Answer:
0.871 mL
Explanation:
Step 1: Write the balanced neutralization reaction
KOH + HF ⇒ KF + H₂O
Step 2: Calculate the reacting moles of HF
9.55 mL of 0.114 M HF react.
9.55 × 10⁻³ L × 0.114 mol/L = 1.09 × 10⁻³ mol
Step 3: Calculate the moles of KOH needed to react with 1.09 × 10⁻³ moles of HF
The molar ratio of KOH to HF is 1:1. The moles of KOH needed are 1/1 × 1.09 × 10⁻³ mol = 1.09 × 10⁻³ mol.
Step 4: Calculate the volume of KOH solution that contains 1.09 × 10⁻³ moles of KOH
An unknown volume of 1.252 M KOH solution contains 1.09 × 10⁻³ moles of KOH.
1.09 × 10⁻³ mol × 1 L/1.252 mol = 8.71 × 10⁻⁴ L = 0.871 mL
