Q: A buffer solution is made by mixing acetic acid and sodium acetate. Which equation can be used to calculate the pH of this buffer?

$$\mathrm{pH} = \mathrm{p}K_a + \log \dfrac{[\text{A}^-]}{[\text{HA}]}$$

Question 1

A hospital pharmacist needs to prepare an intravenous solution that is isotonic with blood plasma. Which colligative property is most relevant for ensuring the solution is safe for injection?

Accepted Answer

Osmotic pressure

Question 2

Which of the following best describes the effect of adding a nonvolatile solute to a solvent on the vapor pressure of the solution?

Accepted Answer

The vapor pressure decreases because the solute particles block solvent evaporation.

Question 3

A student dissolves 0.5 mol of NaCl in 1.0 kg of water. Given that NaCl dissociates completely, what is the expected van't Hoff factor ($$i) $$for this solution?

Accepted Answer

$$i = 2$$

Question 4

Which equation correctly relates the change in boiling point ($$\Delta T_b) to $$the molality ($$m) of a $$solution?

Accepted Answer

$$\Delta T_b = i K_b m$$

Question 5

A reaction has an activation energy of $$50\ \mathrm{kJ/mol}. If $$the temperature is increased, what happens to the rate constant $$k$$ according to the Arrhenius equation?

Accepted Answer

The rate constant increases.

Question 6

Which of the following statements about catalysts is correct?

Accepted Answer

Catalysts provide an alternative pathway with lower activation energy.

Question 7

A chemical reaction is exothermic and has a negative entropy change ($$\Delta S \u003c 0). $$Under what temperature conditions will this reaction be spontaneous?

Accepted Answer

At low temperatures

Question 8

Which of the following best describes the second law of thermodynamics?

Accepted Answer

The entropy of the universe increases in a spontaneous process.

Question 9

A solution is prepared by mixing 100 mL of 0.1 M HCl with 100 mL of 0.1 M NaOH. What is the pH of the resulting solution?

Accepted Answer

pH = 7

Question 10

Which of the following is the correct expression for the equilibrium constant $$K_c$$ for the reaction $$\mathrm{N_2$}(g) + 3\mathrm{H_2$}(g) \rightleftharpoons 2\mathrm{NH_3$}(g)$$?

Accepted Answer

$$K_c = \dfrac{[\mathrm{NH_3$}]^2}{[\mathrm{N_2$}][\mathrm{H_2$}]^3}$$

Question 11

A buffer solution is made by mixing acetic acid and sodium acetate. Which equation can be used to calculate the pH of this buffer?

Accepted Answer

$$\mathrm{pH} = \mathrm{p}K_a + \log \dfrac{[	ext{A}^-]}{[	ext{HA}]}$$

Question 12

Which of the following best explains why salt is spread on icy roads in winter?

Accepted Answer

Salt lowers the freezing point of water, causing ice to melt at lower temperatures.

Question 13

Which of the following is the correct Nernst equation for the cell potential at non-standard conditions?

Accepted Answer

$$E = E^\circ - \dfrac{0.0592}{n} \log Q$$

Question 14

A solution contains $$0.10\ \mathrm{M}$$ $$\mathrm{Ca$$^{2+}$$}$$ and $$0.10\ \mathrm{M}$$ $$\mathrm{SO_4$^{2-}}. $$The $$K_{sp}$$ for $$\mathrm{$$CaSO_4$$} is$$ $$2.4 	imes 10$$^{-5}$$. Will a precipitate form?

Accepted Answer

Yes, because $$Q \u003e K_{sp}$$

Question 15

Which of the following best describes a strong acid?

Accepted Answer

A strong acid has a high $$K_a$$ value and ionizes completely in water.

Question 16

Which of the following is the correct relationship between Gibbs free energy change ($$\Delta G) $$and the equilibrium constant ($$K$$)?

Accepted Answer

$$\Delta G = -RT \ln K$$

Question 17

A voltaic (galvanic) cell is constructed using a zinc electrode in $$1.0\ \mathrm{M}$$ $$\mathrm{$$ZnSO_4$$}$$ and a copper electrode in $$1.0\ \mathrm{M}$$ $$\mathrm{$$CuSO_4$$}. $$Which half-reaction occurs at the cathode?

Accepted Answer

$$\mathrm{Cu$$^{2+}$$ + 2e^- \rightarrow Cu}$$

Question 18

Which of the following statements about nuclear fission and fusion is correct?

Accepted Answer

Fission releases energy by splitting heavy nuclei; fusion releases energy by combining light nuclei.

Question 19

A solution is prepared by dissolving $$0.10\ \mathrm{mol} of a $$monoprotic strong acid in $$1.0\ \mathrm{L} of $$water. What is the pH of the solution?

Accepted Answer

pH = 1

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