What is pH of HCl solution containing 0.365 g of HCl in 100 mL of...

What is pH of HCl solution containing 0.365 g of HCl in 100 mL of solution, assuming complete dissociation at 298 K? ( Molar mass of HCl = 36.5 g/mol)

Options

A $2$
B $1$
C $3.65$
D $3$

Correct answer

B. $1$

Step-by-step solution

Number of moles of

\text{HCl} = \dfrac{\text{Mass}}{\text{Molar mass}} = \dfrac{0.365}{36.5} = 0.01 \text{ mol}

Volume of solution

= 100 \text{ mL} = 0.1 \text{ L}

Molarity of

\text{HCl} = \dfrac{\text{Moles}}{\text{Volume in L}} = \dfrac{0.01}{0.1} = 0.1 \text{ M}

Since

\text{HCl}

is a strong acid, it dissociates completely.

[\textH^{+}] = 0.1 \text{ M} = 10^{-1} \text{ M}

\text{pH} = -\log[\textH^{+}] = -\log(10^{-1}) = 1

Answer:

1

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