How many millilitres of 0.5 M H2SO4 are needed to dissolve 0.5g of copper sulphate
Answers
Answered by
65
Sol . The balanced chemical reaction is :
CuCO3 + H2SO4 → CuSO4 + H2O + CO2
Millimol of CuCO3 = (0.5 × 1000)/123.5
= 4.048
⇒ millimol of H2SO4 required = 4.048
∵ millimol = Molarity × Volume (in mL)
⇒ Vol = 4.048/0.50 = 8.1 mL
CuCO3 + H2SO4 → CuSO4 + H2O + CO2
Millimol of CuCO3 = (0.5 × 1000)/123.5
= 4.048
⇒ millimol of H2SO4 required = 4.048
∵ millimol = Molarity × Volume (in mL)
⇒ Vol = 4.048/0.50 = 8.1 mL
Answered by
8
Answer:
CuCO3 + H2SO4 → CuSO4 + H2O + CO2
For 123.5 g of Cu(II) carbonate 98 g of H2SO4 are required.
.'. 0.5 g of Cu(II) carbonate = 98 x 0.5/123.5 g of H2SO4 are required.
Weight of required H2SO4 = 0.39676 g
Weight = mol.wt x molarity x volume in mL/1000 = 0.39676 = 98 x 0.5 x V/1000
Volume of H2SO4 solution = 8.097 mL
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