Question

What volume of a 0.169 M barium hydroxide solution is required to neutralize 15.2 mL of a 0.397 M hydrochloric acid solution?

_____________mL barium hydroxide

Answer 1

Ba(OH)₂ + 2HCl → BaCl₂ + 2H₂O

Proportion 1:

0.397 mol – 1000 mL

x mol – 15.2 mL

$x = \frac{0.397 \times 15.2}{1000} = 0.00603\;mol \;(HCl)$

According to the reaction equation:

n(Ba(OH)₂) $= \frac{1}{2}n(HCl) = \frac{1}{2} \times 0.00603 = 0.00301 \;mol$

Proportion 2:

0.169 mol – 1000 mL

0.00301 – y mL

$y = \frac{0.00301 \times 1000}{0.169} = 17.853 \;mL$

Answer: 17.85 mL