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Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% by weight H2SO4. What is the molality of this acid? What is its molarity? 

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Greg Montoya
Greg MontoyaLv10
21 Oct 2020

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Related questions

Common commercial acids and bases are aqueous solutions with the following properties:

 

Density (g/cm3)

Mass percent of solute

Hydrochloric acid

1.19

38

Nitric acid

1.42

70

Sulfuric acid

1.84

95

Acetic acid

1.05

99

Ammonia

0.95

28

 

Calculate the molarity, molality, and mole fraction of each of the preceding reagents.

A sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm3. Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of H2SO4 in this solution.

Concentrated sulfuric acid (18.4-molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20-molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage batteries for automobiles. (a) Calculate the volume of concentrated acid required to prepare 1.00 liter of 5.20-molar H2SO4. (b) Determine the mass percent of H2SO4 in the original concentrated solution. (c) Calculate the volume of 5.20-molar H2SO4 that can be completely neutralized with 10.5 grams of sodium bicarbonate, NaHCO3. (d) What is the molality of the 5.20-molar H2SO4?

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