Acids and Bases and Equilibrium

Write a balanced equation for the neutralization of each of the following:

a. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right) and \mathrm{NaOH}\left(aq\right)$

b. $\mathrm{HI}\left(aq\right) and \mathrm{LiOH}\left(aq\right)$

c. ${\mathrm{HNO}}_3\left(aq\right) and \mathrm{Ca}\left(\mathrm{OH}{)}_2\right(s)$

Balance each of the following neutralization equations:

a. ${\mathrm{HNO}}_3\left(aq\right)+\mathrm{Ba}\left(\mathrm{OH}{)}_2\right(s)⟶{\mathrm{H}}_2\mathrm{O}(l)+\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2(aq)$

b. ${\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right)+\mathrm{Al}\left(\mathrm{OH}{)}_3\right(s)⟶{\mathrm{H}}_2\mathrm{O}(l)+{\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3(aq)$

If $38.2 \mathrm{mL}$ of a $0.163\mathrm{M} \mathrm{KOH}$ solution is required to titrate $25.0 \mathrm{mL}$ of a solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$, what is the molarity of the ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution$?$

${\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right)+2\mathrm{NaOH}\left(aq\right)⟶2{\mathrm{H}}_2\mathrm{O}\left(l\right)+{\mathrm{Na}}_2{\mathrm{SO}}_4\left(aq\right)$

What is the molarity of an acetic acid solution if $25.0 \mathrm{mL}$  of the ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$ solution is titrated with $29.7 \mathrm{mL}$ of a $0.205\mathrm{M}$ $\mathrm{KOH}$ solution$?$

${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2\left(aq\right)+\mathrm{KOH}\left(aq\right)⟶{\mathrm{H}}_2\mathrm{O}\left(l\right)+{\mathrm{KC}}_2{\mathrm{H}}_3{\mathrm{O}}_2\left(aq\right)$

Balance each of the following neutralization equations:

a. $\mathrm{HCl}\left(aq\right)+\mathrm{Mg}\left(\mathrm{OH}{)}_2\right(s)⟶{\mathrm{H}}_2\mathrm{O}(l)+{\mathrm{MgCl}}_2(aq)$

b. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right)+\mathrm{LiOH}\left(aq\right)⟶{\mathrm{H}}_2\mathrm{O}\left(l\right)+{\mathrm{Li}}_3{\mathrm{PO}}_4\left(aq\right)$

Complete and balance the equation for each of the following reactions:

a.  ${\mathrm{ZnCO}}_3\left(s\right)+\mathrm{HBr}\left(aq\right)⟶$

b.  $\mathrm{Zn}\left(s\right)+\mathrm{HCl}\left(aq\right)⟶$

c.  $\mathrm{HCl}\left(aq\right)+{\mathrm{NaHCO}}_3\left(s\right)⟶$

d.  ${\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right)+\mathrm{Mg}\left(\mathrm{OH}{)}_2\right(s)⟶$

Which of the following represents a buffer system? Explain.

a. $\mathrm{NaOH}$ and $\mathrm{NaCl}$

b.  ${\mathrm{H}}_2{\mathrm{CO}}_3$ and ${\mathrm{NaHCO}}_3$

c.  $\mathrm{HF}$ and $KF$

d. $\mathrm{KCl}$ and $\mathrm{NaCl}$

Which of the following represents a buffer system? Explain.

a. $H_{3}P{O}_3$

b. ${\mathrm{NaNO}}_3$

c. ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2\text{ and }{\mathrm{NaC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$

d. $\mathrm{HCl}\text{ and }\mathrm{NaOH}$

Consider the buffer system of hydrofluoric acid, HF, and its salt, NaF .

$\mathrm{HF}\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)+{\mathrm{F}}^{-}\left(aq\right)$

a. The purpose of this buffer system is to:

            1. maintain [HF]

            2. maintain $\left[{\mathrm{F}}^{-}\right]$

            3. maintain $\mathrm{pH}$

b. The salt of the weak acid is needed to:

            1. provide the conjugate base

            2. neutralize added ${\mathrm{H}}_3{\mathrm{O}}^{+}$

            3. provide the conjugate acid

c. If ${\mathrm{OH}}^{-}$is added, it is neutralized by:

             1. the salt

             2. ${\mathrm{H}}_2\mathrm{O}$

             3. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

d.  When${\mathrm{H}}_3{\mathrm{O}}^{+}$is  added, the equilibrium shifts in the direction of the:

             1. reactants

             2. products

             3. does not change

Consider the buffer system of nitrous acid, ${\mathrm{HNO}}_2$, and its salt, ${\mathrm{NaNO}}_2$.

${\mathrm{HNO}}_2\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)+{\mathrm{NO}}_2^{-}\left(aq\right)$

a.   The purpose of this buffer system is to:

             1. maintain $\left[{\mathrm{HNO}}_2\right]$

             2. maintain $\left[{{\mathrm{NO}}_2}^{-}\right]$

             3. maintain $\mathrm{pH}$

b.  The weak acid is needed to:

             1. provide the conjugate base

             2. neutralize added ${\mathrm{OH}}^{-}$

             3. provide the conjugate acid

c.  If ${\mathrm{H}}_3{\mathrm{O}}^{+}$is added, it is neutralized by:

             1. the salt

             2. ${\mathrm{H}}_2\mathrm{O}$

             3. ${\mathrm{OH}}^{-}$

d. When ${\mathrm{OH}}^{-}$is added, the equilibrium shifts in the direction of the:

             1. reactants

             2. products

             3. does not change

Why would the pH of your blood plasma increase if you breathe fast?

Why would the pH of your blood plasma decrease if you hold your breath?

Someone with severe diabetes obtains energy by the breakdown of fats, which produce large amounts of acidic substances. How would this affect the $pH$ of the blood plasma?

Someone with kidney failure excretes urine with large amounts of${\mathrm{HCO}}_3^{-}$. How would this loss of ${\mathrm{HCO}}_3^{-}$affect the $\mathrm{pH}$ of the blood plasma?

At rest, the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ of the stomach fluid is $2.0\times {10}^{-4}\mathrm{M}$̣ What is the pH of the stomach fluid.

In Larry's esophagal pH test, a pH value of 3.60 was recorded in the esophagus. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ in his esophagus?

Write the balanced chemical equation for the neutralization reaction of stomach acid HCL with Al(OH)3, an ingredient in some antacids.

How many grams of $CaC{O}_3$ are required to neutralize 100mL of stomach acid, which is equivalent to 0.0400 M HCL?

Write the balanced chemical equation for the neutralization reaction of stomach acid HCL with $CaC{O}_3$ an ingredient in some antacids.

At rest, the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$of the stomach fluid is $2.0\times {10}^{-4}\mathrm{M}$. What is the $\mathrm{pH}$ of the stomach fluid?

In Larry's esophageal pH  test, a pH value of  3.60 was recorded in the esophagus. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$in his esophagus?

After Larry had taken Nexium for 4 weeks, the $\mathrm{pH}$ in his stomach was raised to 4.52. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$in his stomach?

When food enters the stomach,$\mathrm{HCl}$ is released and the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ of the stomach fluid rises to $4\times {10}^{-2}\mathrm{M}$. What is the $\mathrm{pH}$ of the stomach fluid?

How many grams of  ALOH), are required to neutralize 150, mL of stomach acid with a pH of $1.5$ ?

State whether each of the following is acidic, basic, or neutral:

a. blood plasma. pH $1 7.38$

b. vinegar, $\mathrm{pH} 2.8$

c. drain cleaner $pH 11.2$

d. coffee, $pH 5.52$

e. tomatoes, $pH 4.2$

f. chocolate cake, $pH 7.6$

State whether each of the following is acidic, basic, or neutral:

a. soda $pH 13.22$

b. shampoo, $pH 5.7$

c. laundry detergent, $pH 9.44$

d. rain $pH 5.8$

e. honey, $pH 3.9$

f. cheese, $\mathrm{pH} 4.9$

Complete the following table-

State whether each of the following solutions is acidic, basic. or neutral: (10.6)

a. rain, pH $5.2$

b. tears, pH$7.5$

c. tea, pH$3.8$

d. cola, pH $2.5$

e. photo developer, $\mathrm{pH}12.0$

Identify each of the following as an acid or a base: (10.1)

a. ${\mathrm{H}}_2{\mathrm{SO}}_4$

b.$\mathrm{RbOH}$

c.$\mathrm{Ca}(\mathrm{OH}{)}_2$

d.$\mathrm{HI}$

Identify each of the following as an acid or a base; (10.1)

A. $\mathrm{Sr}(\mathrm{OH}{)}_2$$\mathrm{Sr}(\mathrm{OH}{)}_2$

B. ${\mathrm{H}}_2{\mathrm{SO}}_3$

C. ${\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$

D. $\mathrm{CsOH}$

State whether each of the following solutions is acidic, basic, or neutral: (10.6)

a. saliva, pH 6.8

b. urine, pH 5.9

c. pancreatic juice, pH 8.0

d. bile, pH 8.4

e. blood, pH 7.45

Identify the stronger acid in each of the following pairs: (10.3)

a. HF or HCN

b. ${\mathrm{H}}_3{\mathrm{O}}^{+}\text{or }{\mathrm{H}}_2\mathrm{S}$

c. ${\mathrm{HNO}}_2\text{ or }{\mathrm{HC}}_2{\mathrm{H}}_3{\mathrm{O}}_2$

d. ${\mathrm{H}}_2\mathrm{O}\text{ or }{\mathrm{HCO}}_3^{-}$

Identify the weaker acid in each of the following pairs: 

a. ${\mathrm{HNO}}_2$ and ${\mathrm{H}}_2{\mathrm{CO}}_3$

b. HF or $HC{O_3}^{-}$

c. $\mathrm{HBr} \mathrm{or} {\mathrm{HSO}}_4^{-}$

d. ${\mathrm{NH}}_4^{+} or {\mathrm{H}}_3{\mathrm{PO}}_4$

Use Le Châtelier's principle to predict if each of the following changes causes the system to shift in the direction of products or reactants: 

${\mathrm{H}}_2\mathrm{S}\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)+{\mathrm{HS}}^{-}\left(aq\right)$

a. adding more ${\mathrm{H}}_2\mathrm{S}\left(aq\right)$

b. removing some ${\mathrm{HS}}^{-}\left(aq\right)$

c. adding more ${\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

d. removing some ${\mathrm{H}}_2\mathrm{S}\left(aq\right)$

Use Le Châtelier's principle to predict if each of the following changes causes the system to shift in the direction of products or reactants:

$\mathrm{HClO}\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)+{\mathrm{ClO}}^{-}\left(aq\right)$

a. removing some $\mathrm{HClO}\left(aq\right)$

b. adding more ${\mathrm{ClO}}^{-}\left(aq\right)$

c. removing some ${\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

d. adding more $\mathrm{HClO}\left(aq\right)$

Determine the pH for the following solutions:

a. $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=1.0\times {10}^{-11}\mathrm{M}$

b. $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=5.0\times {10}^{-2}\mathrm{M}$

c. $\left[{\mathrm{OH}}^{-}\right]=3.5\times {10}^{-4}\mathrm{M}$

d. $\left[{\mathrm{OH}}^{-}\right]=0.005\mathrm{M}$

Determine the pH for the following solutions:

a.$\left[{\mathrm{OH}}^{-}\right]=1.0\times {10}^{-7}\mathrm{M}$

b.$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=4.2\times {10}^{-3}\mathrm{M}$

c.$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=0.0001\mathrm{M}$

d.$\left[{\mathrm{OH}}^{-}\right]=8.5\times {10}^{-9}\mathrm{M}$

Identify each of the solutions in problem 10.87 as acidic, basic, or neutral. 

Identify each of the solutions in problem 10.88 as acidic, basic, or neutral. 

Determine if each of the following diagrams represents a strong acid or a weak acid. The acid has the formula HX. (10.3)

Adding a few drops of a strong acid io water will lower the phi appreciably. However, adding the same number of drags to a buffer does not appreciably alter the ph. Why? (10.8)

Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting. (10.8)

a. What changes occur in the blood $\mathrm{pH}$ during hyperventilation?

h. How does breathing into a paper bag help return blood pH to normal??

In the blood plasma. pH is maintained by the carbonic acid bicarbonate buffer system, $(10,8)$

a. How is pH maintained when acid is added to the buffer system?

b. How is pH maintained when base is added to the buffer system?

Determine the pH for the follow ing solutions: $(10,6)$

a. $\left[\mathrm{OH}\right]=1.0\times {10}^{-7}\mathrm{M}$

b.$\left[{\mathrm{H}}_2{\mathrm{O}}^{\text{'}}\right]=4.2\times {10}^{-3}\mathrm{M}$

c. $\left[{\mathrm{H}}_2{\mathrm{O}}^{+}\right]=0.0001\mathrm{M}$

d. $\left[\mathrm{OH}\right]=8.5\times {10}^{-9}\mathrm{M}$

Calculate the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]\text{and }\left[{\mathrm{OH}}^{-}\right]$ for a solution with the following pH values:

a. 3.40

b. 6.00

c. 8.0

d. 11.0

e. 9.20

Calculate the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]and\left[{\mathrm{OH}}^{-}\right]$ for a solution with the following pH values:

a. 10.0

b. 5.0

c. 7.00

d. 6.5

Solution X has a pH of 9.0, and solution Y has a pH of 7.0.

a. Which solution is more acidic?

b. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ in each?

c. What is the $O{H}^{-}$ in each?

Calculate the volume, in millilitres, of a 0.215 M KOH solution that will completely neutralize each of the following: 

a. 2.50 mL of a $0.825 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution

b. 18.5 mL of a $0.560 \mathrm{M} {\mathrm{HNO}}_3$ solution

c. 5.00 mL of a $3.18 \mathrm{M} \mathrm{HCl}$ solution

A buffer solution is made by dissolving ${\mathrm{H}}_3{\mathrm{PO}}_4\text{ and }{\mathrm{NaH}}_2{\mathrm{PO}}_4$ in water.

a. Write an equation that shows how this buffer neutralizes added acid.

b. Write an equation that shows how this buffer neutralizes added base.