The density of an aqueous solution of sulfuric acid is 1.67 g/mL and the concent

Question

The density of an aqueous solution of sulfuric acid is 1.67 g/mL and the concentration is 3.31 m. What is the concentration of this solution in molarity? Marks: 1 Answer. 23 Marks: 1 The density of an aqueous solution of sulfuric acid is 1.45 g/mL and the concentration is 2.28 M. What is the concentration of this solution in mole fraction? Answer: 24 Marks: 1 The density of an aqueous solution of sulfuric acid is 1.26 g/mL and the concentration is 3.49 M. What is the concentration of this solution in percent by mass? Answer:

Explanation / Answer

Ans 22

Step 1. Make an assumption.

Assume you have 1 kg of solvent (water).

Step 2. Find the total mass of H2SO4.

3.31 m means 3.31moles /kg solvent (water).

3.31X 98.079 g/mole = 324.64 grams .

Step 3. Calculate the total grams of the solution.

1000 grams solvent (water) + 324.64 grams H2SO4 = 1324.64 grams solution.

Step 4. Calculate the volume (Liters) of solution.

1324.64 grams X 1mL/1.67grams (density) = 793.19 mL = 0.793 L

Step 5. Calculate the molarity.

3.31 moles solute / 0.793 L = 4.17 M

Ans 23

Moles of H2SO4 in 1000 ml of water is 2.28.

Moles of water = 1000 /18 = 55.55 moles.

Mole fraction = moles of solute/moles of solute+moles of solvent

=2.28/(2.28+55.5)

=0.039

Ans 24

Mass percent=mass of solute/mass of solution *100

let 1000mL of h2so4 contains 3.49moles

3.49 moles=3.49*98.079

=342.29g

mass of solution=density*volume

=1.26*1000

=1260g

mass percente=342.29/1260 *100

27.14%

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