Answer
$pH = 1.18$
Work Step by Step
1000ml = 1L
50ml = 0.05 L
10ml = 0.01 L
1. Find the numbers of moles:
$C(HCl) * V(HCl) = 0.1* 0.05 = 5 \times 10^{-3}$ moles
$C(NaOH) * V(NaOH) = 0.1* 0.01 = 1 \times 10^{-3}$ moles
2. Write the acid-base reaction:
$HCl(aq) + NaOH(aq) -- \gt NaCl(aq) + H_2O(l)$
- Total volume: 0.05 + 0.01 = 0.06L
3. Since the base is the limiting reactant, only $ 0.001$ mol of the compounds will react.
Therefore:
Concentration (M) = $\frac{n(mol)}{Volume(L)}$
$[HCl] = 0.005 - 0.001 = 4 \times 10^{-3}$ moles.
Concentration: $\frac{4 \times 10^{-3}}{ 0.06} = 0.067M$
$[NaOH] = 0.001 - 0.001 = 0 $ moles
- Since $HCl$ is a strong acid:
$[HCl] = [H_3O^+] = 0.067M$
5. Calculate the pH Value
$pH = -log[H_3O^+]$
$pH = -log( 0.067)$
$pH = 1.18$
