Introductory Chemistry Essentials

Problem 38

Write the formula for the conjugate acid of each base.
(a) $\mathrm{CH}_{3} \mathrm{NH}_{2}$
(b) $\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}$
(c) $\mathrm{Cl}^{-}$
(d) $\mathrm{F}^{-}$

David Collins

Numerade Educator

03:01

Problem 39

Write a neutralization reaction for each acid and base pair.
(a) $\mathrm{HI}(a q)$ and $\mathrm{NaOH}(a q)$
(b) $\mathrm{HBr}(a q)$ and $\mathrm{KOH}(a q)$
(c) $\mathrm{HNO}_{3}(a q)$ and $\mathrm{Ba}(\mathrm{OH})_{2}(a q)$
(d) $\mathrm{HClO}_{4}(a q)$ and $\mathrm{Sr}(\mathrm{OH})_{2}(a q)$

David Collins

Numerade Educator

02:45

Problem 40

Write a balanced chemical equation showing how each metal reacts with $\mathrm{HCl}$.
(a) $K$
(b) $\mathrm{Ca}$
(c) $\mathrm{Na}$
(d) Sr

David Collins

Numerade Educator

01:45

Problem 41

Write a neutralization reaction for each acid and base pair.
(a) $\mathrm{CH}_{3} \mathrm{COOH}$ and $\mathrm{KOH}$
(b) $\mathrm{H}_{2} \mathrm{SO}_{4}$ and $\mathrm{NaOH}$
(c) $\mathrm{HCl}$ and $\mathrm{LiOH}$
(d) $\mathrm{H}_{3} \mathrm{PO}_{4}$ and $\mathrm{Ca}(\mathrm{OH})_{2}$

Susan Hallstrom

Numerade Educator

02:45

Problem 42

Write a balanced chemical equation showing how each metal reacts with HCl.
(a) $\mathrm{K}$
(b) Ca
(c) Na
(d) Sr

David Collins

Numerade Educator

03:10

Problem 43

Write a balanced chemical equation showing how each metal oxide reacts with $\mathrm{HNO}_{3}$.
(a) $\mathrm{Li}_{2} \mathrm{O}$
(b) $\mathrm{CaO}$
(c) $\mathrm{Na}_{2} \mathrm{O}$
(d) $\mathrm{Al}_{2} \mathrm{O}_{3}$

David Collins

Numerade Educator

02:18

Problem 44

Write a balanced chemical equation showing how each metal oxide reacts with HCl.
(a) SrO
(b) $\mathrm{Na}_{2} \mathrm{O}$
(c) $\mathrm{Li}_{2} \mathrm{O}$
(d) $\mathrm{BaO}$

David Collins

Numerade Educator

02:50

Problem 45

Predict the products of each reaction.
(a) $\mathrm{HClO}_{4}(a q)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow$
(b) $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\operatorname{Sr}(s) \longrightarrow$
(c) $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{KOH}(a q) \longrightarrow$

David Collins

Numerade Educator

02:50

Problem 46

Predict the products of each reaction.
(a) $\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{K}(s) \longrightarrow$
(b) $\mathrm{HNO}_{3}(a q)+\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) \longrightarrow$
(c) $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow$

David Collins

Numerade Educator

04:14

Problem 47

Four solutions of unknown HCl concentration are titrated with solutions of $\mathrm{NaOH}$. The following table lists the volume of each unknown HCl solution, the volume of $\mathrm{NaOH}$ solution required to reach the equivalence point, and the concentration of each $\mathrm{NaOH}$ solution. Calculate the concentration (in M) of the unknown HCl solution in each case.
$$\begin{array}{lcl}\hline \text { HCI Volume (mL) } & \text { NaOH Volume (mL) } & \text { [NaOH] (M) } \\\hline \text { (a) } 25.00 \mathrm{~mL} & 28.44 \mathrm{~mL} & 0.1231 \mathrm{M} \\\text { (b) } 15.00 \mathrm{~mL} & 21.22 \mathrm{~mL} & 0.0972 \mathrm{M} \\\text { (c) } 20.00 \mathrm{~mL} & 14.88 \mathrm{~mL} & 0.1178 \mathrm{M} \\
\text { (d) } 5.00 \mathrm{~mL} & 6.88 \mathrm{~mL} & 0.1325 \mathrm{M}\end{array}$$

David Collins

Numerade Educator

04:50

Problem 48

Four solutions of unknown $\mathrm{NaOH}$ concentration are titrated with solutions of $\mathrm{HCl}$. The following table lists the volume of each unknown $\mathrm{NaOH}$ solution, the volume of $\mathrm{HCl}$ solution required to reach the equivalence point, and the concentration of each $\mathrm{HCl}$ solution. Calculate the concentration (in M) of the unknown $\mathrm{NaOH}$ solution in each case.
$$\begin{array}{lcc}\hline \text { NaOH Volume }(\mathrm{mL}) & \text { HCI Volume }(\mathrm{mL}) & {[\mathrm{HCl}](\mathrm{M})} \\\hline \text { (a) } 5.00 \mathrm{~mL} & 9.77 \mathrm{~mL} & 0.1599 \mathrm{M} \\\text { (b) } 15.00 \mathrm{~mL} & 11.34 \mathrm{~mL} & 0.1311 \mathrm{M} \\\text { (c) } 10.00 \mathrm{~mL} & 10.55 \mathrm{~mL} & 0.0889 \mathrm{M} \\\text { (d) } 30.00 \mathrm{~mL} & 36.18 \mathrm{~mL} & 0.1021 \mathrm{M} \\\hline\end{array}$$

David Collins

Numerade Educator

01:36

Problem 49

A $25.00-\mathrm{mL}$ sample of an $\mathrm{H}_{2} \mathrm{SO}_{4}$ solution of unknown concentration is titrated with a $0.1322 \mathrm{M}$ KOH solution. A volume of $41.22 \mathrm{~mL}$ of $\mathrm{KOH}$ is required to reach the equivalence point. What is the concentration of the unknown $\mathrm{H}_{2} \mathrm{SO}_{4}$ solution?

Kratika Bhadauria

Numerade Educator

03:32

Problem 50

A $5.00 \mathrm{~mL}$ sample of an $\mathrm{HClO}_{4}$ solution of unknown concentration is titrated with a $0.025 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$ solution. A volume of $5.68 \mathrm{~mL}$ of the $\mathrm{Sr}(\mathrm{OH})_{2}$ solution was required to reach the equivalence point. What is the concentration of the unknown $\mathrm{HClO}_{4}$ solution?

Adriano Chikande

Numerade Educator

01:32

Problem 51

What volume in milliliters of a 0.121 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a $10.0-\mathrm{mL}$ sample of $0.102 \mathrm{M}$ sulfuric acid?

David Collins

Numerade Educator

04:07

Problem 52

What volume of a $0.125 \mathrm{M} \mathrm{KOH}$ solution is required to reach the equivalence point in the complete titration of a $25.0-\mathrm{mL}$ sample of $0.25 \mathrm{M} \mathrm{HBr} ?$

Sneha Hoysala

Duquesne University

01:17

Problem 53

Classify each acid as strong or weak.
(a) HCl
(b) HF
(c) HBr
(d) $\mathrm{H}_{2} \mathrm{SO}_{3}$

Shazia Naz

Numerade Educator

01:58

Problem 54

Classify each acid as strong or weak.
(a) $\mathrm{H}_{2} \mathrm{SO}_{4}$
(b) $\mathrm{NaHSO}_{3}$
(c) $\mathrm{CH}_{3} \mathrm{COOH}$
(d) $\mathrm{HClO}_{4}$

Tracy Tourville

Numerade Educator

01:44

Problem 55

Determine $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ in each acid solution. If the acid is weak, indicate the value that $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ is less than.
(a) $1.7 \mathrm{M} \mathrm{HBr}$
(b) $1.5 \mathrm{M} \mathrm{HNO}_{3}$
(c) $0.38 \mathrm{M} \mathrm{H}_{2} \mathrm{CO}_{3}$
(d) $1.75 \mathrm{M} \mathrm{HCHO}_{2}$

David Collins

Numerade Educator

01:40

Problem 56

Determine $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ in each acid solution. If the acid is weak, indicate the value that $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ is less than.
(a) $0.5 \mathrm{M} \mathrm{HCl}$
(b) $0.25 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$
(c) $0.11 \mathrm{M} \mathrm{HClO}_{4}$
(d) $0.75 \mathrm{M} \mathrm{HF}$

David Collins

Numerade Educator

Problem 57

Classify each base as strong or weak.
(a) $\mathrm{LiOH}$
(b) $\mathrm{NH}_{4} \mathrm{OH}$
(c) $\mathrm{Ca}(\mathrm{OH})_{2}$
(d) $\mathrm{NH}_{3}$

David Collins

Numerade Educator

Problem 58

Classify each base as strong or weak.
(a) $\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}$
(b) $\mathrm{NaOH}$
(c) $\mathrm{Ba}(\mathrm{OH})_{2}$
(d) KOH

David Collins

Numerade Educator

02:09

Problem 59

Determine $\left[\mathrm{OH}^{-}\right]$ in each base solution. If the acid is weak, indicate the value that $\left[\mathrm{OH}^{-}\right]$ is less than.
(a) $0.25 \mathrm{M} \mathrm{NaOH}$
(b) $0.25 \mathrm{M} \mathrm{NH}_{3}$
(c) $0.25 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$
(d) $1.25 \mathrm{M} \mathrm{KOH}$

David Collins

Numerade Educator

02:09

Problem 60

Determine $\left[\mathrm{OH}^{-}\right]$ in each base solution. If the acid is weak, indicate the value that $\left[\mathrm{OH}^{-}\right]$ is less than.
(a) $0.75 \mathrm{M} \mathrm{KOH}$
(b) $0.5 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}$
(c) $1 \mathrm{MNH}_{3}$
(d) $0.25 \mathrm{M} \mathrm{LiOH}$

David Collins

Numerade Educator

01:39

Problem 61

Determine if each solution is acidic, basic, or neutral.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-5} \mathrm{M} ;\left[\mathrm{OH}^{-}\right]=1 \times 10^{-9} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-6} \mathrm{M} ;\left[\mathrm{OH}^{-}\right]=1 \times 10^{-8} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-7} \mathrm{M} ;\left[\mathrm{OH}^{-}\right]=1 \times 10^{-7} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1 \times 10^{-8} \mathrm{M} ;\left[\mathrm{OH}^{-}\right]=1 \times 10^{-6} \mathrm{M}$

David Collins

Numerade Educator

00:26

Problem 62

Determine if each solution is acidic, basic, or neutral.
(a) $0.25 \mathrm{M} \mathrm{HCl}+0.5 \mathrm{M} \mathrm{NaOH}$
(b) $0.5 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}+0.5 \mathrm{M} \mathrm{KOH}$
(c) $0.25 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}+0.25 \mathrm{M} \mathrm{CaCO}_{3}$
(d) $0.5 \mathrm{M} \mathrm{HCl}+0.5 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}$

Shazia Naz

Numerade Educator

02:05

Problem 63

Calculate [OH $^{-}$ ] given $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ in each aqueous solution and classify the solution as acidic or basic.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.5 \times 10^{-9} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=9.3 \times 10^{-9} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.2 \times 10^{-6} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.4 \times 10^{-4} \mathrm{M}$

David Collins

Numerade Educator

01:59

Problem 64

Calculate $\left[\mathrm{OH}^{-}\right]$ given $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ in each aqueous solution and classify the solution as acidic or basic.
(a) $1 \times 10^{-5} \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$
(b) $1 \times 10^{-5} \mathrm{M} \mathrm{HCl}$
(c) $2 \times 10^{-7} \mathrm{M} \mathrm{HNO}_{3}$
(d) $6 \times 10^{-4} \mathrm{M} \mathrm{HClO}_{4}$

David Collins

Numerade Educator

Problem 65

Calculate $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ given $\left[\mathrm{OH}^{-}\right]$ in each aqueous solution and classify each solution as acidic or basic.
(a) $\left[\mathrm{OH}^{-}\right]=2.7 \times 10^{-12} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=2.5 \times 10^{-2} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=1.1 \times 10^{-10} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=3.3 \times 10^{-4} \mathrm{M}$

David Collins

Numerade Educator

01:59

Problem 66

Calculate $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ given $\left[\mathrm{OH}^{-}\right]$ in each aqueous solution and classify each solution as acidic or basic.
(a) $\left[\mathrm{OH}^{-}\right]=2.1 \times 10^{-7} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=3.6 \times 10^{-5} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=6.2 \times 10^{-11} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=1.4 \times 10^{-2} \mathrm{M}$

David Collins

Numerade Educator

Problem 67

Classify each solution as acidic, basic, or neutral according to its $\mathrm{pH}$ value.
(a) $\mathrm{pH}=8.0$
(b) $\mathrm{pH}=7.0$
(c) $\mathrm{pH}=3.5$
(d) $\mathrm{pH}=6.1$

David Collins

Numerade Educator

01:12

Problem 68

Classify each solution as acidic, basic, or neutral according to its $\mathrm{pH}$ value.
(a) $\mathrm{pH}=4.0$
(b) $\mathrm{pH}=3.5$
(c) $\mathrm{pH}=13.0$
(d) $\mathrm{pH}=0.85$

David Collins

Numerade Educator

Problem 69

Calculate the $\mathrm{pH}$ of each solution.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.7 \times 10^{-8} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.0 \times 10^{-7} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.2 \times 10^{-6} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.4 \times 10^{-4} \mathrm{M}$

David Collins

Numerade Educator

01:33

Problem 70

Calculate the $\mathrm{pH}$ of each solution.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=2.4 \times 10^{-10} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=7.6 \times 10^{-2} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=9.2 \times 10^{-13} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3.4 \times 10^{-5} \mathrm{M}$

David Collins

Numerade Educator

Problem 71

Calculate $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ for each solution.
(a) $\mathrm{pH}=8.55$
(b) $\mathrm{pH}=11.23$
(c) $\mathrm{pH}=2.87$
(d) $\mathrm{pH}=1.22$

David Collins

Numerade Educator

Problem 72

Calculate $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]$ for each solution.
(a) $\mathrm{pH}=8.55$
(b) $\mathrm{pH}=11.23$
(c) $\mathrm{pH}=2.87$
(d) $\mathrm{pH}=1.22$

David Collins

Numerade Educator

01:51

Problem 73

Calculate the $\mathrm{pH}$ of each solution.
(a) $\left[\mathrm{OH}^{-}\right]=1.9 \times 10^{-7} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=2.6 \times 10^{-8} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=7.2 \times 10^{-11} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=9.5 \times 10^{-2} \mathrm{M}$

David Collins

Numerade Educator

01:49

Problem 74

Calculate the $\mathrm{pH}$ of each solution.
(a) $\left[\mathrm{OH}^{-}\right]=2.8 \times 10^{-11} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=9.6 \times 10^{-3} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=3.8 \times 10^{-12} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=6.4 \times 10^{-4} \mathrm{M}$

David Collins

Numerade Educator

Problem 75

Calculate $\left[\mathrm{OH}^{-}\right]$ for each solution.
(a) $\mathrm{pH}=2.2$
(b) $\mathrm{pH}=5.6$
(c) $\mathrm{pH}=7.8$
(d) $\mathrm{pH}=10.1$

David Collins

Numerade Educator

Problem 76

Calculate [OH $^{-}$ ] for each solution.
(a) $\mathrm{pH}=2.2$
(b) $\mathrm{pH}=5.6$
(c) $\mathrm{pH}=7.8$
(d) $\mathrm{pH}=10.1$

David Collins

Numerade Educator

Problem 77

Calculate the $\mathrm{pH}$ of each solution:
(a) $0.001 \mathrm{M} \mathrm{HCl}$
(b) $0.0025 \mathrm{M} \mathrm{LiOH}$
(c) $1.25 \times 10^{-5} \mathrm{MHNO}_{3}$
(d) $2.5 \times 10^{-4} \mathrm{M} \mathrm{KOH}$

David Collins

Numerade Educator

02:36

Problem 78

Calculate the $\mathrm{pH}$ of each solution:
(a) $1.34 \times 10^{-3} \mathrm{M} \mathrm{HClO}_{4}$
(b) $0.0211 \mathrm{M} \mathrm{NaOH}$
(c) $0.0109 \mathrm{M} \mathrm{HBr}$
(d) $7.02 \times 10^{-5} \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$

David Collins

Numerade Educator

Problem 79

Detemine the $\mathrm{pOH}$ of each solution and classify it as acidic, basic, or neutral.
(a) $\left[\mathrm{OH}^{-}\right]=1.5 \times 10^{-9} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=7.0 \times 10^{-5} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=1.0 \times 10^{-7} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=8.8 \times 10^{-3} \mathrm{M}$

David Collins

Numerade Educator

01:21

Problem 80

Detemine the $\mathrm{pOH}$ of each solution and classify it as acidic, basic, or neutral.
(a) $\left[\mathrm{OH}^{-}\right]=4.5 \times 10^{-2} \mathrm{M}$
(b) $\left[\mathrm{OH}^{-}\right]=3.1 \times 10^{-12} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=5.4 \times 10^{-5} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=1.2 \times 10^{-2} \mathrm{M}$

David Collins

Numerade Educator

01:52

Problem 81

Determine the $\mathrm{pOH}$ of each solution.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.2 \times 10^{-8} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=5.5 \times 10^{-2} \mathrm{M}$
(c) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3.9 \times 10^{-9} \mathrm{M}$
(d) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.88 \times 10^{-13} \mathrm{M}$

David Collins

Numerade Educator

01:52

Problem 82

Determine the $\mathrm{pOH}$ of each solution.
(a) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=1.2 \times 10^{-5} \mathrm{M}$
(b) $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=3.7 \times 10^{-11} \mathrm{M}$
(c) $\left[\mathrm{OH}^{-}\right]=2.4 \times 10^{-3} \mathrm{M}$
(d) $\left[\mathrm{OH}^{-}\right]=5.7 \times 10^{-9} \mathrm{M}$

David Collins

Numerade Educator

01:15

Problem 83

Determine the $\mathrm{pH}$ of each solution and classify it as acidic, basic, or neutral.
(a) $\mathrm{pOH}=8.5$
(b) $\mathrm{pOH}=4.2$
(c) $\mathrm{pOH}=1.7$
(d) $\mathrm{pOH}=7.0$

David Collins

Numerade Educator

02:58

Problem 84

Determine the $\mathrm{pH}$ of each solution and classify it as acidic, basic, or neutral.
(a) $\mathrm{pOH}=2.4$
(b) $\mathrm{pOH}=5.5$
(c) $\mathrm{pOH}=7.01$
(d) $\mathrm{pOH}=13.0$

Karoline García

Numerade Educator

01:41

Problem 85

Determine whether or not each mixture is a buffer.
(a) HCl and HF
(b) $\mathrm{NaOH}$ and $\mathrm{NH}_{3}$ 3
(c) HF and NaF
(d) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$ and $\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$

David Collins

Numerade Educator

03:52

Problem 86

Determine whether or not each mixture is a buffer.
(a) $0.5 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}+0.3 \mathrm{M} \mathrm{NaOH}$
(b) $0.25 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}+0.25 \mathrm{M} \mathrm{KOH}$
(c) $0.6 \mathrm{M} \mathrm{CH}_{3} \mathrm{COONa}+0.3 \mathrm{M} \mathrm{HCl}$
(d) $0.3 \mathrm{M} \mathrm{NH}_{3}+0.1 \mathrm{M} \mathrm{HBr}$

Jenna Nikles

Numerade Educator

Problem 87

Write reactions showing how each of the buffers in Problem 85 would neutralize added HCl.

David Collins

Numerade Educator

02:01

Problem 88

What is the $\mathrm{pH}$ of unpolluted, $\mathrm{CO}_{2}$ -saturated rain? Calculate the concentration of $\left[\mathrm{H}_{3} \mathrm{O}\right]^{+}$ in $\mathrm{CO}_{2}$ -saturated rain.

Sima Sarker

Numerade Educator

01:40

Problem 89

What substance could you add to each solution to make it a buffer solution?
(a) $0.100 \mathrm{M} \mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$
(b) $0.500 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}$
(c) $0.200 \mathrm{M} \mathrm{HCHO}_{2}$

David Collins

Numerade Educator

01:22

Problem 90

What substance could you add to each solution to make it a buffer solution?
(a) $0.050 \mathrm{M} \mathrm{NaHSO}_{3}$
(b) $0.150 \mathrm{M}$ HF
(c) $0.200 \mathrm{M} \mathrm{KCHO}_{2}$

David Collins

Numerade Educator

01:22

Problem 91

How much $0.100 \mathrm{M} \mathrm{HCl}$ is required to completely neutralize $20.0 \mathrm{~mL}$ of $0.250 \mathrm{M} \mathrm{NaOH} ?$

David Collins

Numerade Educator

Problem 92

How much $0.250 \mathrm{M} \mathrm{KOH}$ is required to completely neutralize $12.6 \mathrm{~mL}$ of $0.100 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4} ?$

David Collins

Numerade Educator

Problem 93

What is the minimum volume of $1.2 \mathrm{M} \mathrm{HNO}_{3}$ required to completely dissolve $3.2 \mathrm{~g} \mathrm{Na}_{2} \mathrm{O} ?$

David Collins

Numerade Educator

01:41

Problem 94

What is the minimum volume of $3.0 \mathrm{M}$ HBr required to completely dissolve $15.0 \mathrm{~g}$ of potassium metal?

David Collins

Numerade Educator

01:32

Problem 95

When $18.5 \mathrm{~g}$ of $\mathrm{K}_{2} \mathrm{O}(\mathrm{s})$ is completely dissolved by $\mathrm{HI}(a q)$, how many grams of $\mathrm{KI}(a q)$ form in solution?

David Collins

Numerade Educator

01:37

Problem 96

When $5.88 \mathrm{~g}$ of $\mathrm{CaO}(\mathrm{s})$ is completely dissolved by $\mathrm{HBr}(a q)$ how many grams of $\mathrm{CaBr}_{2}(a q)$ form in solution?

David Collins

Numerade Educator

02:48

Problem 97

A 0.125-g sample of a monoprotic acid of unknown molar mass is dissolved in water and titrated with $0.1003 \mathrm{M}$ $\mathrm{NaOH}$. The equivalence point is reached after adding 20.77 $\mathrm{mL}$ of base. What is the molar mass of the unknown acid?

Shazia Naz

Numerade Educator

01:51

Problem 98

A 0.105-g sample of a diprotic acid of unknown molar mass is dissolved in water and titrated with $0.1288 \mathrm{M} \mathrm{NaOH}$. The equivalence point is reached after adding $15.2 \mathrm{~mL}$ of base. What is the molar mass of the unknown acid?

David Collins

Numerade Educator

02:55

Problem 99

People take antacids, such as milk of magnesia, to reduce the discomfort of acid stomach or heartburn. The recommended dose of milk of magnesia is 1 teaspoon, which contains $400 \mathrm{mg}$ of $\mathrm{Mg}(\mathrm{OH})_{2}$. What volume of $\mathrm{HCl}$ solution with a $\mathrm{pH}$ of 1.1 can be neutralized by 1 dose of milk of magnesia? (Assume two significant figures in your calculations.)

Shazia Naz

Numerade Educator

Problem 100

A $25 \mathrm{~mL}$ solution of an unknown acid at a concentration of $1.25 \mathrm{M}$ requires $157 \mathrm{~mL}$ of $0.4 \mathrm{M} \mathrm{NaOH}$ to titrate to its equivalence point. What is the basicity of the acid?

Keenan Mintz

University of Miami