20 mL of 0.1 M acetic acid is mixed with 50 mL of potassium aceta

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 Multiple Choice QuestionsMultiple Choice Questions

201.

Which one of the following salts give an acidic solution in water?

  • CH3COONa

  • NH4Cl

  • NaCl

  • CH3COONH4


202.

The equilibrium constant for the reaction 

SO2(g)+ 12O2(g)   SO3(g) is5× 10-2 atm. The equilibnum constant of the reaction 2SO3(g) 2SO2(g) + O2(g) wouldbe.

  • 100 atm

  • 200 atm

  • 4 × 102 atm

  • 6.25 × 104 atm


203.

If the equilibrium constant for the reaction,

H2(g)+ I2(g)  2HI (g) is K. what is the equilibrium constant of HI(g)  12H2(g) +12I2(g) ?

 

  • 1/K

  • √K

  • K

  • 1/√K


204.

The pH of 0.01 M solution of acetic acid is 5.0. What are the values of [H+] and Ka respectively?

  • 1 × 10-5M, 1× 10-8

  • 1 × 10-5M, 1× 10-9

  • 1 × 10-4M, 1 × 10-8

  • 1 × 10-3M, 1 × 10-8


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205.

pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic acid is added to 250 mL of a buffer solution of acetic acid and potassium acetate at 27°C. The buffer capacity of the solution is

  • 0.1

  • 10

  • 1

  • 0.4


206.

The equilibnum constant for the given reaction is 100.

N2 (g) + 2O2 (g)  2NO2 (g)

What is the equilibrium constant for the reaction given below?

NO2 (g)  12N2 (g) + O2 (g)

  • 10

  • 1

  • 0.1

  • 0.01


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207.

20 mL of 0.1 M acetic acid is mixed with 50 mL of potassium acetate. Ka of acetic acid = 1.8 × 10-5 at 27°C. Calculate concentration of potassium acetate if pH of the mixture is 4.8.

  • 0.1 M

  • 0.04 M

  • 0.4 M

  • 0.02 M


B.

0.04 M

Let the concentration of potassium acetate is x.

From Henderson's equation,

pH = pKa + logsaltacid

4.8 = -log (1.8 × 10-5) + log x × 5020 × 0.1 M

4.8 = 4.74 + log 25 x

log 25x = 0.06

     25x = 1.148

         x = 0.045 M


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208.

If the equilibrium constant for the reaction,

2AB  A2 + B2 

is 49, what is the equilibrium constant for AB  12A1 + 12A2 ? 

  • 7

  • 17

  • 24.5

  • 49


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209.

The pH of 0.05 M acetic acid is Ka = 2 × 10-5)

  • 2

  • 11

  • 10-3

  • 3


210.

The degree of ionization of 0.10 M lactic acid is 4.0%

The value of Kc is

  • 1.66 × 10-5

  • 1.66 × 10-4

  • 1.66 × 10-3

  • 1.66 × 10-2


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