A 0.00100 moles sample of ca (oh) 2 requires 25.00 ml of aqueous hcl for neutralization. how many moles of acid are contained in the 25.00 ml?

a. 0.0200

d. 4.00 ' 10-5

b. 0.0400

e. none of the above

c. 0.002

The balanced chemical equation for the reaction is as follows;

Ca (OH) 2 + 2HCl - > CaCl2 + 2H2O

The stoichiometry of Ca (OH) 2 to HCl is 1:2.

Number of Ca (OH) 2 moles reacted = 0.00100 mol

Therefore number of HCl moles that should react with base is double the amount of moles of base reacted.

Number of acid moles in 25.00 ml

= 0.00100 mol x2 = 0.00200 mol

Correct answer is 0.002 mol