Question
Asked Oct 27, 2019
10. A water solution of sulfuric acid has a density of 1.67 g/mL and is 75 percent HSO
by mass. How many moles of H2SO4 are contained in 400. mL of this solution?
7
5g H2soy
2S04
04
306 -
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10. A water solution of sulfuric acid has a density of 1.67 g/mL and is 75 percent HSO by mass. How many moles of H2SO4 are contained in 400. mL of this solution? 7 5g H2soy 2S04 04 306 -

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Step 1

Given,

Density of solution = 1.67 g/mL

Mass percent of sulfuric acid in the solution = 75 %

Volume of solution = 400 mL

Mass of solution can be calculated as:

Mass
Density
Volume
Mass Density x Volume
Mass 1.67 g/mL x 400 mL
Mass = 668 g
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Mass Density Volume Mass Density x Volume Mass 1.67 g/mL x 400 mL Mass = 668 g

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Step 2

The mass of sulfuric acid can be calculated using the mass percent formula:

Mass of sulfuric acid
% mass
x 100%
Mass of solution
Mass of sulfuric acid
x 100%
75%
668 g
75% X 668 g
Mass of sulfuric acid
100%
Mass of sulfuric acid
501 g
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Mass of sulfuric acid % mass x 100% Mass of solution Mass of sulfuric acid x 100% 75% 668 g 75% X 668 g Mass of sulfuric acid 100% Mass of sulfuric acid 501 g

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Step 3

Therefore, moles of sulfuric ac...

Molar mass of H2SO4
(2x1)32 (4x16)
98 g/mol
Mass
Moles
Molar mass
501 g
Moles
98 g/mol
Moles 5.11 mol
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Molar mass of H2SO4 (2x1)32 (4x16) 98 g/mol Mass Moles Molar mass 501 g Moles 98 g/mol Moles 5.11 mol

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