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Chapter 14: Problem 112

Calculate the \(\mathrm{pH}\) of a \(5.0 \times 10^{-3}-M\) solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\).

Short Answer

Expert verified
The pH of a \(5.0 \times 10^{-3}\) M solution of H\(_2\)SO\(_4\) is 2.

Step by step solution

01

Calculate the concentration of hydrogen ions

Since H2SO4 is a diprotic acid, it will release two hydrogen ions per molecule. In 5.0 x 10^-3 M solution of H2SO4, the total concentration of hydrogen ions (H+) will be: [H+] = 2 * (5.0 x 10^-3 M) = 1.0 x 10^-2 M
02

Calculate the pH of the solution

Now that we have the concentration of hydrogen ions, we can use the formula for the pH of a solution: pH = -log10[H+] Plugging in the values: pH = -log10(1.0 x 10^-2)
03

Simplify the expression and find the pH value

Simplify the expression: pH = -(-2) So, the pH of the solution is: pH = 2 The pH of a 5.0 x 10^-3 M solution of H2SO4 is 2.

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