EASY

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The titration curve for titration of a $50 mL$ solution of a diprotic acid with $0.1 M NaOH$ is shown below.

$K_{a 1}$ and $K_{a 2}$ are approximately

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Important Questions on Equilibrium

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of

{5.7}^{o} C

was measured for the beaker and its contents (Expt.1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant

(- 57.0 k J m o l^{- 1})

, this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid

(K_{a} = 2.0 \times 10^{- 5})

was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of

{5.6}^{o} C

was measured. (Consider heat capacity of all solutions as

4.2 J g^{- 1} K^{- 1}

and density of all solutions as

1.0 g m L^{- 1}

)

The pH of the solution after Expt. 2 is

EASY

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Incorrect statement for the use of indicator in acid-base titration is:

EASY

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

100 mL

0.1 M HCl

is taken in a beaker and to it

100 mL

0.1 M NaOH

of is added in steps of

2 mL

and the

pH

is continuously measured. Which of the following graphs correctly depicts the change in

pH

EASY

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is

10^{- 5}

, the ratio of salt to acid concentration in the buffer solution will be:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Given below are two statements:
Statement I : In the titration between strong acid and weak base methyl orange is suitable as an indicator.
Statement II : For titration of acetic acid with $\mathrm{NaOH}$ phenolphthalein is not a suitable indicator.
In the light of the above statements, choose the most appropriate answer from the options given below:

EASY

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Which one of the following pairs of solution is not an acidic buffer?

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

In an acid-base titration,

0.1 M H C l

solution was added to the

N a O H

solution of unknown strength. Which of the following correctly shown the change of

p H

of the titration mixture in this experiment?
Question Image

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

If the

pH

of a solution containing

10 mL

0.5 M {CH}_{3} COOH

and

10 mL

0.25 M NaOH

5

. What is the

{pK}_{a}

of the acid?

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

In base vs. Acid titration, at the end point methyl orange is present as

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

A compound '

X

' is a weak acid and it exhibits colour change at

pH

close to the equivalence point during neutralization of

NaOH

with

{CH}_{3} COOH

. Compound '

X

' exists in ionized form in basic medium. The compound '

X

' is

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Which will make basic buffer?

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

In a complexometric titration of metal ion with ligand

M (M e t a l i o n) + L (L i g a n d) \to C (C o m p l e x)

end point is estimated spectrophotometrically (through light absorption). If 'M' and 'C' do not absorb light and only 'L' absorbs then the titration plot between absorbed light

(A)

versus volume of ligand 'L'

(V)

would look like:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

The strength of an aqueous

N a O H

solution is most accurately determined by titrating: (Note: consider that an appropriate indicator is used)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

20 ml

{0.1 M H}_{2} {SO}_{4}

solution is added to

30 mL

0 .2 M {NH}_{4} OH

solution. The

pH

of the resultant mixture is:

[{pk}_{b} of {NH}_{4} OH = 4 .7]

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

A solution of

0.1

mole of

{CH}_{3} {NH}_{2} (K_{b} = 5 \times 10^{- 4})

and

0.08 mole

HCl

is diluted to one litre, then the

pOH

of the solution is

(\log 1.25 = 0.1)

EASY

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

Among the following, the correct statement is

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

2 {KMnO}_{4} + 3 H_{2} {SO}_{4} + 5 H_{2} O_{2} \to K_{2} {SO}_{4} + 2 {MnSO}_{4} + 8 H_{2} O + 5 O_{2}

Find the nonnality of

H_{2} O_{2}

solution, if

20 mL

of it is required to react completely with

16 mL

0.02 {MKMnO}_{4}

solution. ( Molar mass of

{KMnO}_{4} = 158 g {mol}^{- 1}

)

HARD

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

The Plot of

pH

-metric titration of weak base

{NH}_{4} OH

vs strong acid

HCl

looks like

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

An alkali is titrated against acid with methyl orange as an indicator, which of the following is a correct combination?

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Titrations of Acids and Bases

50 mL

0 .5 M

oxalic acid is needed to neutralize

25 mL

of sodium hydroxide solution. What is the amount of

NaOH

50 mL

of the given sodium hydroxide solution?

The titration curve for titration of a 50 mL solution of a diprotic acid with 0.1 M NaOH is shown below. Ka1 and Ka2 are approximately

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

The titration curve for titration of a $50 mL$ solution of a diprotic acid with $0.1 M NaOH$ is shown below.

$K_{a 1}$ and $K_{a 2}$ are approximately