The hydrogen sulfite ion, $\mathrm{HSO}_{3}^{-}$, is a weak acid in aqueous solution. Write an equation showing the equilibrium established when hydrogen sulfite is dissolved in aqueous solution, using unequal arrows to show the equilibrium.

Which of the following is true of a neutral aqueous solution? A. Its $H_3O^+$ ion concentration is 7.0 M. B. It contains buffers that resist a change in pH. C. It contains neither hydronium ions nor hydroxide ions. D. It has an equal number of hydronium ions and hydroxide ions.

How does Bronsted and Lowry’s definition of an acid differ from Arrhenius’s definition of an acid? Explain which definition is broader.

Giving examples, explain how strong acids and weak acids differ.

What is a neutral solution? What is its pH?

What is a neutralization reaction?

Write a balanced nuclear equation for each reaction. a. decay of sulfur-35 by $\beta$ emission b. decay of thorium-225 by $\alpha$ emission c. decay of rhodium-93 by positron emission d. decay of silver-114 by $\beta$ emission

Describe two methods of measuring pH, and explain the advantages and disadvantages of each method.

Explain how you can calculate pH from $[H_3O^+]$ by using your calculator.

By what factor does $[OH^−]$ change when the pH increases by 3? by 2? by 1? by 0.5?

Three solutions have pHs of 3, 7, and 11. Which solution is basic? Which is acidic? Which is neutral?

Write an equation that shows the self-ionization of water.

Explain the relationship between the self-ionization of water and $K_w$.

Write chemical equations that show how the hydrogen carbonate ion, $HCO ^− _3$, acts as an amphoteric ion.