Q: A solution has a pH of 2. What is the hydrogen ion concentration ($$[\mathrm{H^+}]) in $$this solution?

$$1 \times 10$$^{-2}$$\ \mathrm{M}$$

Question 1

Which of the following best describes the difference between the Arrhenius and Brønsted-Lowry theories of acids and bases?

Accepted Answer

Arrhenius theory defines acids as substances that increase the concentration of H+ ions in water, while Brønsted-Lowry theory defines acids as substances that donate protons (H+).

Question 2

Which of the following is a balanced neutralization reaction between sulfuric acid ($$\mathrm{H_2SO_4}) $$and sodium hydroxide ($$\mathrm{NaOH}$$)?

Accepted Answer

$$\mathrm{H_2SO_4} + 2\mathrm{NaOH} \rightarrow 2\mathrm{H_2O} + \mathrm{Na_2SO_4}$$

Question 3

A solution has a pH of 2. What is the hydrogen ion concentration ($$[\mathrm{H^+}]) in $$this solution?

Accepted Answer

$$1 	imes 10$$^{-2}$$\ \mathrm{M}$$

Question 4

Which of the following environmental processes is most directly affected by soil pH?

Accepted Answer

Nutrient availability for plants

Question 5

What is the main reason why most metals are more soluble at low pH?

Accepted Answer

Increased concentration of H+ ions promotes dissolution of metal compounds.

Question 6

Which of the following is the correct formula for calculating pH?

Accepted Answer

$$\mathrm{pH} = -\log[\mathrm{H^+}]$$

Question 7

If a solution changes from pH 6 to pH 4, how does the hydrogen ion concentration change?

Accepted Answer

It increases by a factor of 100.

Question 8

Which of the following best describes a buffer solution?

Accepted Answer

A solution that contains a weak acid and its conjugate base, and resists changes in pH when small amounts of acid or base are added.

Question 9

Which of the following reactions represents the formation of carbonic acid from carbon dioxide and water?

Accepted Answer

$$\mathrm{CO_2$} + \mathrm{H_2O} \rightarrow \mathrm{H_2CO_3}$$

Question 10

Which of the following is the conjugate base of carbonic acid ($$\mathrm{H_2CO_3}$$)?

Accepted Answer

$$\mathrm{$$HCO_3$$^-}$$

Question 11

A soil sample has a pH of 4.4. Which of the following is most likely to occur?

Accepted Answer

Aluminum toxicity may affect plant growth.

Question 12

Which of the following best explains why ocean acidification is a concern for marine organisms?

Accepted Answer

Lower pH increases the concentration of hydrogen ions, which can dissolve calcium carbonate shells.

Question 13

Which of the following is NOT a contributor to alkalinity in natural waters?

Accepted Answer

Sodium chloride

Question 14

Which of the following statements about pH and alkalinity is correct?

Accepted Answer

Higher pH means more basic, but does not necessarily mean higher alkalinity.

Question 15

Which of the following is a real-world example of a neutralization reaction?

Accepted Answer

Antacid tablets neutralizing stomach acid

Question 16

Which of the following equations represents the reaction of ammonia ($$\mathrm{NH_3$}) $$with water according to the Brønsted-Lowry theory?

Accepted Answer

$$\mathrm{NH_3$} + \mathrm{H_2O} \rightleftharpoons \mathrm{NH_4$^+} + \mathrm{OH^-}$$

Question 17

If a freshwater stream is affected by acid mine drainage, which of the following is most likely to occur?

Accepted Answer

The pH of the stream will decrease, increasing metal solubility.

Question 18

Which of the following best describes the role of the carbonate buffer system in the ocean?

Accepted Answer

It helps maintain a stable pH by neutralizing added acids or bases.

Question 19

A solution has a hydrogen ion concentration of $$1 	imes 10$$^{-8}$$\ \mathrm{M}. $$How would you classify this solution?

Accepted Answer

Slightly basic

Lecture 18

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