Answer
$pH = 1.18$
Work Step by Step
- Identify the electrolytes:
$HClO_4$: Strong acid.
$RbOH$: Strong base.
1. Find the hydronium ion concentration produced by the acid.
Strong acid: $[H_3O^+] = [HClO_4]_{initial} = 0.088M$
2. Find the hydroxide ion concentration produced by the base.
Strong base: $[OH^-] = [RbOH]_{initial} = 0.022M$
3. Calculate their difference.
$0.088M - 0.022M = 0.066M$
- Since $H_3O^+$ had greater concentration, there is $0.066M$ $H_3O^+$ in excess.
4. Calculate the pH Value
$pH = -log[H_3O^+]$
$pH = -log( 0.066)$
$pH = 1.18$
