Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 16

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IMPORTANT

Earn 100

Van't Hoff's equation giving the effect of temperature on chemical equilibrium is represented as

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Important Questions on Equilibrium

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IMPORTANT

Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 17

Molarity of

A^{-}

ions in

0.01 M HA is [K_{a} = 4 \times 10^{- 10}]

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IMPORTANT

Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 18

In general, dissociation constant of a weak monoprotic acid is numerically equal to the dissociation constant of its conjugate base. The

pH

of

0.1 M

solution of this acid is

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Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 19

HCOOH

and

{CH}_{3} COOH

solutions have equal

[H^{+}]

. If

\frac{K_{a_{1}}}{K_{a_{2}}}

(ratio of acid ionisation constants) is

4

, then their molar concentration ratio will be

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IMPORTANT

Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 20

Find the

pH

of a decinormal solution of

{NH}_{4} OH

which is

20 %

ionised (

\log 5 = 0.7

) at

0 ° C . (K_{w} = 10^{- 15})

.

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Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 21

The degree of dissociation of

A_{x} B_{y}

electrolyte with concentration

C

and dissociation constant

K

is: (Given,

α ≪ 1

)

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Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 22

The pH of the solution obtained on mixing equal volumes of

0.1 N KOH and 0.1 N Ba {(OH)}_{2}

is

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Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 23

' V' mL

water was added to a

50 mL

solution of

0.01 M Ba (OH)_{2}

, such that the final

pH

is

12

. The value of

' V'

is

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IMPORTANT

Chemistry Crash Course JEE Main>Chapter 12 - Equilibrium>Level 2>Q 24

To $100 mL$ of an aqueous $HCl$ solution of $pH 1.0, 900 mL$ of distilled water is added. Then $pH$ of the resulting solution is