Chemistry: What is the ph of a solution that contains 5.23g of hydrochloride acid dissolved in 52.32l of water

What is the ph of a solution that contains 5.23g

DepressionCentral

27.01.2022

2.56

Explanation:

What is the pH of a solution that contains 5.23g of hydrochloric acid dissolved in 52.32L of water?

Step 1: Calculate the moles of hydrochloric acid

The molar mass of hydrochloric acid is 36.46 g/mol. The moles corresponding to 5.23 g are:

$5.23g \times \frac{1mol}{36.46g} =0.143mol$

Step 2: Calculate the molar concentration of hydrochloric acid

$M= \frac{0.143mol}{52.32L} =2.73 \times 10^{-3} M$

Step 3: Calculate the molar concentration of H⁺

Hydrochloric acid is a strong monoprotic acid that dissociates according to the following expression.

HCl(aq) ⇒ H⁺(aq) + Cl⁻(aq)

Then, [H⁺] = 2.73 × 10⁻³ M

Step 4: Calculate the pH of the solution

We use the following expression.

pH = -log [H⁺]

pH = -log 2.73 × 10⁻³

pH = 2.56

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