Question

Aqueous sulfuric acid
will react with solid sodium hydroxide
to produce aqueous sodium sulfate
and liquid water
. Suppose 53.0 g of sulfuric acid is mixed with 24. g of sodium hydroxide. Calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

Answer 1

Answer on Question #82114 - Chemistry - General Chemistry

Question:

Aqueous sulfuric acid

will react with solid sodium hydroxide

to produce aqueous sodium sulfate

and liquid water

. Suppose 53.0 g of sulfuric acid is mixed with 24. g of sodium hydroxide. Calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

Solution:

H2SO4 + 2NaOH → Na2SO4 + 2H2O

$$n = m / M$$ $$n(\mathrm{H_2SO_4}) = 31.4\ \mathrm{g} \times 1\ \mathrm{mole} / 98.08\ \mathrm{g} = 0.32\ \mathrm{moles};$$ $$n(\mathrm{NaOH}) = 40.\ \mathrm{g} \times 1\ \mathrm{mole} / 40.00\ \mathrm{g} = 1.0\ \mathrm{moles};$$

1 mole of NaOH would react with 0.5 mole of H2SO4, but there's not that much.

0.32 moles H2SO4 reacts with $2 \times 0.32 = 0.64$ moles NaOH, so H2SO4 reacts completely, and 1.0 - $0.640 = 0.36$ moles NaOH will be unreacted.

0.0 g of H2SO4 will be left over.

Answer: 0.0 g.

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