How many millilitres of 0.5M H _ 2 SO _ 4 are needed to dissolve 0.5g of copper(II)carbonate? Report your answer by rounding it up to nearest integer.

Correct answer: 8 The balanced chemical reaction is: CuCO 3 + H 2 SO 4 → CuS0 4 + H 2 O + CO 2 milli mol of CuCO 3 = (0.5 × 1000)/(123.5) = 4.048 mM milli mol of H 2 SO 4 required = 4.048 mM = Molarity x Volume (in mL) Volume = (4.048)/(0.50) = 8.1 mL

NTA Abhyas 2020

Exam: NTA Abhyas
Year: 2020
Subject: Chemistry
Chapter: Redox Reactions

NTA Abhyas 2020 · Chemistry · Redox Reactions

How many millilitres of 0.5M H _ 2 SO _ 4 are needed to dissolve...

How many millilitres of

\text{0}\text{.5}\text{M}{H}_{2} {\text{SO}}_{4}

are needed to dissolve

\text{0}\text{.5}\text{g}

of copper(II)carbonate?
Report your answer by rounding it up to nearest integer.

Correct answer

Step-by-step solution

The balanced chemical reaction is:
CuCO₃ + H₂SO₄→ CuS0₄ + H₂O + CO₂
milli mol of CuCO₃ =

\dfrac{0.5 \times 1000}{123.5}

= 4.048 mM
milli mol of H₂SO₄ required = 4.048 mM
= Molarity x Volume (in mL)
Volume =

\dfrac{4.048}{0.50}

= 8.1 mL

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