Answer
The pH of this solution is equal to $7.00$ (Neutral).
Work Step by Step
1000ml = 1L
24ml = 0.024 L
20ml = 0.02 L
1. Find the numbers of moles:
$C(HClO_4) * V(HClO_4) = 0.125* 0.024 = 3 \times 10^{-3}$ moles
$C(KOH) * V(KOH) = 0.15* 0.02 = 3 \times 10^{-3}$ moles
2. When the number of moles is equal, the reactants are totally consumed:
$HClO_4(aq) + KOH(aq) -- \gt KClO_4(aq) + H_2O(l)$
- Total volume: 0.024 + 0.02 = 0.044L
3. So, those are the final concentrations:
$[HClO_4] = 0.003 - 0.003 = 0$ mol.
$[KOH] = 0.003 - 0.003 = 0$ mol
- Therefore, the solution doesn't have any significant electrolyte: pH = 7 (Neutral)
