How many millilitre of 0.5 M H2SO4 are needed to dissolve 0.5 g of Cu(II) carbonate?
Correct answer: C. 8.1
- A. 6.01
- B. 4.5
- C. 8.1
- D. 11.1
Explanation
To determine the volume of 0.5 M H2SO4 needed, we first calculate the moles of Cu(II) carbonate (CuCO3) using its molar mass (123.55 g/mol). For 0.5 g of CuCO3, the moles are 0.5 g / 123.55 g/mol = 0.00405 moles. The balanced chemical equation shows that one mole of CuCO3 reacts with one mole of H2SO4. Therefore, 0.00405 moles of H2SO4 are required. Given the concentration of the solution is 0.5 M, the volume needed is moles/concentration = 0.00405 moles / 0.5 M = 0.0081 L or 8.1 mL. The other options either underestimate or overestimate the volume based on incorrect stoichiometric calculations.
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