The impure 6g of NaCl is dissolved in water and then treated with excess of silver nitrate solution. The mass of p[recipitate of silver chloride is found to be 14g. The % purity of NaCl solution would be:

When 0.01 mole of a cobalt complex is treated with excess silver nitrate solution, 4.305 g silver chloride is precipitated. The formula of the complex is

A coordination complex compound of cobalt has molecular formula containing five ammonia molecules, one nitro group and two chlorine atoms for one cobalt atom. One mole of this compound produces three mole ions in an aqueous solution. On reacting this solution with excess of silver nitrate solution, two moles of AgCl get precipitated. The formula of this compound would be

A silver coin weighing 11.34 g was dissolved in nitric acid When sodium chloride was added to the solution all the silver (present as AgNO_(3) ) precipitated as silver chloride. The mass of the precipitated silver chloride was 14.35 g. Calculate the percentage of silver in the coin.

A 1.0g sample of a pure organic compound cotaining chlorine is fused with Na_(2)O_(2) to convert chlorine to NaCl. The sample is then dissolved in water, and the chloride precipitated with AgNO_(3) , giving 1.96 g of AgCl. If the molecular mass of organic compound is 147, how many chlorine does each molecule contain ?

Pragya tested the solubility of three different substances at different temperatures and collected the data as given below (results are given in the following table, as grams of substance dissolved in 100 grams of water to form a saturated solution). What mass of potassium nitrate would be needed to produce a saturated solution of potassium nitrate in 50 grams of water at 313 K ?

A solution contains 40 g of NaCl in 320g of water. Calculate its concentration in terms of mass percentage of solution

A sample of 1.0g of solid Fe_(2)O_(3) of 80% purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7mL of a 0.1M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

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:

A solution is prepared by dissolving 2g of substance A in 18g of water. calculate the mass percentage of solute?