Answer:
0.89
Explanation:
You are mixing an acid and a base, so there will be a neutralization reaction.
One of the reactants will be in excess, so we must determine its concentration and then calculate the pH.
Moles of NaOH
Moles of NaOH = 25 × 0.173
Moles of NaOH = 4.32 mmol
===============
Moles of HCl
Moles of HCl = 35 × 0.342
Moles of HCl = 12.0 mmol
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Amount of excess reactant
NaOH + HCl ⟶ NaCl +H₂O
n/mmol: 4.32 12.0
The 4.32 mmol of NaOH reacts completely with 4.32 mmol of HCl.
Excess HCl = 12.0 – 4.32
Excess HCl = 7.6 mmol
===============
Concentration of the excess HCl
Total volume = 25 + 35
Total volume = 60 mL
c = millimoles HCl/millilitres HCl
c = 7.6/60
c = 0.13 mol/L
===============
Calculate the pH
The HCl dissociates completely to hydronium ions, so
[H₃O⁺] = 0.13 mol·L⁻¹
pH = -log[H₃O⁺]
pH = -log0.13
pH = 0.89
