Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 62

MEDIUM

NEET

IMPORTANT

Earn 100

$0.1 M$ solution of a weak base $BOH$ has a $pH$ of $8$ when it is half neutralized with $0.1 M {HNO}_{3}$ . The value of $K_{b}$ of the base is:

45% studentsanswered this correctly

Important Questions on Equilibrium

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 63

100 ml

of

0.1 M

of acetic acid,

({pK}_{a} = 5.1)

is titrated against

100 ml

of

0.1 M

ammonia solution

({pK}_{b} = 5.1) the pH

of solution at equivalence point at

0 ° C ({pK}_{w} = 15)

is:

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 64

The $pH$ of solution in which equal volume of $0.1 M NaCN$ and $0.05 M HCl$ are added is; $({pK}_{a} of HCN = 6)$

EASY

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 65

200 ml

of

0.1 M {CH}_{3} COOH

is mixed with

200 ml

of

0.1 M NaOH .

The resulting solution

EASY

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 66

On adding a catalyst to a reversible reaction,

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 67

At the temperature

T

, a compound

{AB}_{2} (g)

dissociates, according to the reaction

2 {AB}_{2} (g) ⇌ 2 AB (g) + B_{2} (g)

with a degree of dissociation

x

, which is small compared with unity. The expression for

K_{p}

in terms of

x

and the total pressure,

P

is

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 68

$X_{2} + X^{-} ⇌ X_{3}^{-} (X = Iodine)$

This reaction is set up in an aqueous medium. The reaction started with $1 mol$ of $X_{2}$ and $0.5 mol$ of $X^{-}$ in a $1 L$ flask. After equilibrium is reached, the excess ${AgNO}_{3}$ gave $0.25 mol$ of yellow precipitate. The equilibrium constant is:

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 69

One mole of

N_{2} O_{4} (g) at 300 K

is kept in a closed vessel at

1 atm

pressure. It is heated to $600 K$ when

20 %

by mass of

N_{2} O_{4} (g)

decomposes to

{NO}_{2} (g)

. The resultant pressure is:

MEDIUM

NEET

IMPORTANT

Chemistry Crash Course NEET>Chapter 5 - Equilibrium>Level 2>Q 70

For the reaction equilibrium,

2 NOBr (g) ⇌ 2 NO (g) + {Br}_{2} (g),

if

P_{{Br}_{2}} = \frac{P}{9}

at equilibrium and

P

is total pressure, then the ratio

\frac{K_{P}}{P}

is equal to: (assume that equilibrium was achieved starting with only

NOBr

)