A `20.0mL` sample of `CuSO_(4)` solution was evaporated to dryness, leaving `0.967g` of residue. What was the molarity of the original solution ? `(Cu=63.5)`

The molarity of 4 g of NaOH in 100 mL solution is 0.5 M.

0.5 Faraday of electricity was passed jo deposit áll the copper present in 500ml of CuSO_4, solution. What was the molarity of this solution?

0.5 Faraday of electricity was passed jo deposit áll the copper present in 500ml of CuSO_4, solution. What was the molarity of this solution?

One litre of a saturated solution of CaCO_3 is evaporated to dryness due to which 7.0 mg of residue is left. The solubility product for CaCO_3 is

The density of the solution of a salt X is 1.15 "g mL"^(-1) . 20 mL of the solution when completely evaporated gave a residue of 4.6g of the salt. Calculate the mass percentage of the solute in solution.

The density of the solution of a salt X is 1.15 "g mL"^(-1) . 20 mL of the solution when completely evaporated gave a residue of 4.6g of the salt. Calculate the mass percentage of the solute in solution.

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?

One litre of a saturated solution of CaCO_(3) is evaporated to dryness due to which 7.0 mg of residue is left . The solubility product for CaCO_(3) is

One litre of a saturated solution of CaCO_(3) is evaporated to dryness due to which 7.0 mg of residue is left . The solubility product for CaCO_(3) is

12 g of a saturated solution of potassium chloride at 20^@C , when evaporated to dryness, leaves a solid residue of 3 g. Calculate the solubility of potassium chloride.