Problem: A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00 × 10−2 M HCl requires 36.6 mL of the acid to reach the end point.Ca(OH)2(aq) + 2HCl(aq) ⟶ CaCl2(aq) + 2H2O(l)What is the molarity?

FREE Expert Solution

The titration is at endpoint which means that all of the base is neutralized by the acid. 


Ca(OH)2(aq) + 2HCl(aq) ⟶ CaCl2(aq) + 2H2O(l)

1 mole Ca(OH)2 : 2 mole HCl


Recall: 

Molarity = moles solute L solution


Calculate moles Ca(OH)2:

5.00 × 10−2 mol HCl 1 L×36.6 mL×10-3 L1 mL×1 mol Ca(OH)22 mol HCl 

= 9.15 x 10-4 mol Ca(OH)2 


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Problem Details

A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00 × 10−2 M HCl requires 36.6 mL of the acid to reach the end point.

Ca(OH)2(aq) + 2HCl(aq) ⟶ CaCl2(aq) + 2H2O(l)

What is the molarity?

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