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Principles of Descriptive Inorganic Chemistry

Gary Wulfsberg

Chapter 3

Ionic Solids and Precipitation Reactions of Hydrated Ions - all with Video Answers

Educators

Chapter Questions

01:59

Problem 1

Which of the following salts will be insoluble in water? $\mathrm{Co}\left(\mathrm{NO}_3\right)_2, \mathrm{CsBrO}_4$, $\mathrm{CePO}_4, \mathrm{Cs}_3 \mathrm{AsO}_4, \mathrm{BaSeO}_4, \mathrm{Hg}_5\left(\mathrm{IO}_6\right)_2, \mathrm{TiO}_2$.

Kim Trang Nguyen
Kim Trang Nguyen
Numerade Educator
01:15

Problem 2

Which of the following salts will be insoluble in water? $\mathrm{CuMoO}, \mathrm{Cs}_2 \mathrm{MoO}_4$, $\mathrm{Cr}_2 \mathrm{TeO}_6, \mathrm{Cr}\left(\mathrm{NO}_3\right)_3, \mathrm{HgO}, \mathrm{NaOH}, \mathrm{RbTcO}_4, \mathrm{KIO}_4, \mathrm{~K}_5 \mathrm{IO}_6$.

David Collins
David Collins
Numerade Educator
02:29

Problem 3

Write general chemistry-type specific solubility rules for the salts of the following oxo anions: a. chromate; b. ferrate; c. pertechnetate; d. silicate; e. tellurate. These rules should state whether most salts of this anion are soluble or insoluble; then list some ions that are exceptions.

Eileen Sullivan
Eileen Sullivan
Numerade Educator
00:27

Problem 4

Describe the structures of ice and of liquid water, and explain why ice floats in water.

David Collins
David Collins
Numerade Educator
02:18

Problem 5

Use one of the following ions $\left(\mathrm{Al}^{3+}, \mathrm{Li}^{+}, \mathrm{Rb}^{+},\left(\mathrm{C}_4 \mathrm{H}_9\right)_4 \mathrm{~N}^{+}\right)$to complete each of the following: a. the ion that attaches the fewest water molecules when it dissolves in water; $\mathbf{b}$, the ion that forms the largest hydrated ion; $\mathbf{c}$, a hydrophobic structure maker; d. an electrostatic structure maker; e. an electrostatic structure breaker.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:18

Problem 6

Consider the following set of ions: $\mathrm{K}^{+}, \mathrm{Zn}^{2+}, \mathrm{Al}^{3+}, \mathrm{SiO}_4{ }^{4-}, \mathrm{ClO}_4^{-}, \mathrm{SeO}_4^{2-}$. a. Which cation will form the largest hydrated ion? $\mathbf{b}$. Which cation(s) will be electrostatic structure makers? c. Which cation(s) will disrupt the icebergs in liquid water? d. Which anion is most likely to be an electrostatic structure breaker? e. Which cation(s) will give insoluble salt(s) with the $\mathrm{ClO}_4^{-}$ion? f. Which cation(s) will give insoluble salt(s) with the $\mathrm{SiO}_4^{4-}$ ion? g. Write the formula of any salt containing just these ions that will precipitate for reasons connected with an entropy change. $\mathbf{h}$. Write the formula of any soluble salt containing just these ions and explain (in terms of lattices, etc.) why it is soluble.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:07

Problem 7

Give an example of a salt composed of a cation and an anion, each of which is an electrostatic structure maker. Is such a salt likely to be soluble or insoluble? Give the physical reason for this (in terms of the structure of the hydrated ions, the suitability of its lattice, etc.). Is this solubility/insolubility associated with entropy or enthalpy effects?

Arpit Gupta
Arpit Gupta
Numerade Educator
03:36

Problem 8

Enthalpies of precipitation are known for the following halides: LiF, $-5 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{NaCl},-4 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{AgCl},-65 \mathrm{~kJ} / \mathrm{mol} ; \mathrm{CaCl}_2,+83 \mathrm{~kJ} / \mathrm{mol}$.
8.1 Use data on hydration enthalpies (Tables 2.1 and 2.5) to calculate the lattice energies of these compounds.
8.2 All but one of these halides (which one?) have the $\mathrm{NaCl}$ structure. Calculate the lattice energies of these compounds from their ionic radii, Madelung constants, etc. (Use the radius ratio to choose the lattice type for the halide with the non- $\mathrm{NaCl}$ structure.) For which halide is there the greatest discrepancy between your answers to the previous part and to this part? How does the cation in this halide differ from the other three cations, and how might this explain the discrepancy?

Shazia Naz
Shazia Naz
Numerade Educator
00:52

Problem 9

The hydration energy of the sulfate ion is not given in Table 2.5.
9.1 Use the known lattice energies for $\mathrm{CaSO}_4(-2653 \mathrm{~kJ} / \mathrm{mol}), \mathrm{SrSO}_4$ $(-2603 \mathrm{~kJ} / \mathrm{mol})$, and $\mathrm{BaSO}_4(-2423 \mathrm{~kJ} / \mathrm{mol})$, along with data from Tables 2.1 and 3.1 , to compute the hydration energy of the sulfate ion. How well do your results agree for each of these three salts?
9.2 Compare your result with the hydration energy of the perchlorate ion, which has a similar size, and explain any differences between the two.

Aashna Calidas
Aashna Calidas
Numerade Educator
02:59

Problem 10

Usually, $\Delta H^{\circ}$ for the precipitation of an ionic salt is about equal to zero. Use this approximate value and the hydration energies for $\mathrm{Al}^{3+}$ and for $\mathrm{ClO}_4$ (Tables 2.1 and 2.5) to estimate the lattice energy of aluminum perchlorate.

Lottie Adams
Lottie Adams
Numerade Educator
08:50

Problem 11

Using Tables C, 2.5, and 3.4: a. calculate the radius ratio for $\mathrm{CeO}_2$ and predict the coordination numbers of the cerium and oxide ions and the type of lattice that $\mathrm{CeO}_2$ would adopt; $\mathbf{b}$. calculate the lattice energy of $\mathrm{CeO}_2$.

James Irizarry
James Irizarry
Numerade Educator
02:48

Problem 12

Cesium and gold form an ionic compound, $\mathrm{Cs}^{+} \mathrm{Au}^{-}$, with a cesium-gold distance of 369 pm. a. What type of lattice will CsAu adopt? b. Estimating a suitable Born exponent for the $\mathrm{Au}^{-}$ion, calculate the lattice energy of $\mathrm{CsAu}$. c. Assuming that the enthalpy of precipitation of CsAu is zero, calculate the enthalpy of hydration of the $\mathrm{Au}^{-}$ion.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
03:25

Problem 13

Calculate the Madelung constant for: a. a simple cube consisting of four cations alternating corners with four anions; $\mathbf{b}$. an infinite linear arrangement of alternating cations and anions. This case involves an infinite series. Do you know the sum of this series from your calculus course? If not, add up the first ten terms.

Suzanne W.
Suzanne W.
Numerade Educator
04:41

Problem 14

Aluminum phosphate is quite insoluble. Which effect is responsible for its insolubility? a. An enthalpy effect resulting from the very stable lattice formed; b. an entropy effect resulting from the very stable lattice formed; c. an enthalpy effect resulting from the release of numerous waters of hydration when forming aluminum phosphate from its ions; d. an entropy effect resulting from the release of numerous waters of hydration when forming aluminum phosphate from its ions; $\mathbf{e}$. an enthalpy effect resulting from the disruption of the structure of liquid water by the large ions; $\mathbf{f}$. an entropy effect resulting from the large ions disrupting the structure of liquid water.

Shazia Naz
Shazia Naz
Numerade Educator
01:34

Problem 15

Explain, with reference to the structure of water, of crystal lattices, and or of hydrated ions, why: a. iron(III) perchlorate is soluble in water; $\mathbf{b}$. iron(III) phosphate is insoluble in water; c. rubidium permanganate is fairly insoluble in water; $\mathbf{d}$. tetrabutylammonium tetrabutylborate is insoluble in water.

Hitendra Singh
Hitendra Singh
Numerade Educator
01:08

Problem 16

Will $\mathrm{BeSO}_4$ or $\mathrm{BaSO}_4$ be more likely to be a. a good desiccant, or b. crystallize as a hydrate?

Anand Jangid
Anand Jangid
Numerade Educator
01:27

Problem 17

Liming a lake to neutralize acid rain in it could seriously affect the availability of nutrients such as phosphate and molybdate, but not nitrate. Explain.

David Collins
David Collins
Numerade Educator
00:54

Problem 18

Assume that the rare, radioactive elements astatine and polonium form anions $\mathrm{At}^{-}$and $\mathrm{Po}^{2-}$, each of which has a radius of about $226 \mathrm{pm}$. Which of the following lattice types $\left(\mathrm{ZnS}, \mathrm{NaCl}, \mathrm{CsCl}, \mathrm{SiO}_2, \mathrm{TiO}_2, \mathrm{CaF}_2\right)$ would be expected to be adopted by: a. the astatide of each Group 1 metal ( Na through Cs); b. the astatide of each Group 2 metal ( $\mathrm{Mg}$ through Ba); $\mathbf{c}$. the polonide of each Group 2 metal ( $\mathrm{Mg}$ through $\mathrm{Ba}$ ).

ES
Eugene Schneider
University of Minnesota - Twin Cities
00:58

Problem 19

Using your results from the previous question and Table 3.4, calculate the lattice energy of barium astatide. If we assume that the enthalpy of solution of barium astatide in water in zero, calculate the hydration energy of the astatide ion. Draw the hydrated astatide ion, showing how the water molecules would orient themselves.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:14

Problem 20

In organic lab you have just synthesized the tropylium ion, $\mathrm{C}_7 \mathrm{H}_7{ }^{+}$, in solution. Tell how you would isolate it from solution to get a stable crystalline solid.

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
03:17

Problem 21

Generalized solubility rule IV in section 3.2 says that many feebly acidic cations and feebly basic anions give insoluble salts. Both $\mathrm{Li}^{+}$and $\mathrm{Ba}^{2+}$ are feebly acidic cations, and $\mathrm{NO}_2^{-}, \mathrm{ClO}_2^{-}, \mathrm{SO}_4{ }^{2-}$, and $\mathrm{SeO}_4{ }^{2-}$ are all feebly basic anions. Although $\mathrm{BaSO}_4$ and $\mathrm{BaSeO}_4$ are indeed insoluble, $\mathrm{Ba}\left(\mathrm{NO}_2\right)_2$, $\mathrm{Ba}\left(\mathrm{ClO}_2\right)_2, \mathrm{Li}_2 \mathrm{SO}_4$, and $\mathrm{Li}_2 \mathrm{SeO}_4$ are all soluble. Can you explain this?

Mahendra K
Mahendra K
Numerade Educator
02:07

Problem 22

Which of the following structural descriptions is/are inconsistent with the stoichiometry of the salt being described?
22.1 $\mathrm{CdCl}_2$ adopts a hep lattice of chloride ions in which all the octahedral holes are occupied by cadmium ions.
$22.2 \mathrm{CdCl}_2$ adopts a ccp lattice of chloride ions in which half of the octahedral holes are occupied by cadmium ions.
22.3 $\mathrm{Li}_2 \mathrm{SO}_4$ adopts a hep lattice of sulfate ions in which all the tetrahedral holes are occupied by lithium ions.
$22.4\left(\mathrm{CH}_3\right)_4 \mathrm{NF}$ adopts a cep lattice of tetramethylammonium ions in which all the octahedral holes are occupied by fluoride ions.

Arpit Gupta
Arpit Gupta
Numerade Educator
04:38

Problem 23

Rewrite each of the following molecular equations as a net ionic equation:
$$
\begin{aligned}
& 23.1 \mathrm{Ba}\left(\mathrm{ClO}_4\right)_2(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{BaSO}_4(\mathrm{~s})+2 \mathrm{HClO}_4(\mathrm{aq}) \\
& 23.2 \mathrm{Na}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{H}_2 \mathrm{SeO}_3(\mathrm{aq})+\mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\
& 23.32 \mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq})+\mathrm{Na}_4 \mathrm{SiO}_4(\mathrm{aq}) \rightarrow \mathrm{Si}(\mathrm{OH})_4(\mathrm{~s})+2 \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq}) \\
& 23.43 \mathrm{Th}\left(\mathrm{NO}_3\right)_4(\mathrm{aq})+4 \mathrm{~K}_2 \mathrm{NaPO}_4(\mathrm{aq}) \rightarrow \mathrm{Th}_3\left(\mathrm{PO}_4\right)_4(\mathrm{~s})+8 \mathrm{KNO}_3(\mathrm{aq})+ \\
& 4 \mathrm{NaNO}_3(\mathrm{aq}) \\
& 23.52 \mathrm{NaHSO}_3(\mathrm{aq})+\mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq}) \rightarrow \mathrm{Na}_2 \mathrm{SO}_4(\mathrm{aq})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+2 \mathrm{SO}_2(\mathrm{~g}) \\
&
\end{aligned}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
05:12

Problem 24

Using a chemistry handbook, write specific instructions (compounds used, weight of each compound needed) to carry out the following net ionic equations and produce $0.20 \mathrm{~mol}$ of product:
$$
\begin{aligned}
& 24.13 \mathrm{Co}^{2+}(\mathrm{aq})+2 \mathrm{VO}_4{ }^{3-}(\mathrm{aq}) \rightarrow \mathrm{Co}_3\left(\mathrm{VO}_4\right)_2(\mathrm{~s}) \\
& 24.22 \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{SO}_4^{2-}(\mathrm{aq}) \rightarrow \mathrm{Ag}_2 \mathrm{SO}_4(\mathrm{~s}) \\
& 24.33 \mathrm{Mg}^{2+}(\mathrm{aq})+2 \mathrm{AsO}_4{ }^{3-}(\mathrm{aq}) \rightarrow \mathrm{Mg}_3\left(\mathrm{AsO}_4\right)_2(\mathrm{~s}) \\
& 24.43 \mathrm{UO}_2{ }^{2+}(\mathrm{aq})+2 \mathrm{VO}_4{ }^{3-}(\mathrm{aq}) \rightarrow\left(\mathrm{UO}_2\right)_3\left(\mathrm{VO}_4\right)_2(\mathrm{~s})
\end{aligned}
$$

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator

Problem 25

If you did not do the experiment at the beginning of this chapter, go back and try to apply the principles of this chapter to predict what would have happened at each step. Also answer the questions included.

Check back soon!