MEDIUM
Earn 100

Differentiate between end point and equivalence point.

Important Questions on Acids and Bases (AHL)

HARD
A compound 'X' is a weak acid and it exhibits colour change at pH close to the equivalence point during neutralization of NaOH with CH3COOH. Compound 'X' exists in ionized form in basic medium. The compound 'X' is
HARD
Number of moles of dichromate needed to oxidise one mole of Sn2+ is
HARD
In base vs. Acid titration, at the end point methyl orange is present as
EASY

Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R).

Assertion (A) : An aqueous solution of KOH when for volumetric analysis, its concentration should be checked before the use.

Reason (R) : On aging,KOH solution absorbs atmospheric CO2.

In the light of the above statements, choose the correct answer from the options given below.

MEDIUM
50mL of 0.5M oxalic acid is needed to neutralize 25mL of sodium hydroxide solution. What is the amount of NaOH in 50mL of the given sodium hydroxide solution?
HARD
The Plot of pH-metric titration of weak base NH4OH vs strong acid HCl looks like
MEDIUM
By the reaction of aqueous NaHCO3, with which of the following compounds CO2, is produced?
HARD
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 5.7oC 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 kJ mol-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 (Ka=2.0×10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC 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 mL-1 )

The pH of the solution after Expt. 2 is
HARD
0.4 g mixture of NaOH,Na2CO3 and some inert impurities was first titrated with N10HCl using phenolphthalein as an indicator, 17.5 mL of HCl was required at the end point. After this methyl orange was added and titrated. 1.5 mL of same HCl was required for the next end point. The weight percentage of Na2CO3 in the mixture is (Rounded-off to the nearest integer)
MEDIUM
In Tollen's test for aldehyde, the overall number of electron(s) transferred to the Tollen's reagent formula AgNH32+ per aldehyde group to form silver mirror is ___.(Round off to the Nearest integer)
HARD

The titration curve of weak acid vs. strong base with phenolphthalein as indicator is shown below. The Kphenolphthalein =4×10-10

Given: log 2 = 0.3

Question Image

The number of following statement/s which is/are correct about phenolphthalein is _______

A. It can be used as an indicator for the titration of weak acid with weak base.

B. It begins to change colour at pH = 8.4

C. It is a weak organic base

D. It is colourless in acidic medium

 

MEDIUM
An alkali is titrated against acid with methyl orange as an indicator, which of the following is a correct combination?
EASY
Which one of the following pairs of solution is not an acidic buffer?
HARD

20 mL of 0.02 M hypo solution is used for the titration of 10 mL of copper sulphate solution, in the presence of excess of KI using starch as an indicator. The molarity of Cu2+ is found to be _____×10-2M (nearest integer)

Given : 2Cu2++4I-Cu2I2+I2I2 + 2S2O3-2    2I + S4O6-2

EASY
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
The strength of an aqueous NaOH solution is most accurately determined by titrating: (Note: consider that an appropriate indicator is used)
MEDIUM
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:
MEDIUM
2KMnO4+3H2SO4+5H2O2K2SO4+2MnSO4+8H2O+5O2
Find the nonnality of H2O2 solution, if 20 mL of it is required to react completely with 16 mL of 0.02MKMnO4 solution. ( Molar mass of KMnO4=158 g mol-1)
HARD
In a complexometric titration of metal ion with ligand M (Metal ion)+L(Ligand)C (Complex) 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: