## Air contain O2 and N2 in the ratio of  1 : 4. Calculate the ratio of solubilities in term of mole fraction of O2 and N2 dissolved in water at atmospheric pressure and room temperature at which Henry’s constant for O2 and N2 are 3.30 × 10^7 torr and 6.60 × 10^7 torr respectively.

Air contain O2 and N2 in the ratio of  1 : 4. Calculate the ratio of solubilities in term of mole fraction of O2 and N2 dissolved in water at atmospheric pressure and room temperature at which Henry’s constant for O2 and N2 are 3.30 × 10^7 torr and 6.60 × 10^7 torr respectively.

## At what partial pressure, oxygen will have solubility of 0.05 g L-1 in water at 293 K? Henry’s constant (KH) for O2 in water at 293 K is 34.36 k bar. Assume the density of the solution to be same as that of the solvent.

At what partial pressure, oxygen will have solubility of 0.05 g L-1 in water at 293 K? Henry’s constant (KH) for O2 in water at 293 K is 34.36 k bar. Assume the density of the solution to be same as that of the solvent.

## If N2 gas is bubbled through water at 293 K, how many milli moles of N2 gas would dissolve in 1 litre of water. Assume that N2 exerts a partial pressure of 0.987 bar. The KH for N2 at 293 K is 76.48 k bar.

If N2 gas is bubbled through water at 293 K, how many milli moles of N2 gas would dissolve in 1 litre of water. Assume that N2 exerts a partial pressure of 0.987 bar. The KH for N2 at 293 K is 76.48 k bar.

## One litre solution of N/2 HCl is heated in a beaker. It was observed that when the volume of the solution is reduced to 600 mL, 3.25 g of HCl is lost. Calculate the normality of the new solution.

One litre solution of N/2 HCl is heated in a beaker. It was observed that when the volume of the solution is reduced to 600 mL, 3.25 g of HCl is lost. Calculate the normality of the new solution.

## Concentrated sulphuric acid has a density 1.9 g/mL and is 99 % H2SO4 by mass. Calculate the molarity of sulphuric acid.

Concentrated sulphuric acid has a density 1.9 g/mL and is 99 % H2SO4 by mass. Calculate the molarity of sulphuric acid.

## A solution of glucose in water is labelled as 10 % (w/w). The density of the solution is 1.20 g/ml. Calculate the (a) molality (b) molarity   and (c) mole fraction of each component in solution.

A solution of glucose in water is labelled as 10 % (w/w). The density of the solution is 1.20 g/ml. Calculate the (a) molality (b) molarity   and (c) mole fraction of each component in solution.

## Calculate the mole fraction of ethylene glycol (C2H6O2) in a solution containing 20 % of C2H6O2 by mass.

Calculate the mole fraction of ethylene glycol (C2H6O2) in a solution containing 20 % of C2H6O2 by mass.

## The density of a 2.05 M acetic acid in water is 1.02 g/ml. Calculate the molality of the solution

The density of a 2.05 M acetic acid in water is 1.02 g/ml. Calculate the molality of the solution

## Battery acid is 4.27 M H2SO4 and has density of 1.25 g/ml. What is the molality of H2SO4 in the solution?

Battery acid is 4.27 M H2SO4 and has density of 1.25 g/ml. What is the molality of H2SO4 in the solution?

## 100 ml of a solution containing 5 g of NaOH are mixed with 200 ml of M/5 NaOH solution. Calculate the molarity of the resulting solution.

100 ml of a solution containing 5 g of NaOH are mixed with 200 ml of M/5 NaOH solution. Calculate the molarity of the resulting solution.

## Calculate the molarity of a solution of CaCl2 if on chemical analysis it is found that 500 mL of CaCl2 solution contain 1.505 × 10^23 Cl- ions

Calculate the molarity of a solution of CaCl2 if on chemical analysis it is found that 500 mL of CaCl2 solution contain 1.505 × 10^23 Cl- ions

## Calculate the molality of a solution containing 20.7 g of K2CO3 dissolved in 500 mL of the solution (assuming density of solution = 1 g/ml)

Calculate the molality of a solution containing 20.7 g of K2CO3 dissolved in 500 mL of the solution (assuming density of solution = 1 g/ml)

## Calculate the percentage composition in terms of mass of a solution obtained by mixing 300 g of a 25 % and 400 g of a 40 % solution by mass.

Calculate the percentage composition in terms of mass of a solution obtained by mixing 300 g of a 25 % and 400 g of a 40 % solution by mass.

## Calculate the mass percentage of aspirin (C9H8O4) in acetonitrile (CH3CN) when 6.5 g of C9H8O4 is dissolved in 450 g of CH3CN.

Calculate the mass percentage of aspirin (C9H8O4) in acetonitrile (CH3CN) when 6.5 g of C9H8O4 is dissolved in 450 g of CH3CN.

## Quiz 9 for Class 12 Chemistry Chapter 2 Solutions

Quiz 9 for Class 12 Chemistry Chapter 2 Solutions : This quiz consists of 15 questions of 1 mark each. There is no negative marking. You have to complete the quiz in 15 minutes. Your score will be displayed after you submit the quiz.

## Quiz 8 for Class 12 Chemistry Chapter 2 Solutions

Quiz 8 for Class 12 Chemistry Chapter 2 Solutions : This quiz consists of 15 questions of 1 mark each. There is no negative marking. You have to complete the quiz in 15 minutes. Your score will be displayed after you submit the quiz.

## Quiz 7 for Class 12 Chemistry Chapter 2 Solutions

Quiz 7 for Class 12 Chemistry Chapter 2 Solutions : This quiz consists of 15 questions of 1 mark each. There is no negative marking. You have to complete the quiz in 15 minutes. Your score will be displayed after you submit the quiz.

## Quiz 6 for Class 12 Chemistry Chapter 2 Solutions

Quiz 6 for Class 12 Chemistry Chapter 2 Solutions : This quiz consists of 15 questions of 1 mark each. There is no negative marking. You have to complete the quiz in 15 minutes. Your score will be displayed after you submit the quiz.