Question

1.25 grams of an acidnis completely neutralised by 25ml of a 0.25M Ba(OH)2 SOLUTION.which of the following statements are correct.
a)if the acid is dibasic its molar mass would be 200
b)if it is dibasic /0.5g of the acid would neutralise completely 12.5ml of 0.40N NaOH.
C)volume of base used is independent of strength of the acid

Answer 1

The only way I know to do this is to work each answer as a separate problem.
a. H2A + Ba(OH)2 ==> BaA + 2H2O
mols Ba(OH)2 = M x L = ?
mols = grams/molar mass. You have mols from above and grams from the problem, solve for molar mass. If you get 200 for molar mass then a must be right.

b. mols H2A = grams/molar mass. Use 0.5 g as in the problem and use molar mass found in part a. Then
H2A + 2NaOH ==> Na2A + 2H2O
Convert mols H2A to mols NaOH needed and compare with mols generated by 12.5 mL of 0.40M NaOH. YOu do that with mols = M x L = ? This answer will tell you if b is correct or not.

c. C is a dumb answer; you know it can't be right.