Answer :
Below are the step-by-step procedure to prepare 500 mL of a 2.00 M solution of aqueous H2SO4 from deionized water and concentrated H2SO4, as provided in the options:
Steps to prepare Solution:
a. Weigh 98.1 g of concentrated sulfuric acid into a 500 ml beaker. Slowly add deionized water to the beaker, with occasional swirling until the liquid reaches the 500 mL mark.
b. Weigh 98.1 g of concentrated sulfuric acid into a 500 mL volumetric flask, slowly add deionized water to the mark and mix.
c. Weigh 98.1 g of concentrated sulfuric acid into a 100 ml beaker, then slowly pour the H2SO4 into a 500 ml beaker with about 250 mL deionized water in it. Pour this solution into a 500 mL volumetric flask and fill to the mark with deionized water and mix.
d. Weigh 446.6 g of deionized water into a 500 mL volumetric flask, fill to the mark with concentrated sulfuric acid and mix.The correct answer to this question is option b. Weigh 98.1 g of concentrated sulfuric acid into a 500 mL volumetric flask, slowly add deionized water to the mark and mix.
The molarity of a solution is defined as the number of moles of solute per litre of solution. The formula to calculate molarity is given as:
Molarity (M) = Number of moles of solute (n) / Volume of solution in litres (V)
Liter (L) is the standard unit for measuring volume in the International System of Units (SI), and it is equal to one cubic decimetre (1 dm³) or 1000 milliliters (1000 mL).
Therefore, the volume of the solution is in liters or millilitres.
We are required to prepare 500 mL of a 2.00 M solution of aqueous H2SO4 using deionized water and concentrated H2SO4. We can use the molarity formula to calculate the number of moles of H2SO4 needed for the solution.
To calculate the number of moles of H2SO4, we use the formula:
Number of moles (n) = Molarity (M) × Volume of solution (V) in litres / Molar mass (Mm) of H2SO4
The molar mass of H2SO4 = (2 × 1) + (1 × 32) + (4 × 16) = 98 g/mol
To obtain 500 mL of 2.00 M H2SO4, the number of moles of H2SO4 required is:
Number of moles (n) = 2 × 0.5 L = 1 mol
The density of concentrated H2SO4 is given as 1.84 g/mL. To calculate the volume of concentrated H2SO4 required, we use the formula:
Mass (m) = Density (ρ) × Volume (V) of H2SO4
Therefore,Volume of concentrated H2SO4 = Mass of H2SO4 / Density of H2SO4 = 98.1 g / 1.84 g/mL = 53.26 mLThis means that we require 53.26 mL of concentrated H2SO4 to prepare the solution.
To prepare the solution, we can weigh 98.1 g of concentrated sulfuric acid into a 500 mL volumetric flask, slowly add deionized water to the mark and mix.
Learn more about Molarity (M).
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