Chemistry HW help

Question

How many milliliters of 0.100 M HCIO3 are required to neutralize 39.4 mL of 0.140 M KOH?

Answer 1

Write the balanced chemical reaction equation:

HCIO₃ + KOH → KClO₃ + H₂O

(notice that no prefix coefficients were required)

Determine the number of moles of KOH in the 39.4 mL of 0.140 M solution:

39.4 mL = 0,0394 liters x 0.140 moles/liter = 0.005516 moles

Determine the number of moles of HClO₃ required to neutralize 0.005516 moles of KOH:

Using the chemical reaction equation, you see it takes 1 mole of HClO₃ to neutralize 1 mole of HOH so 0.005516 moles of HClO₃ is required.

Determine the volume of HClO₃ required to give 0.005516 moles:

(0.005516 moles)/(0.100 moles/liter) = 0.05516 liters

Convert liters to mL:

0.05516 liters x 1000 mL/1liter = 55.16 mL then round to 3 sig figs to get 55.2 mL of HClO₃