An aqueous solution has a hydrogen ion contamination of 1.15x10^-2M (1)What is the hydroxide ion concentration in this solution? (2)What is the pOH of this solution? (3)What is the pH of this solution?

See explanation

Explanation:

We know that

pH = - log [H^+]

but [H^+] = 1.15x10^-2M

Hence;

pH =  - log(1.15x10^-2)

pH = 1.94

And;

pH + pOH = 14

pOH = 14-pH

pOH = 14 - 1.94

pOH = 12.06

Since;

pOH = - log [OH^-]

hence;

[OH^-] = Antilog (-pOH)

[OH^-] = Antilog (12.06)

[OH^-] = 8.7 * 10^-13 M

the dissociation of nickel hydroxide is follows:

the concentration of hydroxide ion is

the equilibrium constant value of nickel hydroxide is = 6.1 * 10^-^1^6 and thus equilibrium equation can be written as:

thus, concentration of ni is 0.23 * 10^-^4 mol /l