Find out % of oxalate ion in a given sample of an alkali metal oxalate salt, `0.30g` of it is dissolved in `100mL` water and its required `90mL` of centimolar `KMnO_4` solution in acidic medium :

1.26 g of hydrated oxalic acid was dissolved in water to prepare 250ml of solution. calculate molarity of the solution.

4.0 g of NaOH and 4.9 g of H_(2)SO_(4) are dissolved in water and volume is made upto 250 mL. The pH of this solution is:

A sample of NaOH weighing 0.38 g is dissolved in water and solution is made to 50.0 mL in a volumetric flask. What is the molarity of the solution?

If a g is the mass of NaHC_(2)O_(4) required to neutralize 100mL of 0.2M NaOH and b g that required to reduce 100mL of 0.02M KMnO_(4) in acidic medium then:

0.63 g of HNO_(3) dissolved in 100 ml of solution. Calculate its pH value.

A mixture of H_(2)SO_(4) and H_(2)C_(2)O_(4) (oxalic acid ) and some inert impurity weighing 3.185 g was dessolved in water and the solution made up to 1litre. 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another experiment 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO_(4) solution for complete reaction. The mass % of H_(2)SO_(4) in the mixture was:

At 300 K, 40 mL of O_(3)(g) dissolves in 100g of water at 1.0atm . What mass of ozone dissolved in 400g of water at a pressure of 4.0atm at 300 K ?

A solution is prepared by dissolving 1.0 g of NaOH in water to get 250 ml of solution . Calculate its molarity .

6.2g of a sample containing Na_2CO_3, NaHCO_3 and non-volatile inert impurity on gentle heating loses 5% of its mass due to reaction 2NaHCO_3 rarr Na_2 CO_3 + H_2 O + CO_2 . Residue is dissolved in water and formed 100mL solution and its 10mL portion requires 7.5 mL of 0.2M aqueous solution of BaCI_2 for complete precipitation of carbonates. Determine mass (in gram) of Na_2 CO_3 in the original sample.

6.0 g weak acid HA (mol.mass=60 g/mol.) is dissolved in water and formed 10 m^(3) solution. If K_(a)(HA)=10^(-9), then pOH of solution is : [Given: log 4=0.6]