Exam 10: Acids and Bases in Our Environment

Pour vinegar onto beach sand from the Caribbean and the result is a lot of froth and bubbles. Pour vinegar onto beach sand from California, however, and nothing happens. Why?

Which should be a stronger base: ammonia, , or trifluoronitrogen, ? Why?

Which of the following statements describes a basic solution?

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

Sodium hydroxide is added to a buffer solution of ammonia, N , and ammonium chloride, . What is the effect on the concentration of ammonia? What is the effect on the concentration of ammonium chloride?

Why is the H-F bond so much stronger than the H-I bond?

What is an acid?

What happens to the pH of soda water as it loses its carbonation?

The overall rate at which humans are producing carbon dioxide is ________.

In the following buffer system, what happens to the concentration of the highlighted molecule if you add acid in the form of H₃O⁺? HF + NaF + H₂O ⇌ F^- + H₃O⁺ _{+ Na}+

Which of the above illustrations shows a neutral aqueous solution?

Which of the following items would you use to make a basic buffer solution?

If the pH of a solution is 10, what is the hydroxide ion concentration?

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

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

How might warmer oceans accelerate global warming?

In the reaction below, what does the symbol ⇌ mean? OH^- + NH₄⁺ ⇌ H₂O + NH₃

Arrange the following images of an aqueous base solution in order of increasing base strength:

How might you tell whether or not your toothpaste contained either calcium carbonate, CaC , or baking soda, NaHC , without looking at the ingredients label?

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.