10 g of a sample of `Ca(OH)_2` is dissolved in 10 mL of 0.5 N HCL solution . The excess of HCl was titrated with 0.2 N NaOH. The volume of NaOH used was 10 cc. Calculate the percentage of `Ca(OH)_2` in the sample.

10ml 0.05 N H_2SO_4 solution is mixed with 10 ml 0.1 N NaOH solution. The pH of the final mixture is

25 mL, 0.2 M Ca(OH)_2 is neutralised by 10 mL of 1 M HCl. then pH of resulting solution is-

5.3g of M_(2)CO_(3) is dissolved in 150 mL of 1(N) HCl. Unused acid required 100 mL of 0.5(N) NaOH. Hence equivalent weight of M is-

0.804 g sample of iron was dissolved in acid , Iron was reduced to +2 state and it required 47.2 mL of 0.112 N KMnO_4 solution for titration. Calculate the percentage of iron and Fe_3O_4 in the ore.

The volume of 0 -1M Ca(OH)_2 required to neutralize 10 ml of 0 -1N HCI will be

5 mL of 0.4 N NaOH is mixed with 20 mL of 0.1 N HCl The pH of the resulting solution will be

On adding 20 ml. of N/10 NaOH solution to 10 ml. of N/10 HCl, the resulting solution will

0.35 g of an organic substance was Kjeldahlised and the ammonia obtained was passed into 100 ml of N/5 H_(2)SO_(4) . The excess acid required 154 ml of N/10 NaOH for neutralisation. Calculate the percentage of nitrogen in the compound.

A100 ml solution of 0.1 N HCl was titrated with 0.2 N NaOH solution. The titration was discontinued after adding 30 ml of NaOH solution. The remaining titration was completed by adding 0.25 N KOH solution. The volume of KOH required for completing the titration is

10 ml of NaHC_2O_4 solution is neutralized by 10 ml of 0.1 M NaOH solution. 10 ml of same NaHC_2O_4 solution is oxidised by 10 ml of KMnO_4 solution in acidic medium. Calculate the molarity of KMnO_4 solution.