to make $\left[\mathrm{Br}^{-}\right]=0.050 \mathrm{M}$ ?
(c) What will $\left[\mathrm{Br}^{-}\right]$ be when enough $\mathrm{AgNO}_{3}$ has been added to make $\left[\mathrm{Ag}^{+}\right]=0.020 \mathrm{M}$ ?

Aadit Sharma
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03:36

Problem 25

The solubility product of $\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}$ is $2.4 \times 10^{-5} .$ What mass of this salt will dissolve in 1.0 $\mathrm{L}$ of 0.010 $\mathrm{M}$ $\mathrm{SO} 4^{2-} ?$

Rikhil Makwana
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04:50

Problem 26

Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a
saturated solution of each of the following (see Appendix J for solubility products).
(a) TICl
(b) $\mathrm{BaF}_{2}$
(c) $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$
(d) $\mathrm{CaC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O}$
(e) the mineral anglesite, PbSO_

Aadit Sharma
Aadit Sharma
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06:13

Problem 27

Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a
saturated solution of each of the following (see Appendix J for solubility products):
(a) AgI
(b) $\mathrm{Ag}_{2} \mathrm{SO}_{4}$
(c) $\mathrm{Mn}(\mathrm{OH})_{2}$
(d) $\mathrm{Sr}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}$
(e) the mineral brucite, $\mathrm{Mg}(\mathrm{OH})_{2}$

Rikhil Makwana
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04:24

Problem 28

The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:
(a) AgBr: $\left[\mathrm{Ag}^{+}\right]=5.7 \times 10^{-7} M,\left[\mathrm{Br}^{-}\right]=5.7 \times 10^{-7} \mathrm{M}$
(b) $\mathrm{CaCO}_{3} :\left[\mathrm{Ca}^{2+}\right]=5.3 \times 10^{-3} M,\left[\mathrm{CO}_{3}^{2-}\right]=9.0 \times 10^{-7} M$
(c) $\mathrm{PbF}_{2} :\left[\mathrm{Pb}^{2+}\right]=2.1 \times 10^{-3} M,\left[\mathrm{F}^{-}\right]=4.2 \times 10^{-3} M$
(d) $\mathrm{Ag}_{2} \mathrm{CrO}_{4} :\left[\mathrm{Ag}^{+}\right]=5.3 \times 10^{-5} M, 3.2 \times 10^{-3} M$
(e) $\operatorname{In} \mathrm{F}_{3} :\left[\operatorname{In}^{3+}\right]=2.3 \times 10^{-3} M,\left[\mathrm{F}^{-}\right]=7.0 \times 10^{-3} \mathrm{M}$

Aadit Sharma
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04:29

Problem 29

The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate $K_{\mathrm{sp}}$ for each of the slightly soluble solids indicated:
(a) TICl: $[\mathrm{T}]^{+} ]=1.21 \times 10^{-2} \mathrm{M},\left[\mathrm{Cl}^{-}\right]=1.2 \times 10^{-2} \mathrm{M}$
(b) $\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{4} :\left[\mathrm{Ce}^{4+}\right]=1.8 \times 10^{-4} M,\left[\mathrm{IO}_{3}^{-}\right]=2.6 \times 10^{-13} \mathrm{M}$
(c) $\mathrm{Gd}_{2}\left(\mathrm{SO}_{4}\right)_{3} :\left[\mathrm{Gd}^{3+}\right]=0.132 \mathrm{M},\left[\mathrm{SO}_{4}^{2-}\right]=0.198 \mathrm{M}$
(d) $\mathrm{Ag}_{2} \mathrm{SO}_{4} :\left[\mathrm{Ag}^{+}\right]=2.40 \times 10^{-2} M,\left[\mathrm{SO}_{4}^{2-}\right]=2.05 \times 10^{-2} \mathrm{M}$
(e) $\mathrm{BaSO}_{4} :\left[\mathrm{Ba}^{2+}\right]=0.500 \mathrm{M},\left[\mathrm{SO}_{4}^{2-}\right]=2.16 \times 10^{-10} \mathrm{M}$

Rikhil Makwana
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04:06

Problem 30

Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for $K_{\mathrm{sp}}$ values. $)$
(a) $\mathrm{KClO}_{4} :\left[\mathrm{K}^{+}\right]=0.01 M,\left[\mathrm{ClO}_{4}^{-}\right]=0.01 M$
(b) $\mathrm{K}_{2} \mathrm{PtCl}_{6} :\left[\mathrm{K}^{4}\right]=0.01 \mathrm{M},\left[\mathrm{PtCl}_{6}^{2-}\right]=0.01 \mathrm{M}$
(c) $\mathrm{PbI}_{2} :\left[\mathrm{Pb}^{2+}\right]=0.003 M,[\mathrm{I}]=1.3 \times 10^{-3} \mathrm{M}$
(d) $\mathrm{Ag}_{2} \mathrm{S} :\left[\mathrm{Ag}^{+}\right]=1 \times 10^{-10} M,\left[\mathrm{S}^{2-}\right]=1 \times 10^{-13} \mathrm{M}$

Aadit Sharma
Aadit Sharma
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04:43

Problem 31

Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for $K_{\mathrm{sp}}$ values.)
(a) $\mathrm{CaCO}_{3} :\left[\mathrm{Ca}^{2+}\right]=0.003 M,\left[\mathrm{CO}_{3}^{2-}\right]=0.003 \mathrm{M}$
(b) $\mathrm{Co}(\mathrm{OH})_{2} :\left[\mathrm{Co}^{2+}\right]=0.01 M,\left[\mathrm{OH}^{-}\right]=1 \times 10^{-7} M$
(c) $\mathrm{CaHPO}_{4} :\left[\mathrm{Ca}^{2+}\right]=0.01 M,\left[\mathrm{HPO}_{4}^{2-}\right]=2 \times 10^{-6} \mathrm{M}$
(d) $\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2} :\left[\mathrm{Pb}^{2+}\right]=0.01 \mathrm{M},\left[\mathrm{PO}_{4}^{3-}\right]=1 \times 10^{-13} \mathrm{M}$

Rikhil Makwana
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01:28

Problem 32

Calculate the concentration of $\mathrm{T}$ t $^{+}$ when TICl just begins to precipitate from a solution that is 0.0250 $\mathrm{M}$ in $\mathrm{Cl}^{-}$

Aadit Sharma
Aadit Sharma
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02:04

Problem 33

Calculate the concentration of sulfate ion when BaSO_ just begins to precipitate from a solution that is 0.0758 $M$ in $\mathrm{Ba}^{2+} .$

Rikhil Makwana
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01:26

Problem 34

Calculate the concentration of $\mathrm{Sr}^{2+}$ when $\mathrm{SrF}_{2}$ starts to precipitate from a solution that is 0.0025$M$ in $\mathrm{F}$ .

Aadit Sharma
Aadit Sharma
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01:11

Problem 35

Calculate the concentration of $\mathrm{PO}_{4}^{3-}$ when $\mathrm{Ag}_{3} \mathrm{PO}_{4}$ starts to precipitate from a solution that is 0.0125 $\mathrm{M}$ in $\mathrm{Ag}^{+} .$

Rikhil Makwana
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01:25

Problem 36

Calculate the concentration of $\mathrm{F}$ - required to begin precipitation of CaF_{in a solution that is } 0 . 0 1 0 \mathrm { M } \text { in } \mathrm { Ca } ^ { 2 + } .

Aadit Sharma
Aadit Sharma
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01:26

Problem 37

Calculate the concentration of Ag' required to begin precipitation of $\mathrm{Ag}_{2} \mathrm{CO}_{3}$ in a solution that is $2.50 \times 10^{-6}$ M in $\mathrm{CO}_{3}^{2-} .$

Rikhil Makwana
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01:17

Problem 38

What $\left[\mathrm{Ag}^{+}\right]$ is required to reduce $\left[\mathrm{CO}_{3}^{2-}\right]$ to $8.2 \times 10^{-4} \mathrm{M}$ by precipitation of $\mathrm{Ag}_{2} \mathrm{CO}_{3} ?$

Aadit Sharma
Aadit Sharma
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01:22

Problem 39

What $\left[\mathrm{F}^{-}\right]$ is required to reduce $\left[\mathrm{Ca}^{2+}\right]$ to $1.0 \times 10^{-4} \mathrm{M}$ by precipitation of $\mathrm{CaF}_{2} ?$

Rikhil Makwana
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03:14

Problem 40

A volume of 0.800 $\mathrm{L}$ of a $2 \times 10^{-4}-M \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ solution is added to 0.200 $\mathrm{L}$ of $5 \times 10^{-4} \mathrm{M} \mathrm{Li}_{2} \mathrm{SO}_{4}$ . Does BaSO_ precipitate? Explain your answer.

Aadit Sharma
Aadit Sharma
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05:32

Problem 41

Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing $\mathrm{NiCO}_{3}$ be washed to dissolve 0.100 $\mathrm{g}$ of this compound? Assume that the wash water becomes saturated with $\mathrm{NiCO}_{3}\left(K_{\mathrm{sp}}=1.36 \times 10^{-7}\right)$
(b) If the NiCO_ were a contaminant in a sample of $\operatorname{CoCO}_{3}\left(K_{\mathrm{sp}}=1.0 \times 10^{-12}\right),$ what mass of $\mathrm{CoCO}_{3}$ would have been lost? Keep in mind that both NiCO_ a and CoCO_ dissolve in the same solution.

Rikhil Makwana
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01:13

Problem 42

Iron concentrations greater than $5.4 \times 10^{-6} M$ in water used for laundry purposes can cause staining. What $\left[\mathrm{OH}^{-}\right]$ is required to reduce $\left[\mathrm{Fe}^{2+}\right]$ to this level by precipitation of Fe(OH $)_{2} ?$

Aadit Sharma
Aadit Sharma
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04:01

Problem 43

A solution is 0.010$M$ in both $\mathrm{Cu}^{2+}$ and $\mathrm{Cd}^{2+}$ . What percentage of $\mathrm{Cd}^{2+}$ remains in the solution when 99.9$\%$ of the $\mathrm{Cu}^{2+}$ has been precipitated as CuS by adding sulfide?

Rikhil Makwana
Rikhil Makwana
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02:24

Problem 44

A solution is 0.15$M$ in both $\mathrm{Pb}^{2+}$ and $\mathrm{Ag}^{+}$ . If $\mathrm{Cl}$ is added to this solution, what is $\left[\mathrm{Ag}^{+}\right]$ when $\mathrm{PbCl}_{2}$ begins to precipitate?

Aadit Sharma
Aadit Sharma
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08:31

Problem 45

45. What reagent might be used to separate the ions in each of the following mixtures, which are 0.1$M$ with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the $K_{\text { sp values given in }}$Appendix J.)
(a) $\mathrm{Hg}_{2}^{2+}$ and $\mathrm{Cu}^{2+}$
(b) $\mathrm{SO}_{4}^{2-}$ and $\mathrm{Cl}^{-}$
(c) $\mathrm{Hg}^{2+}$ and $\mathrm{Co}^{2+}$
(d) $\mathrm{Zn}^{2+}$ and $\mathrm{Sr}^{2+}$
(e) $\mathrm{Ba}^{2+}$ and $\mathrm{Mg}^{2+}$
(f) $\mathrm{CO}_{3}^{2-}$ and $\mathrm{OH}^{-}$

Aadit Sharma
Aadit Sharma
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02:46

Problem 46

A solution contains $1.0 \times 10^{-5}$ mol of KBr and 0.10 mol of $\mathrm{KCl}$ per liter. AgNO $_{3}$ is gradually added to this solution. Which forms first, solid AgBr or solid AgCl?

Aadit Sharma
Aadit Sharma
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02:52

Problem 47

A solution contains $1.0 \times 10^{-2}$ mol of KI and of KCl per liter. AgNO $_{3}$ is gradually added to this solution. Which forms first, solid AgI or solid AgCl?

Rikhil Makwana
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07:41

Problem 48

The calcium ions in human blood serum are necessary for coagulation (Figure 15.5$) .$ Potassium oxalate, $\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4},$ is used as an anticoagulant when a blood sample is drawn for laboratory tests because it removes the calcium as a precipitate of $\mathrm{CaC}_{2} \mathrm{O}_{4} \mathrm{H}_{2} \mathrm{O}$ . It is necessary to remove all but 1.0$\%$ of the $\mathrm{Ca}^{2+}$ in serum in order to prevent coagulation. If normal blood serum with a buffered pH of 7.40 contains 9.5 $\mathrm{mg}$ of $\mathrm{Ca}^{2+}$ per 100 $\mathrm{mL}$ of serum, what mass of $\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ is required to prevent the coagulation of a 10 $\mathrm{mL}$ blood sample that is 55$\%$ serum by volume? (All volumes are accurate to two significant figures. Note that the volume of serum in a 10
mL blood sample is 5.5 $\mathrm{mL}$ . Assume that the $\mathrm{K}_{\mathrm{sp}}$ value for $\mathrm{CaC}_{2} \mathrm{O}_{4}$ in serum is the same as in water.)

Aadit Sharma
Aadit Sharma
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02:14

Problem 49

About 50$\%$ of urinary calculi (kidney stoney stonst of calcium phosphate, $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$ . The normal mid range calcium content excreted in the urine is 0.10 $\mathrm{g}$ of $\mathrm{Ca}^{2+}$ per day. The normal mid range amount of urine passed may be taken as 1.4 $\mathrm{L}$ per day. What is the maximum concentration of phosphate ion that urine can contain before a calculus begins to form?

Aadit Sharma
Aadit Sharma
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07:37

Problem 50

The pH of normal urine is $6.30,$ and the total phosphate concentration (IPO $_{4}^{3-} ]+\left[\mathrm{HPO}_{4}^{2-}\right]+\left[\mathrm{H}_{2} \mathrm{PO}_{4}-\right]$ $+\left[\mathrm{H}_{3} \mathrm{PO}_{4}\right] \mathrm{i}$ ) is 0.020 $\mathrm{M} .$ What is the minimum concentration of $\mathrm{Ca}^{2+}$ necessary to induce kidney stone formation? (See Exercise 15.49 for additional information.)

Aadit Sharma
Aadit Sharma
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06:23

Problem 51

Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of
uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions:
$\mathrm{Mg}^{2+}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)+\mathrm{Ca}^{2+}(a q)$
$\mathrm{Mg}(\mathrm{OH})_{2}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l)$
$\mathrm{MgCl}_{2}(l) \stackrel{\text { electrolysis }}{\longrightarrow} \mathrm{Mg}(s)+\mathrm{Cl}_{2}(g)$
Sea water has a density of 1.026 $\mathrm{g} / \mathrm{cm}^{3}$ and contains 1272 parts per million of magnesium as $\mathrm{Mg}^{2+}(a q)$ by mass. What mass, in kilograms, of $\mathrm{Ca}(\mathrm{OH})_{2}$ is required to precipitate 99.9$\%$ of the magnesium in $1.00 \times 10^{3} \mathrm{L}$ of sea water?

Aadit Sharma
Aadit Sharma
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03:07

Problem 52

Hydrogen sulfide is bubbled into a solution that is 0.10$M$ in both $\mathrm{Pb}^{2+}$ and $\mathrm{Fe}^{2+}$ and 0.30 $\mathrm{M}$ in HCl. After the solution has come to equilibrium it is saturated with $\mathrm{H}_{2} \mathrm{S}\left(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 M\right) .$ What concentrations of $\mathrm{Pb}^{2+}$ and $\mathrm{Fe}^{2+}$ remain in the solution? For a saturated solution of $\mathrm{H}_{2} \mathrm{S}$ we can use the equilibrium:
$$
\mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-}(a q) \quad K=1.0 \times 10^{-26}
$$
(Hint: The $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ changes as metal sulfides precipitate. $)$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:45

Problem 53

Perform the following calculations involving concentrations of iodate ions:
(a) The iodate ion concentration of a saturated solution of $\mathrm{La}\left(\mathrm{IO}_{3}\right)_{3}$ was found to be $3.1 \times 10^{-3} \mathrm{mol} / \mathrm{L}$ . Find the $K_{\mathrm{sp}}$
(b) Find the concentration of iodate ions in a saturated solution of $\mathrm{Cu}\left(\mathrm{IO}_{3}\right)_{2}\left(K_{\mathrm{sp}}=7.4 \times 10^{-8}\right)$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
01:19

Problem 54

Calculate the molar solubility of AgBr in 0.035$M$ NaBr $\left(K_{\mathrm{sp}}=5 \times 10^{-13}\right)$

Aadit Sharma
Aadit Sharma
Numerade Educator
03:36

Problem 55

How many grams of $\mathrm{Pb}(\mathrm{OH})_{2}$ will dissolve in 500 $\mathrm{mL}$ of a $0.050-\mathrm{M} \mathrm{PbCl}_{2}$ solution $\left(K_{\mathrm{sp}}=1.2 \times 10^{-15}\right) ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:52

Problem 56

Use the simulation (http:llopenstaxcollege. orgll/16solublesalts) from the earlier Link to Learning to complete the following exercise: Using 0.01 $\mathrm{g} \mathrm{CaF}_{2}$ give the $\mathrm{K}_{\mathrm{sp}}$ values found in a $0.2-M$ solution of each of the salts. Discuss why the values change as you change soluble salts.

Aadit Sharma
Aadit Sharma
Numerade Educator
03:27

Problem 57

How many grams of Milk of Magnesia, $\mathrm{Mg}(\mathrm{OH})_{2}(s)(58.3 \mathrm{g} / \mathrm{mol})$ , would be soluble in 200 $\mathrm{mL}$ of water. $K_{\mathrm{sp}}=$ $7.1 \times 10^{-12} .$ Include the ionic reaction and the expression for $K_{\mathrm{sp}}$ in your answer. $\left(K_{\mathrm{w}}=1 \times 10^{-14}=\right.$ $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{OH}^{-}\right] )$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
03:00

Problem 58

Two hypothetical salts, LM_ and LQ, have molubility in $\mathrm{H}_{2} \mathrm{O}$ . If $K_{\mathrm{sp}}$ for $\mathrm{LM}_{2}$ is $3.20 \times 10^{-5}$ , what is the $K_{\mathrm{sp}}$ value for LQ?

Aadit Sharma
Aadit Sharma
Numerade Educator
01:06

Problem 59

Which of the following carbonates will form first? Which of the following will form last? Explain.
$$
\begin{array}{ll}{\text { (a) } \mathrm{MgCO}_{3}} & {K_{\mathrm{sp}}=3.5 \times 10^{-8}} \\ {\text { (b) } \mathrm{CaCO}_{3}} & {K_{\mathrm{sp}}=4.2 \times 10^{-7}} \\ {\text { (c) } \mathrm{SrCO}_{3}} & {K_{\mathrm{sp}}=3.9 \times 10^{-9}} \\ {\text { (d) } \mathrm{BaCO}_{3}} & {K_{\mathrm{sp}}=4.4 \times 10^{-5}} \\ {\text { (e) } \mathrm{MnCO}_{3}} & {K_{\mathrm{sp}}=5.1 \times 10^{-9}}\end{array}
$$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
03:04

Problem 60

How many grams of $\operatorname{Zn}(\mathrm{CN})_{2}(s)(117.44 \mathrm{g} / \mathrm{mol})$ would be soluble in 100 $\mathrm{mL}$ of $\mathrm{H}_{2} \mathrm{O}$ ? Include the balanced
reaction and the expression for $K_{\mathrm{sp}}$ in your answer. The $K_{\mathrm{sp}}$ value for $\mathrm{Zn}(\mathrm{CN})_{2}(s)$ is $3.0 \times 10^{-16} .$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:20

Problem 61

Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?

Rikhil Makwana
Rikhil Makwana
Numerade Educator
01:31

Problem 62

Explain why the addition of $\mathrm{NH}_{3}$ or HNO_{3} to a saturated solution of $\mathrm{Ag}_{2} \mathrm{CO}_{3}$ in contact with solid $\mathrm{Ag}_{2} \mathrm{CO}_{3}$ increases the solubility of the solid.

Aadit Sharma
Aadit Sharma
Numerade Educator
05:47

Problem 63

Calculate the cadmium ion concentration, ICd $^{2+} ],$ in a solution prepared by mixing 0.100 $\mathrm{L}$ of 0.0100 $\mathrm{M}$ $\mathrm{Cd}\left(\mathrm{NO}_{3}\right)_{2}$ with 1.150 $\mathrm{L}$ of 0.100 $\mathrm{NH}_{3}(a q) .$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:20

Problem 64

Explain why addition of $\mathrm{NH}_{3}$ or HNO_ to a saturated solution of $\mathrm{Cu (\mathrm{OH})_{2}$ in contact with solid Cu(OH)_ increases the solubility of the solid.

Aadit Sharma
Aadit Sharma
Numerade Educator
02:13

Problem 65

Sometimes equilibria for complex ions are described in terms of dissociation constants, $K_{\mathrm{d}} .$ For the complex ion AlF $_{6} 3-$ the dissociation reaction is:
$$
\mathrm{AlF}_{6}^{3-} \rightleftharpoons \mathrm{Al}^{3+}+6 \mathrm{F}^{-} \text { and } K_{\mathrm{d}}=\frac{\left[\mathrm{Al}^{3+}\right]\left[\mathrm{F}^{-}\right]^{6}}{\left[\mathrm{AlF}_{6}^{3-}\right]}=2 \times 10^{-24}
$$
Calculate the value of the formation constant, $K_{\mathrm{f}},$ for $\mathrm{AlF}_{6}^{3-}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:54

Problem 66

Using the value of the formation constant for the complex ion $\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{2+},$ calculate the dissociation constant.

Aadit Sharma
Aadit Sharma
Numerade Educator
04:33

Problem 67

Using the dissociation constant, $K_{\mathrm{d}}=7.8 \times 10^{-18}$ , calculate the equilibrium concentrations of $\mathrm{Cd}^{2+}$ and $\mathrm{CN}^{-}$ in a $0.250-\mathrm{M}$ solution of $\mathrm{Cd}(\mathrm{CN})_{4}^{2-}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:36

Problem 68

Using the dissociation constant, $K_{\mathrm{d}}=3.4 \times 10^{-15},$ calculate the equilibrium concentrations of $\mathrm{Zn}^{2+}$ and $\mathrm{OH}^{-\mathrm{in}}$ a $0.0465-\mathrm{M}$ solution of $\mathrm{Zn}(\mathrm{OH})_{4}^{2-}$

Aadit Sharma
Aadit Sharma
Numerade Educator
03:00

Problem 69

Using the dissociation constant, $K_{\mathrm{d}}=2.2 \times 10^{-34},$ calculate the equilibrium concentrations of $\mathrm{Co}^{3+}$ and $\mathrm{NH}_{3} \mathrm{in}$ a $0.500-\mathrm{M}$ solution of $\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
01:45

Problem 70

Using the dissociation constant, $K_{\mathrm{d}}=1 \times 10^{-44},$ calculate the equilibrium concentrations of $\mathrm{Fe}^{3+}$ and $\mathrm{CN}^{-}$ in a 0.333 $\mathrm{M}$ solution of $\mathrm{FeCN} )_{6}^{3-}$

Aadit Sharma
Aadit Sharma
Numerade Educator
05:43

Problem 71

Calculate the mass of potassium cyanide ion that must be added to 100 $\mathrm{mL}$ of solution to dissolve $2.0 \times 10^{-2}$ mol of silver cyanide, AgCN.

Aadit Sharma
Aadit Sharma
Numerade Educator
04:05

Problem 72

Calculate the minimum concentration of ammonia needed in 1.0 $\mathrm{L}$ of solution to dissolve $3.0 \times 10^{-3} \mathrm{mol}$ of silver bromide.

Aadit Sharma
Aadit Sharma
Numerade Educator
03:38

Problem 73

A roll of $35-\mathrm{mm}$ black and white photographic film contains about 0.27 $\mathrm{g}$ of unexposed AgBr before developing. What mass of $\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3} \cdot 5 \mathrm{H}_{2} \mathrm{O}(\text { sodium thiosulfate pentahydrate or hypo) in } 1.0 \mathrm{L} \text { of developer is }$ required to dissolve the $\mathrm{AgBr}$ as $\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-}\left(K_{\mathrm{f}}=4.7 \times 10^{13}\right) ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:14

Problem 74

We have seen an introductory definition of an acid: An acid is a compound that reacts with water and increases the amount of hydronium ion present. In the chapter on acids and bases, we saw two more definitions of acids: a compound that donates a proton (a hydrogen ion, $\mathrm{H}^{+} )$ to another compound is called a Brønsted-Lowry acid, and a Lewis acid is any species that can accept a pair of electrons. Explain why the introductory definition is a macroscopic definition, while the Brønsted-Lowry definition and the Lewis definition are microscopic definitions.

Aadit Sharma
Aadit Sharma
Numerade Educator
06:36

Problem 75

Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid the Lewis base in each:
(a) $\mathrm{CO}_{2}+\mathrm{OH}^{-} \rightarrow \mathrm{HCO}_{3}^{-}$
(b) $\mathrm{B}(\mathrm{OH})_{3}+\mathrm{OH}^{-} \rightarrow \mathrm{B}(\mathrm{OH})_{4}-$
(c) $\mathrm{I}^{-}+\mathrm{I}_{2} \longrightarrow \mathrm{I}_{3}^{-}$
(d) $\mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-}$ (use Al-Cl single bonds)
(e) $\mathrm{O}^{2-}+\mathrm{SO}_{3} \longrightarrow \mathrm{SO}_{4}^{2-}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
04:49

Problem 76

Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each:
(a) $\mathrm{CS}_{2}+\mathrm{SH}^{-} \longrightarrow \mathrm{HCS}_{3}^{-}$
(b) $\mathrm{BF}_{3}+\mathrm{F}^{-} \longrightarrow \mathrm{BF}_{4}^{-}$
(c) $\mathrm{I}^{-}+\mathrm{SnI}_{2} \longrightarrow \mathrm{SnI}_{3}^{-}$
(d) $\mathrm{Al}(\mathrm{OH})_{3}+\mathrm{OH}^{-} \longrightarrow \mathrm{Al}(\mathrm{OH})_{4}^{-}$
(e) $\mathrm{F}^{-}+\mathrm{SO}_{3} \longrightarrow \mathrm{SFO}_{3}^{-}$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:14

Problem 77

Using Lewis structures, write balanced equations for the following reactions:
(a) $\mathrm{HCl}(g)+\mathrm{PH}_{3}(g) \longrightarrow$
(b) $\mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3}^{-} \longrightarrow$
(c) $\mathrm{CaO}+\mathrm{SO}_{3} \longrightarrow$
(d) $\mathrm{NH}_{4}^{+}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{O}^{-} \longrightarrow$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
04:25

Problem 78

Calculate $\left[\mathrm{HgCl}_{4}^{2-}\right]$ in a solution prepared by adding 0.0200 $\mathrm{mol}$ of $\mathrm{NaCl}$ to 0.250 $\mathrm{L}$ of a $0.100-\mathrm{M} \mathrm{HgCl}_{2}$ solution.

Aadit Sharma
Aadit Sharma
Numerade Educator
02:39

Problem 79

In a titration of cyanide ion, 28.72 $\mathrm{mL}$ of 0.0100 $\mathrm{M} \mathrm{AgNO}_{3}$ is added before precipitation begins. [The reaction of $\mathrm{Ag}^{+}$ with $\mathrm{CN}^{-}$ goes to completion, producing the $\mathrm{Ag}(\mathrm{CN})_{2}^{-}$ complex.] Precipitation of solid AgCN takes place when excess Ag^+ is added to the solution, above the amount needed to complete the formation of $\operatorname{Ag}(\mathrm{CN})_{2}-$ How many grams of NaCN were in the original sample?

Aadit Sharma
Aadit Sharma
Numerade Educator
04:38

Problem 80

What are the concentrations of $\mathrm{Ag}^{+}, \mathrm{CN}^{-},$ and $\mathrm{Ag}(\mathrm{CN})_{2}-$ in a saturated solution of AgCN?

Aadit Sharma
Aadit Sharma
Numerade Educator
01:57

Problem 81

In dilute aqueous solution $\mathrm{HF}$ acts as a weak acid. However, pure liquid HF (boiling point $=19.5^{\circ} \mathrm{C} )$ is a strong acid. In liquid HF, HNO_ acts like and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that are Lewis acids and accept $\mathrm{F}^{-}$ ion (for example, $\mathrm{BF}_{3}$ or $\mathrm{SbF}_{5} ) .$ Write balanced chemical equations for the reaction of pure $\mathrm{HNO}_{3}$ with pure $\mathrm{HF}$ and of pure $\mathrm{HF}$ with $\mathrm{BF}_{3}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:41

Problem 82

The simplest amino acid is glycine, $\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CO}_{2} \mathrm{H}$ . The common feature of amino acids is that they contain the functional groups: an amine group, $-\mathrm{NH}_{2},$ and a carboxylic acid group, $-\mathrm{CO}_{2} \mathrm{H}$ . An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},$ and the base strength of the amino group is slightly greater than that of ammonia, $\mathrm{NH}_{3}$
(a) Write the Lewis structures of the ions that form when glycine is dissolved in 1$M \mathrm{HCl}$ and in 1 $\mathrm{M} \mathrm{KOH}$ .
(b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the $-\mathrm{NH}_{2}$ and $-\mathrm{CO}_{2}^{-}$ groups.)

Aadit Sharma
Aadit Sharma
Numerade Educator
01:53

Problem 83

Boric acid, $\mathrm{H}_{3} \mathrm{BO}_{3},$ is not a Bronsted-Lowry acid but a Lewis acid.
(a) Write an equation for its reaction with water.
(b) Predict the shape of the anion thus formed.
(c) What is the hybridization on the boron consistent with the shape you have predicted?

Rikhil Makwana
Rikhil Makwana
Numerade Educator
01:10

Problem 84

A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system called a heterogeneous equilibrium?

Aadit Sharma
Aadit Sharma
Numerade Educator
03:08

Problem 85

Calculate the equilibrium concentration of $\mathrm{Ni}^{2+}$ in a $1.0-M$ solution $\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]\left(\mathrm{NO}_{3}\right)_{2}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:19

Problem 86

Calculate the equilibrium concentration of $\mathrm{Ni}^{2+}$ in a $1.0-M$ solution $\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]\left(\mathrm{NO}_{3}\right)_{2}$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:14

Problem 87

Calculate the equilibrium concentration of $\mathrm{Cu}^{2+}$ in a solution initially with 0.050$M \mathrm{Cu}^{2+}$ and 1.00 $\mathrm{M} \mathrm{NH}_{3}$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:33

Problem 88

Calculate the equilibrium concentration of $\mathrm{Zn}^{2+}$ in a solution initially with 0.150 $\mathrm{M} \mathrm{Zn}^{2+}$ and 2.50 $\mathrm{MCN}$ .

Aadit Sharma
Aadit Sharma
Numerade Educator
02:02

Problem 89

Calculate the Fe $\mathrm{Fe}^{3+}$ equilibrium concentration when 0.0888 mole of $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ is added to a solution with 0.000010 $\mathrm{CN}^{-}$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:17

Problem 90

Calculate the $\mathrm{Co}^{2+}$ equilibrium concentration when 0.100 mole of $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]_{6} ]\left(\mathrm{NO}_{3}\right)_{2}$ is added to a solution with 0.025 $\mathrm{M} \mathrm{NH}_{3}$ . Assume the volume is 1.00 $\mathrm{L}$ .

Aadit Sharma
Aadit Sharma
Numerade Educator
03:23

Problem 91

The equilibrium constant for the reaction $\mathrm{Hg}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{HgCl}_{2}(a q)$ is $1.6 \times 10^{13} .$ Is $\mathrm{HgCl}_{2}$ a
strong electrolyte or a weak electrolyte? What are the concentrations of $\mathrm{Hg}^{2+}$ and $\mathrm{Cl}^{-}$ in a $0.015-\mathrm{M}$ solution of $\mathrm{HgCl}_{2} ?$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:27

Problem 92

Calculate the molar solubility of $\mathrm{Sn}(\mathrm{OH})_{2}$ in a buffer solution containing equal concentrations of $\mathrm{NH}_{3}$ and $\mathrm{NH}_{4}^{+}$

Aadit Sharma
Aadit Sharma
Numerade Educator
03:45

Problem 93

Calculate the molar solubility of All(OH) $_{3}$ in a buffer solution with 0.100$M \mathrm{NH}_{3}$ and 0.400$M \mathrm{NH}_{4}^{+}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
05:06

Problem 94

What is the molar solubility of $\mathrm{CaF}_{2}$ in a $0.100-\mathrm{M}$ solution of $\mathrm{HF} ? K_{\mathrm{a}}$ for $\mathrm{HF}=7.2 \times 10^{-4}$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:57

Problem 95

What is the molar solubility of $\mathrm{BaSO}_{4}$ in a $0.250-M$ solution of $\mathrm{NaHSO}_{4} ? K_{\mathrm{a}}$ for $\mathrm{HSO}_{4}^{-}=1.2 \times 10^{-2}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
03:22

Problem 96

What is the molar solubility of $\mathrm{T} ](\mathrm{OH})_{3}$ in a $0,10-\mathrm{M}$ solution of $\mathrm{NH}_{3} ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:15

Problem 97

What is the molar solubility of $\mathrm{Pb}(\mathrm{OH})_{2}$ in a $0.138-M$ solution of $\mathrm{CH}_{3} \mathrm{NH}_{2} ?$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
03:42

Problem 98

A solution of 0.075$M$ CoBr_ated with $\mathrm{H}_{2} \mathrm{S}\left(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 \mathrm{M}\right) .$ What is the minimum pH at which $\mathrm{CoS}$
begins to precipitate?
$$
\begin{array}{l}{\operatorname{CoS}(s) \rightleftharpoons \mathrm{Co}^{2+}(a q)+\mathrm{S}^{2-}(a q)} \\ {\mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-}(a q) \quad K=1.0 \times 10^{-26}}\end{array}
$$

Aadit Sharma
Aadit Sharma
Numerade Educator
03:33

Problem 99

A $0.125-M$ solution of $\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}$ is saturated with $\mathrm{H}_{2} \mathrm{S}\left(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 \mathrm{M}\right) .$ At what pH does MnS begin to precipitate?
$$
\operatorname{Mn} S(s) \rightleftharpoons \operatorname{Mn}^{2+}(a q)+S^{2-}(a q) \quad K_{\mathrm{sp}}=4.3 \times 10^{-22}
$$
$$
\mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-(a q)} \qquad K=1.0 \times 10^{-26}
$$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
02:40

Problem 100

Calculate the molar solubility of $\mathrm{BaF}_{2}$ in a buffer solution containing 0.20 $\mathrm{M}$ HF and 0.20 $\mathrm{M} \mathrm{NaF}$

Aadit Sharma
Aadit Sharma
Numerade Educator
06:29

Problem 101

Calculate the molar solubility of $\mathrm{CdCO}_{3}$ in a buffer solution containing 0.115 $\mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}$ and 0.120 $\mathrm{M}$
$\mathrm{NaHCO}_{3}$

Rikhil Makwana
Rikhil Makwana
Numerade Educator
04:19

Problem 102

To a $0.10-M$ solution of $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$ is added enough $\mathrm{HF}(g)$ to make $[\mathrm{HF}]=0.10 \mathrm{M}$
(a) Does $\mathrm{PbF}_{2}$ precipitate from this solution? Show the calculations that support your conclusion.
(b) What is the minimum pH at which PbF_ precipitates?

Aadit Sharma
Aadit Sharma
Numerade Educator
03:39

Problem 103

Calculate the concentration of $\mathrm{Cd}^{2+}$ resulting from the dissolution of $\mathrm{CdCO}_{3}$ in a solution that is 0.250 $\mathrm{M}$ in $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}, 0.375 \mathrm{M}$ in $\mathrm{NaCH}_{3} \mathrm{CO}_{2},$ and 0.010 $\mathrm{M}$ in $\mathrm{H}_{2} \mathrm{CO}_{3}$ .

Aadit Sharma
Aadit Sharma
Numerade Educator
03:57

Problem 104

Both AgCl and AgI dissolve in $\mathrm{NH}_{3}$
(a) What mass of AgI dissolves in 1.0 $\mathrm{L}$ of 1.0 $\mathrm{MNH}_{3} ?$
(b) What mass of AgCl dissolves in 1.0 $\mathrm{L}$ of 1.0 $\mathrm{MNH}_{3} ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:10

Problem 105

Calculate the volume of 1.50 $\mathrm{M} \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$ required to dissolve a precipitate composed of 350 $\mathrm{mg}$ each of $\mathrm{CaCO}_{3}, \mathrm{SrCO}_{3},$ and $\mathrm{BaCO}_{3}$ .

Aadit Sharma
Aadit Sharma
Numerade Educator
02:24

Problem 106

Even though $\mathrm{Ca}(\mathrm{OH})_{2}$ is an inexpensive base, its limited solubility restricts its use. What is the pH of a saturated solution of $\mathrm{Ca}(\mathrm{OH})_{2} ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:07

Problem 107

What mass of NaCN must be added to 1 $\mathrm{L}$ of 0.010 $\mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ in order to produce the first trace of $\mathrm{Mg}(\mathrm{OH})_{2} ?$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:19

Problem 108

Magnesium hydroxide and magnesium citrate function as mild laxatives when they reach the small intestine. Why do magnesium hydroxide and magnesium citrate, two very different substances, have the same effect in your small intestine. (Hint: The contents of the small intestine are basic.)

Aadit Sharma
Aadit Sharma
Numerade Educator
02:17

Problem 109

The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service.
Solve the following problem:
$$
\mathrm{MgF}_{2}(s) \rightleftharpoons \mathrm{Mg}^{2+}(a q)+2 \mathrm{F}^{-}(a q)
$$
(a) Write the expression for the solubility-product constant, $K_{\mathrm{sp}},$ and calculate its value at $18^{\circ} \mathrm{C}$
(b) Calculate the equilibrium concentration of $\mathrm{Mg}^{2+}$ in 1.000 $\mathrm{L}$ of saturated $\mathrm{MgF}_{2}$ solution at $18^{\circ} \mathrm{C}$ to which 0.100 mol of solid $\mathrm{KF}$ has been added. The KF dissolves completely. Assume the volume change is negligible.
(c) Predict whether a precipitate of $\mathrm{MgF}_{2}$ will form when 100.0 $\mathrm{mL}$ of a $3.00 \times 10^{-3}$ -M solution of $\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ is mixed with 200.0 $\mathrm{mL}$ of a $2.00 \times 10^{-3}$ -M solution of NaF at $18^{\circ} \mathrm{C} .$ Show the calculations to support your prediction.
(d) At $27^{\circ} \mathrm{C}$ the concentration of $\mathrm{Mg}^{2+}$ in a saturated solution of $\mathrm{MgF}_{2}$ is $1.17 \times 10^{-3} \mathrm{M} .$ . Is the dissolving of $\mathrm{MgF}_{2}$ in water an endothermic or an exothermic process? Give an explanation to support your conclusion.

Aadit Sharma
Aadit Sharma
Numerade Educator
01:05

Problem 110

Which of the following compounds, when dissolved in a 0.01 -M solution of HClO, has a solubility greater
than in pure water: $\mathrm{CuCl}$ , $\mathrm{CaCO}_{3}, \mathrm{MnS}, \mathrm{PbBr}_{2}, \mathrm{CaF}_{2} ?$ Explain your answer.

Aadit Sharma
Aadit Sharma
Numerade Educator
02:38

Problem 111

Which of the following compounds, when dissolved in a $0.01-M$ solution of HClO_ hity greater than in pure water: $\mathrm{AgBr}, \mathrm{BaF}_{2}, \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}, \mathrm{ZnS}, \mathrm{PbI}_{2} ?$ Explain your answer.

Rikhil Makwana
Rikhil Makwana
Numerade Educator
03:34

Problem 112

What is the effect on the amount of solid $\mathrm{Mg}(\mathrm{OH})_{2}$ that dissolves and the concentrations of $\mathrm{Mg}^{2+}$ and $\mathrm{OH}^{-}$ when each of the following are added to a mixture of solid $\mathrm{Mg}(\mathrm{OH})_{2}$ and water at equilibrium?
(a) $\mathrm{MgCl}_{2}$
(b) $\mathrm{KOH}$
(c) $\mathrm{HClO}_{4}$
(d) $\mathrm{NaNO}_{3}$
(e) $\mathrm{Mg}(\mathrm{OH})_{2}$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:47

Problem 113

What is the effect on the amount of CaHPO_ that dissolves and the concentrations of $\mathrm{Ca}^{2+}$ and $\mathrm{HPO}_{4}^{-}$ when each of the following are added to a mixture of solid CaHPO $_{4}$ and water at equilibrium?
(a) $\mathrm{CaCl}_{2}$
(b) $\mathrm{HCl}$
(c) $\mathrm{KClO}_{4}$
(d) $\mathrm{NaOH}$
(e) CaHPO_ $_{4}$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:52

Problem 114

Identify all chemical species present in an aqueous solution of $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$ and list these species in decreasing order of their concentrations. (Hint: Remember that the $\mathrm{PO}_{4}^{3-}$ ion is a weak base.)

Aadit Sharma
Aadit Sharma
Numerade Educator
03:17

Problem 115

A volume of 50 $\mathrm{mL}$ of 1.8 $\mathrm{M} \mathrm{NH}_{3}$ is mixed with an equal volume of a solution containing 0.95 $\mathrm{g}$ of $\mathrm{MgCl}_{2}$ What mass of $\mathrm{NH}_{4} \mathrm{Cl}$ must be added to the resulting solution to precipitation of $\mathrm{Mg}(\mathrm{OH})_{2} ?$

Aadit Sharma
Aadit Sharma
Numerade Educator