a 50 ml aliquot of unknown Cu2+ solution was exhaustively electrolyze to deposit

Question

a 50 ml aliquot of unknown Cu2+ solution was exhaustively electrolyze to deposit all copper on the cathode. The mass of cathode was 15.327 g prior electrolysis and 16.414 g after electrolysis.Find the molarity of Cu2+ in the unknown a 50 ml aliquot of unknown Cu2+ solution was exhaustively electrolyze to deposit all copper on the cathode. The mass of cathode was 15.327 g prior electrolysis and 16.414 g after electrolysis.Find the molarity of Cu2+ in the unknown a 50 ml aliquot of unknown Cu2+ solution was exhaustively electrolyze to deposit all copper on the cathode. The mass of cathode was 15.327 g prior electrolysis and 16.414 g after electrolysis.Find the molarity of Cu2+ in the unknown

Explanation / Answer

mass of Cu deposited = (16.414 - 15.327) g
= 1.087 g
molar mass of Cu = 63.5 g/mol
number of mole of Cu = (mass of Cu deposited)/(molar mass of Cu)
= 1.087/63.5
= 0.0171 mole

molarity of Cu+2 = (number of mole of Cu)/(volume in L)
volume of solution = 50 ml
= 0.05 L
so,
molarity of Cu+2 = 0.0171/0.05
= 0.342 M

Answer : 0.342 M

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