A 34.0% sulfuric acid solution had a density of 1.25 g/mL. How many grams of H2SO4 are contained in 1.00 L of this solution?

Question

A 34.0% sulfuric acid solution had a density of 1.25 g/mL. How many grams of [latex]H_2SO_4[/latex] are contained in 1.00 L of this solution?

Accepted Answer

READ Knowns d = 1.25 g/mL
V = 1.00 L
34.0% [latex]H_2SO_4[/latex] solution
Solving for: mass [latex]H_2SO_4[/latex]
PLAN Find the mass of the solution from the density and then use the mass percent to determine the mass of [latex]H_2SO_4[/latex]

CALCULATE d = mass/V

mass of solution = [latex](\frac{1.25 g}{\cancel {mL}}) (1.00 imes 10^3 \cancel {mL}) =[/latex] 1250 g (solution)

mass percent =[latex](\frac{g solute}{g solution}) 100 [/latex]

g solute = [latex]\frac{(mass percent) (g solution)}{100} [/latex]

g solute = [latex]\frac{(34.0) (1250 g)}{100} [/latex]=425 g [latex]H_2SO_4[/latex]

Therefore, 1.00 L of 34.0% [latex]H_2SO_4[/latex] solution contains 425 g [latex]H_2SO_4[/latex]

Question 14.4: A 34.0% sulfuric acid solution had a density of 1.25 g/mL. H...

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