Molality

Q.

Can the Molarity and molality of a given solution (solute + solvent) be equal?

1. True

2. False

Q.

Which of the following formulae are correctly mentioned?

1. $Molarity=\frac{Numberofmolesofsolvent}{volumeofsolvent\left(litres\right)}$

2. $Molarity=\frac{Numberofmolesofsolvent}{volumeofsolute\left(kg\right)}$

3. $Molarity=\frac{Numberofmolesofsolute}{volumeofsolution\left(litres\right)}$

4. $Molality=\frac{Numberofmolesofsolute}{Massofsolvent\left(kg\right)}$

Q.

What are Molarity and molality represented by respectively?

1. m, M

2. M, m

3. Mo, mol

4. ar, al

Q.

Calculate Molality (in $M$) of a solution in which 36 gm glucose is dissolved in 500 gm water.

1. 0.8

2. 0.4

3. 0.2

4. 0.36

Q. Dissolving 120 g of urea (mol. wt. 60) in 1000 g of water gave a solution of density 1.15 g/mL. The molarity of the solution is

1. 2.05 M
2. 2.22 M
3. 2.00 M
4. 1.78 M

Q. In which mode of expression, the concentration of a solution remains independent of temperature?
(IIT-JEE, 1988)

1. Molarity
2. Normality
3. Formality
4. Molality

Q.

Molality (in mol/kg) of a solution in which 0.13 mole of solute is dissolved in 500 gm of water is:

1. 13

2. 1.3

3. 2.6

4. 0.26

Q.

Which of the following variables are sufficient to calculate molality?

1. Mass of solute

2. Moles of solute

3. Moles of solvent

4. Mass of solvent

Q.

Do you know the molecular mass of glucose and its structural formula?

1. 160,

2. 180,

3. 180,

4. 180,

Q. Molarity of $H_{2}S{O}_4$ is 18M. Its density is 1.8 g/ml. Hence molality is

1. 36
2. 200
3. 500
4. 18