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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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.   

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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.   

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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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

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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

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Class 12 Chemistry Question and Answer 

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)  

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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)

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Class 12 Chemistry Question and Answer 

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.

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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.

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Class 12 Chemistry Question and Answer 

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

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

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