Acids and Bases and Equilibrium

Calculate the $\left[O{H}^{-}\right]$ of each aqueous solution with the following $\left[H_3{O}^{+}\right]$:

a. oven cleaner, $1.0\times {10}^{-12}M$

b. milk of magnesia, $1.0\times {10}^{-9}M$

c. aspirin, $6.0\times {10}^{-4}M$

d. pancreatic juice, $4.0\times {10}^{-9}M$

Calculate the $\left[H_3{O}^{+}\right]$ of each aqueous solution with the following $\left[O{H}^{-}\right]$:

a. stomach acid, $2.5\times {10}^{-13}M$

b. urine, $2.0\times {10}^{-9}M$

c. orange juice, $5.0\times {10}^{-11}M$

d. bile, $2.5\times {10}^{-6}M$

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

a. $\left[H_3{O}^{+}\right]=6.0\times {10}^{-12}M$

b. $\left[H_3{O}^{+}\right]=1.4\times {10}^{-4}M$

c. $\left[O{H}^{-}\right]=5.0\times {10}^{-12}M$

d. $\left[O{H}^{-}\right]=4.5\times {10}^{-2}M$

Calculate the $\left[O{H}^{-}\right]$ of each aqueous solution with the following $\left[H_3{O}^{+}\right]$:

a. coffee, $1.0\times {10}^{-5}M$

b. soap, $1.0\times {10}^{-8}M$

c. cleanser, $5.0\times {10}^{-10}M$

d. lemon juice, $2.5\times {10}^{-2}M$

Calculate the $\left[H_3{O}^{+}\right]$ of each aqueous solution with the following $\left[O{H}^{-}\right]$:

a. baking soda, $1.0\times {10}^{-6}M$

b. blood, $2.5\times {10}^{-7}M$

c. milk, $4.0\times {10}^{-7}M$

d. bleach, $2.1\times {10}^{-3}M$

Indicate whether each of the following statements is characteristic of an acid, a base, or both:

a. has a sour taste

b. neutralizes bases

c. produces $H^{+}$ ions in water

d. is named barium hydroxide

e. is an electrolyte

Indicate whether each of the following statements is characteristic of an acid, a base, or both:

a. neutralizes acids

b. produces $O{H}^{-}$ ions in water

c. has a slippery feel

d. conducts an electrical current in solution

e. turns litmus red

Write formulas for each of the following acids and bases:

a. rubidium hydroxide

b. hydrofluoric acid

c. phosphoric acid

d. lithium hydroxide

e. ammonium hydroxide

f. periodic acid

Write formulas for each of the following acids and bases:

a. barium hydroxide

b. hydroiodic acid

c. bromic acid

d. strontium hydroxide

e. acetic acid

f. hypochlorous acid

Name each of the following acids or bases:

a.$\mathrm{Hcl}$

b.$\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$

c.${\mathrm{HclO}}_4$

d.${\mathrm{HNO}}_3$

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

f.${\mathrm{HBrO}}_2$

Name each of the following acids or bases:

a. $\mathrm{Al}(\mathrm{OH}{)}_3$

b. $\mathrm{HBr}$

c. ${\mathrm{H}}_2{\mathrm{SO}}_4$

d. $\mathrm{KOH}$

e. ${\mathrm{HNO}}_2$

f. ${\mathrm{HClO}}_2$

1. Write the formula for the conjugate acid for each of the following bases:

a.${\mathrm{CO}}_3^{2-}$  

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

c. ${\mathrm{H}}_2{\mathrm{PO}}_4^{-}$

d. ${\mathrm{Br}}^{-}$

Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following:

a. $\mathrm{HI}\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)⟶{\mathrm{I}}^{-}\left(aq\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

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

Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following:

a. ${\mathrm{CO}}_3{}^{2-}(aq)+{\mathrm{H}}_2\mathrm{O}(l)\rightleftarrows {\mathrm{HCO}}_3{}^{-}(aq)+{\mathrm{OH}}^{-}\left(aq\right)$

b. ${\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)⟶{\mathrm{HSO}}_4^{-}\left(aq\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

Write the formula for the conjugate base for each of the following acids:

a. $\mathrm{HF}$

b. ${\mathrm{H}}_2\mathrm{O}$

c. ${\mathrm{H}}_2{\mathrm{PO}}_3^{-}$

d. ${\mathrm{HSO}}_4^{-}$

Write the formula for the conjugate base for each of the following acids:

a. ${\mathrm{HCO}}_3$

b. ${\mathrm{CH}}_3{{\mathrm{NH}}_3}^{+}$

c. ${\mathrm{HPO}}_4^{2-}$

d. ${\mathrm{HNO}}_2$

Identify the Bronsted-Lowry acid-base pairs in each of the following equations:

a. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(aq\right)+{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)$

b. ${\mathrm{CO}}_3{}^{2-}(aq)+{\mathrm{H}}_2\mathrm{O}(l)\rightleftarrows {\mathrm{HCO}}_3^{-}(aq)+{\mathrm{OH}}^{-}(aq)$

c. ${\mathrm{H}}_3{\mathrm{PO}}_4\left(aq\right)+{\mathrm{NH}}_3\left(aq\right)\rightleftarrows {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(aq\right)+{\mathrm{NH}}_4^{+}\left(aq\right)$

Write the formula for the conjugate acid for each of the following bases:

a.${\mathrm{SO}}_4^{2-}$

b. $C{N}^{-}$

c. $N{H}_3$

d. $Cl{O}_2^{-}$

Identify the Brønsted-Lowry acid-base pairs in each of the following equations:

$$\begin{gathered} a) H_{2}C{O}_3(aq)+H_{2}O(l)\rightleftarrows HC{O}_3^{-}(aq)+H_3{O}^{+}(aq\left) \\ b\right) N{H}_3^{+}\left(aq\right)+H_{2}O\left(l\right)\rightleftarrows N{H}_3\left(aq\right)+H_3{O}^{+}\left(aq\right) \\ c) HCN(aq)+N{O}_2^{-}(aq)\rightleftarrows C{N}^{-}(aq)+HN{O}_2(aq) \end{gathered}$$

Identify the weaker acid in each of the following pairs: 

a. $\mathrm{HCl} \mathrm{or} {{\mathrm{HSO}}_4}^{-}$

b. ${\mathrm{HNO}}_2 \mathrm{or} \mathrm{HF}$

c. ${{\mathrm{HCO}}_3}^{- }\mathrm{or} {{\mathrm{NH}}_4}^{+}$

Using Table 103, identify the stronger acid in each of the following pairs:

a. ${\mathrm{NH}}_4^{+}$or ${\mathrm{H}}_3{\mathrm{O}}^{+}$

b. ${\mathrm{H}}_2{\mathrm{SO}}_4$ or $\mathrm{HCN}$

c. ${\mathrm{H}}_2\mathrm{O}$ or ${\mathrm{H}}_2{\mathrm{CO}}_3$

Identify the weaker acid in each of the following pairs:

a. $\mathrm{HCl}$ or ${{\mathrm{HSO}}_4}^{-}$

b. ${\mathrm{HNO}}_2$ or $\mathrm{HF}$

c. ${\mathrm{HCO}}_3^{-}$or ${{\mathrm{NH}}_4}^{+}$

Identify the weaker acid in each of the following pairs:

a. ${\mathrm{HNO}}_3$ or ${\mathrm{HCO}}_3^{-}$

b. ${\mathrm{HSO}}_4^{-}$or ${\mathrm{H}}_2\mathrm{O}$

c. ${\mathrm{H}}_2{\mathrm{SO}}_4$ or ${\mathrm{H}}_2{\mathrm{CO}}_3$

Using Table $10.3$, identify the stronger acid in each of the following pairs:

a. $\mathrm{HBr}$ or ${\mathrm{HNO}}_2$

b. ${\mathrm{H}}_3{\mathrm{PO}}_4$ or ${\mathrm{HSO}}_4^{-}$

c. $\mathrm{HCN}$ or ${\mathrm{H}}_2{\mathrm{CO}}_3$

Which of the following are at equilibrium?

a. The rate of the forward reaction is twice as fast as the rate of the reverse reaction.

b. The concentrations of the reactants and the products do not change.

c. The rate of the reverse reaction does not change.

Which of the following are not at equilibrium?

a. The rates of the forward and reverse reactions are equal.

b. The rate of the forward reaction does not change.

c. The concentrations of reactants and the products are not constant.

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

$HN{O}_2\left(aq\right)+H_{2}O\left(l\right)\rightleftarrows CH{O}_2^{-}\left(aq\right)+H_{3}O\left(aq\right)$

a. adding more ${\mathrm{CHO}}_2^{-}$

b. removing some ${\mathrm{HCHO}}_2$

c. removing some ${\mathrm{H}}_3{\mathrm{O}}^{+}$

d. adding more ${\mathrm{HCHO}}_2$

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

$HN{O}_2\left(aq\right)+H_{2}O\left(l\right)\rightleftarrows N{O}_2^{-}\left(aq\right)+H_3{O}^{+}\left(aq\right)$

a. adding more $HN{O}_2\left(aq\right)$

b. removing some $N{O}_2^{-}\left(aq\right)$

c. adding more $H_3{O}^{+}\left(aq\right)$

d. removing some $HN{O}_2\left(aq\right)$ 

What is meant by the term reversible reaction?

When does a reversible reaction reach equilibrium?

Calculate the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ of each aqueous solution with the following $\left[{\mathrm{OH}}^{-}\right]$:

a. baking soda, $1.0\times {10}^{-6 }\mathrm{M}$

b. blood, $2.5\times {10}^{-7} \mathrm{M}$

c. milk, $4.0\times {10}^{-7} \mathrm{M}$

d. bleach, $2.1\times {10}^{-5} \mathrm{M}$

10.25 Why are the concentrations of ${\mathrm{H}}_3{\mathrm{O}}^{+}$ and ${\mathrm{OH}}^{-}$equal in pure water?

What is the meaning and value of $K_{\mathrm{w}}$ ?

In an acidic solution, how does the concentration of ${\mathrm{H}}_3{\mathrm{O}}^{+}$ compare to the concentration of ${\mathrm{OH}}^{-}$?

If a base is added to pure water, why does the $H_3{O}^{+}$ decrease?

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

a. $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=2.0\times {10}^{-5}\mathrm{M}$

b. $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=1.4\times {10}^{-9}\mathrm{M}$

c. $\left[{\mathrm{OH}}^{-}\right]=8.0\times {10}^{-3}\mathrm{M}$

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

A patient with respiratory alkalosis has a blood plasma pH of 7.58. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ pf the blood plasma?

Why does a neutral solution have a pH of $7.0$?

If you know the $\left[{\mathrm{OH}}^{-}\right]$, how can you determine the pH of a solution?

Calculate the pH of each solution given the follow in:

a. $\left|{\mathrm{H}}_2{\mathrm{O}}^{+}\right|=1\times {10}^4\mathrm{M}$

b. $\left|\mathrm{H},{\mathrm{O}}^{+}\right|=3\times {10}^{-9}\mathrm{M}$

c.$\left[\mathrm{OH}\right]=1\times {10}^{-9}\mathrm{M}$

d. $\lfloor \mathrm{OH}\rfloor =2.5\times {10}^{-11}\mathrm{M}$

e.$\left|\mathrm{H},{\mathrm{O}}^{\text{'}}\right|=6.7\times {10}^{-1}\mathrm{M}$

f. $\left[{\mathrm{OH}}^{-}\right]=8.2\times {10}^{-4}\mathrm{M}$

Calculate the $\mathrm{pH}$ of each solution given the following:

a. $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=1\times {10}^{-8}\mathrm{M}$

b. $\left|{\mathrm{H}}_3{\mathrm{O}}^{+}\right|=5\times {10}^{-6}\mathrm{M}$

c. $\left[{\mathrm{OH}}^{-}\right]=1\times {10}^{-2}\mathrm{M}$

d. $\left[{\mathrm{OH}}^{-}\right]=8.0\times {10}^{-1}\mathrm{M}$

e.$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]=4.7\times {10}^{-2}\mathrm{M}$

f. $\left[{\mathrm{OH}}^{-}\right]=3.9\times {10}^{-6}\mathrm{M}$

Complete the following table:

Complete the following table :

A patient with severe metabolic acidosis has a blood plasma $\mathrm{pH}$ of $6.92$. What is the $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$of the blood plasma?

A patient with respiratory alkalosis has a blood plasma pH of $7.58$. What is the ${\mathrm{H}}_3{\mathrm{O}}^{+}$ of the blood plasma?

If $32.8 \mathrm{mL}$ of a $0.162\mathrm{M} \mathrm{NaOH}$ 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?

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

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

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

What is the molarity of a solution of HCL if 5ml of the HCL solution is titrated with 28.6ml of a 0.145 M NaOH solution?

$\mathrm{HCl}\left(aq\right)+\mathrm{NaOH}\left(aq\right)⟶{\mathrm{H}}_2\mathrm{O}\left(l\right)+\mathrm{NaCl}\left(aq\right)$

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

a.${\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right) \text{and }\mathrm{NaOH}\left(aq\right)$

b. $\mathrm{HCl}\left(aq\right) \text{and }\mathrm{Fe}\left(\mathrm{OH}{)}_3\right(s)$

c.${\mathrm{H}}_2{\mathrm{CO}}_3\left(aq\right) and \mathrm{Mg}\left(\mathrm{OH}{)}_2\right(s)$