Question 1

Which of the following statements best describes the dissociation of a strong acid in water?

Accepted Answer

A strong acid completely dissociates in water, resulting in a direct stoichiometric relationship between the initial acid concentration and $[H^+]$.

Question 2

What is the pH of a $0.010\ \mathrm{M}$ solution of hydrochloric acid ($\mathrm{HCl}$), assuming complete dissociation?

Accepted Answer

$\mathrm{pH} = 2.00$

Question 3

A $0.020\ \mathrm{M}$ solution of sodium hydroxide ($\mathrm{NaOH}$) is prepared. What is the pH of the solution at $25^\circ\mathrm{C}$? (Assume complete dissociation and $K_w = 1.0 	imes 10^{-14}$)

Accepted Answer

$\mathrm{pH} = 12.00$

Question 4

Which of the following best explains why strong acids and strong bases are considered strong electrolytes?

Accepted Answer

They conduct electricity because they completely dissociate into ions in water.

Question 5

A laboratory technician accidentally mixes $50.0\ \mathrm{mL}$ of $0.10\ \mathrm{M}$ $\mathrm{HCl}$ with $50.0\ \mathrm{mL}$ of $0.10\ \mathrm{M}$ $\mathrm{NaOH}$. What is the pH of the resulting solution?

Accepted Answer

$\mathrm{pH} = 7.00$

Question 6

Which equation correctly represents the dissociation of a generic strong base $\mathrm{XOH}$ in water?

Accepted Answer

$\mathrm{XOH}(aq) \rightarrow \mathrm{X}^+(aq) + \mathrm{OH}^-(aq)$

Question 7

A $0.0050\ \mathrm{M}$ solution of $\mathrm{KOH}$ is prepared. What is the $[OH^-]$ in the solution?

Accepted Answer

$[OH^-] = 0.0050\ \mathrm{M}$

Question 8

If the $[OH^-]$ in a solution is $1.0 	imes 10^{-3}\ \mathrm{M}$, what is the pH of the solution at $25^\circ\mathrm{C}$?

Accepted Answer

$\mathrm{pH} = 11.00$

Question 9

A student prepares a $0.025\ \mathrm{M}$ solution of $\mathrm{HNO_3}$ (a strong acid). What is the $[H^+]$ in the solution?

Accepted Answer

$[H^+] = 0.025\ \mathrm{M}$

Question 10

Which of the following best describes the relationship between the initial concentration of a strong acid and the $[H^+]$ in solution?

Accepted Answer

The $[H^+]$ is equal to the initial concentration of the strong acid.

Question 11

A $0.0010\ \mathrm{M}$ solution of $\mathrm{Ba(OH)_2}$ is prepared. What is the $[OH^-]$ in the solution, assuming complete dissociation?

Accepted Answer

$[OH^-] = 0.0020\ \mathrm{M}$

Question 12

A patient is given an intravenous solution containing $0.10\ \mathrm{M}$ $\mathrm{NaOH}$. What is the pOH of the solution?

Accepted Answer

$\mathrm{pOH} = 1.00$

Question 13

Which of the following is a correct calculation for the pH of a $0.020\ \mathrm{M}$ $\mathrm{HCl}$ solution?

Accepted Answer

$\mathrm{pH} = -\log(0.020)$

Question 14

A $0.050\ \mathrm{M}$ solution of $\mathrm{HBr}$ (a strong acid) is prepared. What is the pH of the solution?

Accepted Answer

$\mathrm{pH} = 1.30$

Question 15

A $0.020\ \mathrm{M}$ solution of $\mathrm{Ca(OH)_2}$ is prepared. What is the pH of the solution at $25^\circ\mathrm{C}$? (Assume complete dissociation.)

Accepted Answer

$\mathrm{pH} = 12.60$

Question 16

Which of the following best explains why the pH of a strong base solution can be calculated directly from its initial concentration?

Accepted Answer

Because strong bases completely dissociate, so $[OH^-]$ equals the initial base concentration (or a multiple for polyhydroxide bases).

Question 17

A $0.0010\ \mathrm{M}$ solution of $\mathrm{HClO_4}$ (a strong acid) is prepared. What is the pH of the solution?

Accepted Answer

$\mathrm{pH} = 3.00$

Question 18

A $0.0050\ \mathrm{M}$ solution of $\mathrm{LiOH}$ is prepared. What is the pOH of the solution?

Accepted Answer

$\mathrm{pOH} = 2.30$

Question 19

A $0.020\ \mathrm{M}$ solution of $\mathrm{NaOH}$ is accidentally spilled into a river. If the river has a neutral pH of 7.00 before the spill, what is the expected effect on the river's pH?

Accepted Answer

The pH will increase, making the river more basic.

Strong Acid and Strong Base pH Calculations

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