Question

The equation for the pH of a substance is pH = -log[H], where Ht iS the concentration of hydrogen ions. A basic

solution has a pH of 11.2. An acidic solution has a pH of 2.4. What is the approximate difference in the concentration
of hydrogen ions between the two solutions?

Answer 1

B. 4.0 x
`10^(-3)`

Explanation:

EDG2021

Answer 2

The difference in the H⁺ concentration between the two solutions is approximately equal to the H⁺ concentration of the acidic solution.

Explanation:

The pH is given by:

`pH = -log[H^(+)]`

Where:

`[H^(+)]`: is the concentration of hydrogen ions.

For the basic solution (pH = 11.2), the concentration of H⁺ is given by:

`[H^(+)]_(b) = 10^(-pH) = 10^(-11.2) = 6.31 \cdot 10^(-12)`

And, for the acidic solution (pH = 2.4) we have:

`[H^(+)]_(a) = 10^(-pH) = 10^(-2.4) = 3.98 \cdot 10^(-3)`

Hence, the difference in the concentration of H⁺ between the two solutions is:

`\Delta H^(+) = [H^(+)]_(a) - [H^(+)]_(b) = 3.98 \cdot 10^(-3) - 6.31\cdot 10^(-12) = 3.98 \cdot 10^(-3)`

Therefore, the difference in the H⁺ concentration between the two solutions is approximately equal to the H⁺ concentration of the acidic solution.

I hope it helps you!