Question

. Commercially available sulphuric acid contains 91% acid by mass and has a density of 1.83g mL-1 (i) Calculate the molarity of the solution (ii) volume of concentrated acid required to prepare 3.5L of 0.50 M H2SO4

Answer 1

Answer:91 % acid by mass means 91 g acid in 100 g solution.

Density = 1.83 g/mL

Volume of solution = mass/density

= 91/1.83

= 49.73 mL

Molar mass sulpuric acid, H2SO4 = 2 x 1 + 32 + 4 x 16 = 98 g/mol

Number of moles of sulphuric acid = mass/molar mass

= 91/98

= 0.93

Molarity = number of moles/ volume of solution in litres

= 0.93/0.0497

= 18.71 M

Applying,

M1V1= M2V2

18.71 x V = 0.5 x 3.5

V = 0.093 L

= 93 mL

Thus, 93 ml of concentrated acid is required to prepare 3.5L of 0.50 M H2SO4

Explanation:

Answer 2

Answer:Here is your answer

Explanation: