Q: Given $$K_w = 1.0 \times 10$$^{-14}$$ at 25$$^\circ$$C, what is the $$[\mathrm{OH^-}]$$ in a solution with $$[\mathrm{H_3O^+}] = 2.0 \times $$10^{-4}$$\ \mathrm{M}$$?

$$5.0 \times 10$$^{-11}$$\ \mathrm{M}$$

Question 1

Which of the following statements best describes why hydrochloric acid (HCl) is considered a strong acid in water?

Accepted Answer

Because HCl completely ionizes in water, producing $$\mathrm{H_3O^+}$$ and $$\mathrm{Cl^-}$$ ions.

Question 2

Which of the following is an example of an Arrhenius base?

Accepted Answer

NaOH

Question 3

A solution has $$[\mathrm{H_3O^+}] = 1.0 	imes 10$$^{-5}$$\ \mathrm{M}. $$What is the pH of this solution?

Accepted Answer

$$5.00$$

Question 4

Which of the following pairs are NOT conjugate acid–base pairs?

Accepted Answer

$$\mathrm{H_2SO_4}$$ and $$\mathrm{H_2SO_3}$$

Question 5

Which of the following substances can act as both a Brønsted–Lowry acid and a base?

Accepted Answer

$$\mathrm{H_2O}$$

Question 6

A student adds sodium bicarbonate ($$\mathrm{$$NaHCO_3$$}) to a $$solution of hydrochloric acid ($$\mathrm{HCl}). $$Which reaction best describes what occurs?

Accepted Answer

$$\mathrm{$$NaHCO_3$$}$$ acts as a base and neutralizes $$\mathrm{HCl}$$, producing $$\mathrm{CO_2$}$$, $$\mathrm{H_2O}$$, and $$\mathrm{NaCl}.$$

Question 7

Which of the following acids is triprotic?

Accepted Answer

$$\mathrm{H_3PO_4}$$

Question 8

Given $$K_w = 1.0 	imes 10$$^{-14}$$ at 25$$^\circ$$C, what is the $$[\mathrm{OH^-}]$$ in a solution with $$[\mathrm{H_3O^+}] = 2.0 	imes $$10^{-4}$$\ \mathrm{M}$$?

Accepted Answer

$$5.0 	imes 10$$^{-11}$$\ \mathrm{M}$$

Question 9

Which of the following best explains why weak acids only partially ionize in water?

Accepted Answer

The attraction between $$\mathrm{H^+}$$ and the conjugate base is strong, favoring the reactants.

Question 10

A solution has a pOH of $$3.00. $$What is its pH at $$25^\circC$$?

Accepted Answer

$$11.00$$

Question 11

Which of the following is a property of bases?

Accepted Answer

They turn red litmus paper blue.

Question 12

Which of the following equations represents the autoionization of water?

Accepted Answer

$$2\ \mathrm{H_2O}(l) \rightleftharpoons \mathrm{H_3O^+}(aq) + \mathrm{OH^-}(aq)$$

Question 13

Which of the following acids has the largest $$K_a$$ value based on the diagrams below (HA, HB, HC)?

Accepted Answer

The acid with the greatest number of dissociated ions in solution.

Question 14

Which of the following is the correct expression for the acid ionization constant ($$K_a) $$for a generic acid $$HA$$?

Accepted Answer

$$K_a = \dfrac{[A^-][H_3O^+]}{[HA]}$$

Question 15

A cleaning product contains ammonia ($$\mathrm{NH_3$}). $$According to the Brønsted–Lowry definition, what role does ammonia play when dissolved in water?

Accepted Answer

It accepts a proton from water.

Question 16

Which of the following statements about pH is correct?

Accepted Answer

A solution with pH $$4 is $$ten times more acidic than a solution with pH $$5.$$

Question 17

Which of the following best describes the relationship between $$K_a$$ and $$pK_a$$?

Accepted Answer

$$pK_a = -\log K_a$$

Question 18

A solution has a pH of $$8.37. $$What is the $$[\mathrm{H_3O^+}]$$?

Accepted Answer

$$4.3 	imes 10$$^{-9}$$\ \mathrm{M}$$

Question 19

Which of the following is a property of acids?

Accepted Answer

They turn blue litmus paper red.

Acids and Bases: Properties, Definitions, and Calculations

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