Question

M Na SO, to titrate it to the ehaponi and percent of sodium hypochlorite in the pool chlorine? g sample believed to be copper(I) acetate monohydrate required 11.84 mL of 0.105 ach the endpoint in an iodometric titration. Calculate the experimental percent fcopper in the sample and the theoretical mass percent of copper in copper(II) acetate 4. A 0. M Na,S,O, to re by mass o monohydrate.

Answer 1

Given mass of the compound Cu(CH3COO)2.H2O = 0.25 g

Number of moles of Cu(CH3COO)2 = mass of the compound /molar mass of the compound

Number of moles of Cu(CH3COO)2 = 0.25g/199.65g/mol = 1.2522*10^-3 moles

1 mole of Cu(CH3COO)2.H2O Contains 1 mole of Cu

1.2522 * 10^-3 moles of Cu(CH3COO)2.H2O Contains 1.2522*10^-3 moles of Cu

theoritical mass of Cu = 1.2522*10^-3 mol * 63.55 g/mol

theoritical mass of Cu = 0.0796 g

Theoritical mass prercentage = 0.0796/0.25*100 = 31.84%

Number of moles of Na2S2O3 = 11.84 * 10^-3L * 0.105 mol/L

Number of moles of Na2S2O3 = 1.243*10^-3 moles

According to the following equation,

Cu(CH3COO)2.H2O + Na2S2O3 ------> CuS2O3 + 2NaCH3COO

1 mole of Na2S2O3 requires 1 mole of Cu(CH3COO)2

1.243*10^-3 moles of Na2S2O3 requires 1.243*10^-3 mole of Cu(CH3COO)2

mass of Cu(CH3COO)2 = 1.243*10^-3mol*199.65g/mol = 0.2482g

calculated mass of Cu = 1.243*10^-3 mol*63.55g/mol = 0.07899g

Calculated mass of Cu = 0.07899/0.2482*100 = 31.825%