`1.25g` of a solid dibasic acid is completely neutralised by `25mL` of `0.25` molar Ba `(OH)_2` solution. Molecular mass of the acid is :

Two formulal to calculate number of milli equivalkents (mlQ) Numbr of miliequivalents =("weight")/("GEW")xx1000 Numbr of milliequivalents= volume in ml xx Normality of solution 0.09 grams of dibasic acid neutralise 40 ml of N/20 NaOH solution. Molecular weight of acid is

Calculate normality of H_(2)SO_(4) solutions if 50 ml of it completely neutralise 250 ml. of 0.1 N Ba(OH)_(2) solutions.

If 20 mL of 0.4 N NaOH solution completely neutralised 40 mL of a dibasic acid, the molarity of the acid solution is

40mL of 0.2M oxalic acid can completely decolourise what volume of 0.1M acidified permanganate solution?

8.7 gm of a sample of MnO_2 (molar mass = 87) is used in a chemical reaction with HCl to release Cl_2 Released Cl_2 is used to displace I_2 from excess of KI solution. The iodine hence released is estimated using hypo and consumes 100 ml of hypo solution.12.5 ml of same hypo solution is required for complete reaction with 25 ml of 0.5 N I_2 solution. Number of mili of iodine in the solution used with hypo are

0.84 g. of an acid of Molecular weight 225 is present in 100ml of the solution. 25ml of this solution required 28ml of N/10 NaOH solution for complete neutralisation. The basicity of the acid is

0.63 grams of a dioic acid required 50mL of 0.2M NaOH for neutralisation. Calculate the molar mass of acid .

12ml of H_(2)SO_(4) is completely neutralised with 15ml of 0.1N NaOH.What is the strength of acid in g L^(-1) ?

0.84 g, of an acid of Molecular weight 225 is present in 100ml of the solution. 25ml of this solution required 28 ml of N/10 NaOH solution for complete neutralisation. The basicity of the acid is