Acid-Base Analysis

Practice Questions

GRE Subject Test: Chemistry › Acid-Base Analysis

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47.0g of nitrous acid, HNO2, is added to 4L of water. What is the resulting pH? $\dpi{100} \small \left (K_{a}=4.1\times 10^{-4} \right )$

NaOH is added to a 500mL of 2M acetic acid. If the pKa value of acetic acid is approximately 4.8, what volume of 2M NaOH must be added so that the pH of the solution is 4.8?

Given the following equilibria, what is the hydroxide ion concentration of a solution containing $0.06\textup{ M}$ $NH_{3}$ ?

$NH_{3}+H_{2}O\rightleftharpoons\ NH_{4}^{+}+OH^{-}$

The $K_{b}$ for $NH_{3}$ is $1.75\times10^{-5}$

is a diprotic acid. Which of the following statements is true about its second half equivalence point?

Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.

Mcat8

What is the approximate pKa of the starting acid?

What is the of a 0.12M solution of that has a pH of 5.1?

Which of the following is true regarding the Henderson-Hasselbalch equation?

I. The pH of the solution is always greater than the pKa of the solution

II. As the ratio of conjugate base to acid increases, the pH increases

III. The hydrogen ion concentration can never equal the acid dissociation constant

Consider the titration curve, in which an acid is treated with aqueous 0.5M NaOH.

Mcat8

The pH at the equivalence point was found to be 8.9. Approximately how many milliliters of 0.5M NaOH were needed to reach equivalence?

Given the following equilibria, what is the hydronium ion concentration of a solution containing $0.025\textup{ M}$ ?

$HOCl(aq)+H_{2}O\rightleftharpoons\ OCl^{-}(aq)+H_{3}O^{+}(aq)$

The $K_{a}$ for is $3.0\times10^{-8}$ .

The Ka for HCN is $\small 6.2*10^{-10}$ .

If there is a solution of 2M HCN, what concentration of NaCN is needed in order for the pH to be 9.2?

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