Exam 10: Acids and Bases in Our Environment

When the pH of a solution is 1, the concentration of hydronium ions is M, which is the same as 0.1 M. Assume that the volume of this solution is 500 mL and that the solution is not buffered. What would be the new pH of this solution after 500 mL of pure water is added? You will need a calculator with a log function to answer this question.

How might warmer oceans accelerate global warming?

At what point will a buffer solution cease to moderate changes in pH?

Which of the following statements describes an acidic solution?

Some molecules are able to stabilize a negative charge by passing it from one atom to the next by a flip-flopping of double bonds. This occurs when the negative charge is one atom away from an oxygen double bond as follows. Note that the curved arrows indicate the movement of electrons: Why then is sulfuric acid so much stronger an acid than carbonic acid?

What results when water, O, reacts with sulfur dioxide, S ?

According to the following reaction, which molecule is acting as an acid? H₃O⁺ + HSO₄^- → H₂O + H₂SO₄

Which of the following solutions is the most acidic?

When the hydronium ion concentration equals 1 mole per liter, what is the pH of the solution? Is the solution acidic or basic?

Suggest why people once washed their hands with ashes.

Cutting back on the pollutants that cause acid rain is one solution to the problem of acidified lakes. Suggest another.

Sometimes an individual going through a traumatic experience cannot stop hyperventilating. In such a circumstance, it is recommended that the individual breath into a paper bag or cupped hands as a useful way to avoid an increase in blood pH, which can cause the person to pass out. Explain how this works.

Which of the following statements is not true about a neutralization reaction?

What is the hydroxide ion concentration in an aqueous solution where the pH = 5?

For the following reaction, identify whether the compound in bold is behaving as an acid or a base. H₃PO₄ + H₂O ⇌ H₂PO₄^- + H₃O⁺

What would the concentration of H₃O⁺ be if the concentration of OH^- was 1 × 10^-11M? [H₃O⁺] × [OH^-] = K_w = 1 × 10^-14

As the hydronium ion concentration increases, the pH ________.

What is the main characteristic of a strong acid?

Why do we use the pH scale to indicate the acidity of a solution rather than simply stating the concentration of hydronium ions?

For the following acid-base reaction, identify what is formed in the space marked. HF + KOH ⇌ ???? + H₂O