Question

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

Answer 1

Answer: The pH of the solution is 6.68

Step-by-step explanation:

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

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

We are given:

`[OH^-]=4.8* ^(-8)M`

Putting values in above equation, we get:

`pOH=-\log (4.8* 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

Answer 2

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.