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The curve in the figure shows the variation of the $pH$ during the course of the titration of a weak acid $HA$ , with a strong base ( $NaOH$ ). At which point in the titration curve is the concentration of the acid equal to that of its conjugate base?

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Important Questions on Transfer

MEDIUM

50 mL

0 .2 M

ammonia solution is treated with

25 mL of 0.2 M HCl

. If

{pK}_{b}

of ammonia solution is

4.75

, the

pH

of the mixture will be:

EASY

Chemistry>Change>Transfer>Titration

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

EASY

Chemistry>Change>Transfer>Titration

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>Change>Transfer>Titration

An acidic buffer is obtained on mixing:

MEDIUM

Chemistry>Change>Transfer>Titration

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:

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Chemistry>Change>Transfer>Titration

Which will make basic buffer?

EASY

Chemistry>Change>Transfer>Titration

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

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Chemistry>Change>Transfer>Titration

Which of the following mixtures will have the lowest pH at $298 K ?$

HARD

Chemistry>Change>Transfer>Titration

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

HARD

Chemistry>Change>Transfer>Titration

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

HARD

Chemistry>Change>Transfer>Titration

A solution of $0.1 M$ weak base $(B)$ is titrated with $0.1 M$ of a strong acid $(HA)$ . The variation of $pH$ of the solution with the volume of $HA$ added is shown in the figure below. What is the ${pK}_{b}$ of the base? The neutralisation reaction is given by $B + HA \to {BH}^{+} + A^{-}$ .

Question Image

HARD

Chemistry>Change>Transfer>Titration

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:

HARD

Chemistry>Change>Transfer>Titration

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)

HARD

Chemistry>Change>Transfer>Titration

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

MEDIUM

Chemistry>Change>Transfer>Titration

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>Change>Transfer>Titration

A buffer solution can be prepared by mixing equal volumes of

EASY

Chemistry>Change>Transfer>Titration

Among the following, the correct statement is

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Chemistry>Change>Transfer>Titration

The Plot of

pH

-metric titration of weak base

{NH}_{4} OH

vs strong acid

HCl

looks like

MEDIUM

Chemistry>Change>Transfer>Titration

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

MEDIUM

Chemistry>Change>Transfer>Titration

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 curve in the figure shows the variation of the pH during the course of the titration of a weak acid HA, with a strong base (NaOH). At which point in the titration curve is the concentration of the acid equal to that of its conjugate base?

Important Questions on Transfer

Learn and Prepare for any exam you want !

The curve in the figure shows the variation of the $pH$ during the course of the titration of a weak acid $HA$ , with a strong base ( $NaOH$ ). At which point in the titration curve is the concentration of the acid equal to that of its conjugate base?