Question

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

Answer 1

2.56

Step-by-step 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 * (1mol)/(36.46g) =0.143mol`

Step 2: Calculate the molar concentration of hydrochloric acid

`M= (0.143mol)/(52.32L) =2.73 * 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