Q: A buffer is prepared using acetic acid and sodium acetate. Which equation best describes the pH of the buffer?

$$\text{pH} = \text{p}K_a + \log\left(\frac{[\text{Acetate}]}{[\text{Acetic Acid}]}\right)$$

Question 1

Which of the following best explains why the dissolution of NaCl in water is spontaneous at room temperature?

Accepted Answer

The process is driven by an increase in entropy ($$\Delta S \u003e 0) $$and a favorable free energy change ($$\Delta G \u003c 0).$$

Question 2

A solution is prepared by dissolving 0.5 mol of glucose (a non-electrolyte) and 0.5 mol of NaCl (an electrolyte) in enough water to make 1.0 L of solution. What is the van’t Hoff factor ($$i) $$for NaCl in this solution?

Accepted Answer

$$i = 2$$

Question 3

Which of the following statements about chemical equilibrium is correct?

Accepted Answer

At equilibrium, the rates of the forward and reverse reactions are equal.

Question 4

Consider the reaction $$\ce{N_2$(g) + 3H_2(g)  2NH_3(g)}. If $$the system is at equilibrium and more $$\ce{N_2$} is $$added, what will happen according to Le Châtelier’s Principle?

Accepted Answer

The equilibrium will shift to produce more $$\ce{NH_3$}.$$

Question 5

Which of the following is omitted from the equilibrium expression for the dissociation of acetic acid in water?

Accepted Answer

Water ($$\ce{H_2O})$$

Question 6

A 0.10 M solution of a weak acid has a $$K_a of$$ $$1.8 	imes 10$$^{-5}$$. What is the approximate pH of the solution?

Accepted Answer

pH $$\approx 3.0$$

Question 7

Which salt solution will be acidic?

Accepted Answer

NH$$_4Cl$$

Question 8

Which of the following is a Lewis acid?

Accepted Answer

$$\ce{Al$$^{3+}$$}$$

Question 9

A buffer is prepared using acetic acid and sodium acetate. Which equation best describes the pH of the buffer?

Accepted Answer

$$	ext{pH} = 	ext{p}K_a + \log\left(\frac{[	ext{Acetate}]}{[	ext{Acetic Acid}]}ight)$$

Question 10

During the titration of a weak acid with a strong base, which point corresponds to the maximum buffer capacity?

Accepted Answer

At the half-equivalence point

Question 11

Which of the following best describes the common-ion effect?

Accepted Answer

Addition of a common ion decreases the solubility of a salt.

Question 12

What is the molar solubility of AgCl in water if $$K_{sp} = 1.8 	imes 10$$^{-10}$$?

Accepted Answer

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

Question 13

Which equation represents the integrated rate law for a first-order reaction?

Accepted Answer

$$\ln [A] = \ln [A]_0 - kt$$

Question 14

A reaction has a rate constant $$k$$ that increases when temperature increases. Which equation best describes this relationship?

Accepted Answer

$$k = Ae$$^{-E_a/RT}$$

Question 15

Which statement about catalysts is correct?

Accepted Answer

Catalysts lower the activation energy ($$E_a) $$and increase the rate of reaction.

Question 16

Which equation relates the standard cell potential ($$E^\circ_{cell}) to $$the standard free energy change ($$\Delta G^\circ$$)?

Accepted Answer

$$\Delta G^\circ = -nFE^\circ_{cell}$$

Question 17

Which of the following is true about the Nernst equation?

Accepted Answer

It is used to calculate cell potential under non-standard conditions.

Question 18

Which of the following hydrocarbons is an example of a structural isomer?

Accepted Answer

n-butane and isobutane

Question 19

Which functional group is present in both alcohols and carboxylic acids?

Accepted Answer

Hydroxyl group ($$-\ce{OH})$$

Question 20

According to Crystal Field Theory, which type of ligand causes the largest crystal field splitting energy ($$\Delta$$)?

Accepted Answer

Strong-field ligands

CHEM 10123-015 General Chemistry II: Course Schedule and Topic Overview (Spring 2026)

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