Question 1

Which of the following best explains why a 0.05 M solution of AlCl$$_3$$ has a higher conductivity than a 0.05 M solution of NaCl, assuming complete dissociation?

Accepted Answer

AlCl$$_3$$ produces more ions per formula unit upon dissociation than NaCl.

Question 2

Which of the following dissociation equations correctly represents the behavior of CaCl$$_2 in $$aqueous solution?

Accepted Answer

$$\mathrm{$$CaCl_2$$(aq) \rightarrow Ca$$^{2+}$$(aq) + 2Cl^-(aq)}$$

Question 3

A student measures the conductivity of four solutions, each at 0.05 M: NaCl, CH$$_3$$COOH, CH$$_3OH$$, and HCl. Which solution is expected to have the lowest conductivity?

Accepted Answer

CH$$_3OH$$

Question 4

Which of the following statements about weak electrolytes is TRUE?

Accepted Answer

They partially dissociate in water, resulting in low conductivity.

Question 5

Given the following dissociation equation for a weak acid: $$\mathrm{HF(aq) \rightleftharpoons H^+(aq) + F^-(aq)}$$, what does the double arrow indicate?

Accepted Answer

The reaction is reversible and only partial dissociation occurs.

Question 6

If 0.1 mL of 0.05 M NaCl is added to 35.0 mL of deionized water, what is the final concentration of NaCl in the solution? (Use $$M_1V_1 = M_2V_2)$$

Accepted Answer

$$0.00014\ \mathrm{M}$$

Question 7

Which of the following compounds is a non-electrolyte in aqueous solution?

Accepted Answer

CH$$_3OH$$

Question 8

A solution of 0.05 M H$$_3PO$_4 is $$tested for conductivity. Compared to 0.05 M HCl, what is the expected result and why?

Accepted Answer

H$$_3PO$_4$$ will have lower conductivity because it is a weak acid and only partially dissociates.

Question 9

Which of the following best describes the relationship between molar concentration and conductivity for a strong electrolyte?

Accepted Answer

As molar concentration increases, conductivity increases.

Question 10

Which of the following is the correct dissociation equation for NaOH in water?

Accepted Answer

$$\mathrm{NaOH(aq) \rightarrow Na^+(aq) + OH^-(aq)}$$

Question 11

A student adds 0.1 mL increments of 0.05 M CaCl$$_2 to 35.0 mL of $$deionized water and measures conductivity after each addition. What trend should the student observe?

Accepted Answer

Conductivity increases with each addition due to the increasing concentration of ions.

Question 12

Which of the following best explains why tap water conducts electricity while deionized water does not?

Accepted Answer

Tap water contains dissolved ions, while deionized water does not.

Question 13

Which of the following solutions will have the highest conductivity at the same molar concentration?

Accepted Answer

AlCl$$_3$$

Question 14

A student claims that all acids are strong electrolytes. Which of the following provides the best counterexample?

Accepted Answer

CH$$_3$$COOH is a weak acid and a weak electrolyte.

Question 15

Which of the following best describes the effect of the number of ions produced per formula unit on the conductivity of a solution?

Accepted Answer

The more ions produced per formula unit, the higher the conductivity.

Question 16

Which of the following is a correct dissociation equation for a weak base in water?

Accepted Answer

$$\mathrm{NH_4OH(aq) \rightleftharpoons NH_4$^+(aq) + OH^-(aq)}$$

Question 17

A solution of 0.05 M CH$$_3$$COOH is found to have much lower conductivity than a 0.05 M NaCl solution. What is the most likely explanation?

Accepted Answer

CH$$_3$$COOH is a weak electrolyte and only partially dissociates.

Question 18

Which of the following best describes the relationship between the slope of the conductivity vs. concentration graph and the number of ions produced by an electrolyte?

Accepted Answer

A greater number of ions per formula unit results in a steeper slope.

Question 19

Which of the following is NOT a strong electrolyte?

Accepted Answer

CH$$_3$$COOH

Conductivity of Electrolyte Solutions: Classification, Measurement, and Analysis

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