a.) An aqueous solution of barium hydroxide is standardized by titration with a

Question

a.) An aqueous solution of barium hydroxide is standardized by titration with a 0.177 M solution of nitric acid.

If 25.8 mL of base are required to neutralize 10.4 mL of the acid, what is the molarity of the barium hydroxide solution?

[ ] M barium hydroxide

b.) An aqueous solution of calcium hydroxide is standardized by titration with a 0.143 M solution of hydrochloric acid.

If 15.6 mL of base are required to neutralize 16.2 mL of the acid, what is the molarity of the calcium hydroxide solution?

[ ] M calcium hydroxide

Explanation / Answer

Ans

a)

the balanced reaction is given as :

Ba(OH)2 + 2HNO3 = Ba(NO3)2 + 2H2O

Now using the formula , M1V1/n1 = M2V2/n2

where M is molarity , V is volume and n is number of moles

Putting all the values :

(0.177 x 10.4) / 2 = (M2 x 25.8) /1

M2 = 0.036 M

= [0.036] M barium hydroxide

b) The reaction is given as :

Ca(OH)2 + 2HNO3 = Ca(NO3)2 + 2H2O

using the same formula again:

(0.177 x 16.2) /2 = (M2 x 15.6) / 1

M2 = 0.094 M

[0.094] M calcium hydroxide

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