What is the pH of a solution in which 222 mL of HCl (g), measured at 26.0 ∘C and 1.06 atm, is dissolved in water to give 1.5 L of aqueous solution? (Hint: Use the ideal gas law to find moles of HCl first.)

Question

Yareli Turner

Chemistry

24 May, 00:47

What is the pH of a solution in which 222 mL of HCl (g), measured at 26.0 ∘C and 1.06 atm, is dissolved in water to give 1.5 L of aqueous solution? (Hint: Use the ideal gas law to find moles of HCl first.)

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Answers (1)

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Milton Richards · Answer 1

6.39 * 10⁻³ M

Explanation:

First, we will calculate the moles of HCl using the ideal gas equation.

P * V = n * R * T

n = P * V / R * T

n = 1.06 atm * 0.222 L / 0.0821 atm. L/mol. K * (26.0 + 273.15) K

n = 9.58 * 10⁻³ mol

The molar concentration of HCl is:

M = moles of HCl / liters of solution

M = 9.58 * 10⁻³ mol / 1.5 L

M = 6.39 * 10⁻³ M