Question

A 25.0 ml sample of a saturated c a ( o h ) 2 solution is titrated with 0.022 m h c l , and the equivalence point is reached after 36.4 ml of titrant are dispensed. based on this data, what is the concentration (m) of c a ( o h ) 2 ?

Answer 1

The concentration of the 25 mL Ca(OH)₂ solution needed to reach the equivalence point with 36.4 mL 0.022 M HCl solution is 0.016 M

Balanced equation

2HCl + Ca(OH)₂ —> CaCl₂ + 2H₂O

From the balanced equation above,

• The mole ratio of the acid, HCl (nA) = 2
• The mole ratio of the base, Ca(OH)₂ (nB) = 1

How to determine the concentration of Ca(OH)₂

• Concentration of acid, HCl (Ca) = 0.022 M
• Volume of acid, HCl (Va) = 36.4 mL
• Volume of base, Ca(OH)₂ (Vb) = 25 mL

• Concentration of base, Ca(OH)₂ (Mb) =?

CaVa / CbVb = nA / nB

(0.022 ×36.4) / (Cb × 25) = 2

0.8008 / (Cb × 25) = 2

Cross multiply

Cb × 25 × 2  = 0.8008

Cb × 50 = 0.8008

Divide both side by 50

Cb = 0.8008 / 50

Cb = 0.016 M

Thus, the concentration of the Ca(OH)₂ solution is 0.016 M

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