Question

A sample of 0.0084 mol of HCl is dissolved in water to make a 1500 mL solution. Calculate the molarity of the HCl solution, the [H3O+] and the pH. For a strong acid such as HCl, the [H3O+] is the same as the molarity of the HCl solution.

Answer 1

A solution prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution has a Molarity of HCl of 5.6 × 10⁻³ M, a Molarity of H₃O⁺ of 5.6 × 10⁻³ M and a pH of 2.3.

What is Molarity ?

• Molarity (M) is the amount of a substance in a certain volume of solution.
• Molarity is defined as the moles of a solute per liters of a solution.
• Molarity is also known as the molar concentration of a solution

A solution is prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution. The molarity of HCl is:

[HCl] = 0.0084 moles / 1.5 L

        = 5.6 × 10⁻³ M

HCl is a strong acid according to the following equation.

HCl(aq) + H₂O(l) ⇒ Cl⁻(aq) + H₃O⁺(aq)

Thus, the concentration of H₃O⁺ will be equal to the initial concentration of HCl, 5.6 × 10⁻³ M.

Now, we will calculate the pH of the solution using its Formula ;

pH = - log[H₃O⁺]

 

    = - log [5.6 × 10⁻³]

    = 2.3

Hence, A solution prepared by dissolving 0.0084 moles of HCl in 1500 mL of solution has a Molarity of HCl of 5.6 × 10⁻³ M, a Molarity of H₃O⁺ of 5.6 × 10⁻³ M and a pH of 2.3.

Learn more about pH here ;

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