What is the pH of 2.0 liters of aqueous solution that contains 9.0 grams of HCl?

Question

Quizplus · Accepted Answer

First, calculate the molarity of the HCl solution. The molar mass of HCl is approximately 36.46 g/mol. Thus, 9.0 grams of HCl is 9.0 g / 36.46 g/mol = 0.247 moles of HCl. Since this is dissolved in 2.0 liters of solution, the molarity is 0.247 moles / 2.0 L = 0.1235 M. The concentration of H+ ions in a solution of HCl is equal to the concentration of HCl because HCl is a strong acid and dissociates completely in water. Therefore, the [H+] = 0.1235 M. The pH is calculated using the formula pH = -log[H+]. Plugging in the numbers, pH = -log(0.1235) ≈ 0.90.

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