Q: Which of the following is the correct Henderson-Hasselbalch equation?

$$\mathrm{pH} = pK_a + \log\left(\frac{[\text{base}]}{[\text{acid}]}\right)$$

Q: Which of the following is the correct expression for the solubility product constant ($$K_{sp}) $$for CaF$$_2$$?

$$K_{sp} = [\text{Ca}^{2+}][\text{F}^-]^2$$

Question 1

Which of the following statements best describes a Bronsted-Lowry acid?

Accepted Answer

A substance that donates a proton (H$$^+) to $$another substance.

Question 2

Which of the following pairs are conjugate acid-base pairs?

Accepted Answer

NH$$_3$$ and NH$$_4^+$$

Question 3

What is the pH of a solution with a hydronium ion concentration of $$1.0 	imes 10$$^{-4}$$ M?

Accepted Answer

$$\mathrm{pH} = 4$$

Question 4

Which of the following is NOT one of the seven strong acids?

Accepted Answer

HF

Question 5

A weak acid, HA, has a $$K_a = 1.8 	imes 10$$^{-5}$$. What is its pK_a$?

Accepted Answer

$$pK_a = 4.74$$

Question 6

Which of the following salts will produce a basic solution when dissolved in water?

Accepted Answer

NaNO$$_2$$

Question 7

Which of the following best describes the function of a buffer?

Accepted Answer

It maintains a constant pH by neutralizing added acids or bases.

Question 8

A buffer is made by mixing 0.20 mol of acetic acid and 0.10 mol of sodium acetate in 1.0 L of solution. What is the pH? ($$K_a$$ for acetic acid = $$1.8 	imes 10$$^{-5}$$)

Accepted Answer

$$\mathrm{pH} = 4.44 + \log(0.10/0.20)$$

Question 9

Which of the following is the correct Henderson-Hasselbalch equation?

Accepted Answer

$$\mathrm{pH} = pK_a + \log\left(\frac{[	ext{base}]}{[	ext{acid}]}ight)$$

Question 10

Which of the following best explains the common ion effect?

Accepted Answer

The addition of an ion common to an equilibrium shifts the position of equilibrium to reduce the concentration of that ion.

Question 11

A solution is prepared by dissolving 0.10 mol of NaF in 1.0 L of 0.10 M HF. What will happen to the pH compared to pure 0.10 M HF?

Accepted Answer

The pH will increase.

Question 12

Which of the following best describes the equivalence point in a titration?

Accepted Answer

The point where the amount of acid equals the amount of base in moles.

Question 13

Which indicator would be most appropriate for the titration of a strong acid with a strong base?

Accepted Answer

Phenolphthalein (pH range 8.2–10.0)

Question 14

Which of the following is the correct expression for the solubility product constant ($$K_{sp}) $$for CaF$$_2$$?

Accepted Answer

$$K_{sp} = [	ext{Ca}^{2+}][	ext{F}^-]^2$$

Question 15

If the $$K_{sp} of $$AgCl is $$1.8 	imes 10$$^{-10}$$, what is the molar solubility of AgCl in pure water?

Accepted Answer

$$1.3 	imes 10$$^{-5}$$ M

Question 16

Which of the following will increase the solubility of CaF$$_2 in $$water?

Accepted Answer

Decreasing the pH

Question 17

A solution is saturated with respect to PbI$$_2. If $$more KI is added, what will happen?

Accepted Answer

PbI$$_2$$ will precipitate.

Question 18

Which of the following best explains why blood is able to resist changes in pH?

Accepted Answer

Blood contains a buffer system composed of H$$_2CO$_3$$ and HCO$$_3^-.$$

Question 19

Which of the following statements about the titration curve of a weak acid with a strong base is correct?

Accepted Answer

The buffer region occurs before the equivalence point.

Acids, Bases, and Aqueous Ionic Equilibria: Study Guide

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