What is the pH of a 1.00 molar solution of nitrous acid? The K_a for nitrous acid is 7.1 × 10^-4.

Question

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The correct answer is A because the pH of a 1.00 molar solution of nitrous acid can be calculated using the following equation: pH = -log[H+], where [H+] is the molar concentration of hydrogen ions in the solution. The Ka for nitrous acid is 7.1 × 10-4, which means that the equilibrium constant for the dissociation of nitrous acid is 7.1 × 10-4. This means that for every 1 mole of nitrous acid that dissociates, 7.1 × 10-4 moles of hydrogen ions are produced. Therefore, the molar concentration of hydrogen ions in a 1.00 molar solution of nitrous acid is 7.1 × 10-4 M. Substituting this value into the equation for pH, we get: pH = -log(7.1 × 10-4) = 1.57.

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