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:

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

When two moles of [Co(NH_3)_5Cl]Cl_2 is treated with excess silver nitrate solution, the number of moles of silver chloride formed is

3.6g mixture of sodium chloride and potassium chloride is dissolved in water. The solution is treated with excess of silver nitrate solution, 7.74g of silver chloride is obatined. Find the percentage of sodium chloride and potassium chloride in the mixture.

If 5.85 g of NaCl is dissolved in 90g of water, the mole fraction of solute is

Xg of Ag was dissolved in HNO_3 and the solution was treated with excess of NaCl when 2.87g of AgCl was precipitated. The value of X is

When 0.01 mole of a cobalt complex is treated with excess of silver nitrate solution 4.035 g of silver chloride is precipitated. The formula of the complex is :

Commerical sodium hydroxide weighing 30 g has some sodium chloride in it. The mixture on dissolving in water and subsequent treatment with excess silver nitrate solution formed a precipitate weighing 14.3 g. What is the percentage of sodium chloride in the commercial sample of sodium hydroxide? The equation for the reaction is NaCl+AgNO_(3) to AgCl+NaNO_(3) (Relative molecular mass of NaCl=58,AgCl=143)

10 g of NaCl is dissolved in 250 g water. The correct expressions for concentration of NaCl in solution are :

Out of water and silver nitrate solution, in which case silver choride will dissolve more?