Question

A solution has [oh−] = 4.0×10−8. what is the value of [h+] for the solution? answers

Answer 1

Answer is: the hydrogen ion concentration is 2.5·10⁻⁷ M.
[OH⁻] = 4·10⁻⁸ mol/L, equilibrium concentration of hydroxide anion.
[H⁺] is the equilibrium concentration of hydrogen ions.
[OH⁻] · [H⁺] = 10⁻¹⁴ mol²/L², ionicproduct of water on room temperature.
[H⁺] = 10⁻¹⁴ mol²/L² ÷  4·10⁻⁸ mol/L.
[H⁺] = 2,5·10⁻⁷ mol/L = 0,00000025 mol/L.

Answer 2

Answer: The pH of the solution is 6.68

Explanation:

To calculate the pOH of the solution, we use the equation:

$pOH=-\log[OH^-]$

We are given:

$[OH^-]=4.8\times ^{-8}M$

Putting values in above equation, we get:

$pOH=-\log (4.8\times 10^{-8})\\\\pOH=7.32$

Calculating the pH of the solution:

$pH+pOH=14\\\\pH=14-7.32=6.68$

Hence, the pH of the solution is 6.68