Solutions Test

Result

Solutions Test - 5

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Weekly Quiz Competition

Question 1
1 / -0

If the density of 96% H₂SO₄ is 1.83 g/mL, then the volume required to prepare 2.0 L of 3.0 M H₂SO₄solution is

A
334.7 mL

B
33.47 mL

C
3.347 mL

D
0.334 mL

Solution

Number of moles of solute = Molarity x volume of solution (L)
= 3 x 2.0 = 6.0 moles
Mass of H₂SO₄ = Number of moles x molar mass of H₂SO₄
= 6.0 x 98 = 588 g
Mass of 96% of H₂SO₄ solution containing 588 g of H₂SO₄ = 588 x 100/96 = 612.5 g
Volume of 96% of H₂SO₄ solution weighing 612.5 g = Mass/Density
= 612.5/1.83 = 334.7 mL
Question 2
1 / -0

Assume an ideal solution formed by A and B. Pure component A has vapour pressure of 0.150 atm and pure B has vapour pressure of 0.350 atm at 25°C. In distillation of a solution, that is 50% A and 50% B by moles,

A
the vapour is richer in A than in the solution

B
the vapour has the same composition as the solution

C
the vapour is richer in B than in the solution

D
None of the above

Solution

The vapour pressure of B is more than that of A at the same temperature. So, B being volatile than A, the distillate of the two will be richer in B.
Question 3
1 / -0

During the study of elevation in boiling point of aqueous solution of glucose, the value of K_b for water is found to be 0.51 K kg mol^-1. The value of K_b in K kg mol^-1 that can be expected from the aqueous solution of K₄[Fe(CN)₆] is

A
0.51

B
2 x 0.51

C
5 x 0.51

D
3 x 0.51

Solution

K_b is independent of the nature of the solute.