MCQ Questions for Class 11 Medical Chemistry Equilibrium Quiz 3

If degree of ionization

$(\alpha )$ of a weak electrolyte

$AB$ is very less, then

$\alpha$ is

0%
directly proportional to the square root of volume of solution
0%
inversely proportional to the dilution
0%
inversely proportional to the square root of concentration
0%
directly proportional to concentration

Explanation

$\alpha=\sqrt{\frac{K}{C}}=\sqrt{\frac{K\times V}{n}}$

So directly proportional to the square root of the volume of solution and inversely proportional to the square root of concentration.

1M NaCl and 1M HCl are present in an aqueous solution . The solution is:

0%
Not a buffer solution with pH <7
0%
Not a buffer solution with pH >7
0%
A buffer solution with pH <7
0%
A buffer solution with pH >7

Explanation

Buffer can accept and donate protons at the same time and

$HCl$ is an acid. So, it has

$pH<7$ .

So, this is not a buffer and the solution will be acidic.

Hence, the correct option is

$A$

The solubility of

$CaF_{2}(K_{sp} = 3.4 \times 10^{-11})$ in 0.1M solution of NaF would be:

0%
$3.4 \times 10^{-12}M$
0%
$3.4 \times 10^{-10}M$
0%
$3.4 \times 10^{-9}M$
0%
$3.4 \times 10^{-13}M$

Explanation

The dissociation equilibrium of calcium fluoride is as given below.

$CaF_2 \rightleftharpoons \underset {x}{Ca^{2+}}+ \underset {2x} {2F^-}$

The dissociation of NaF is as shown below.

$NaF \rightarrow \underset {0.1} {Na^+} + \underset{0.1} {F^-}$

Thus total fluoride ion concentration is

$2x+0.1$ M but

$2x<<<0.1$ .

Hence, 2x is neglected and the total fluoride ion concentration is 0.1 M.

The expression for the solubility product is as follows.

$K_{sp}=[Ca^{2+}][F^-]^2$

Substitute values in the above expression:

$3.4 \times 10^{-11}=x(0.1)^2$ or

$x=3.4 \times 10^{-9}$ M.

Hence, option C is correct.

$NH_{4}OH$ is weak base but it becomes still weaker in the aqueous solution of :

0%
0.1 M HCl
0%
0.1 M $NH_{4} Cl$
0%
0.1 M $H_{2}SO_{4}$
0%
0.1 M $CH_{3}COOH$

Explanation

Common ion effect is observed when a solution of weak electrolyte is mixed with a solution of strong electrolyte which provides an ion common to that provided by a weak electrolyte.

Ammonium hydroxide is a weak electrolyte and ammonium chloride is a strong electrolyte. Ammonium chloride provides ammonium ion which is common to that provided by ammonium hydroxide.

Thus the pair

$NH_{4} OH + NH_{4} Cl$ shows common ion effect. Ammonium chloride suppresses the ionization of ammonium hydroxide.

Hence, ammonium hydroxide becomes still weaker in the presence of an aqueous solution of ammonium chloride.

Which of the following mixture is not a buffer solution?

0%
100ml of 0.5 $N - CH_{3}COOH +$ 100 ml of 0.05 N- NaOH
0%
100ml of 0.5 $N-NH_{4}OH +$ 100ml of 0.5 N-HCl
0%
100 ml of 0.5 $N-NH_{4}OH +$ 10 ml of 0.5 $N-H_{2}SO_{4}.$
0%
300 ml of 0.5 $N-NH_{4}OH +$ 200 ml of 0.5 $N-HNO_{3}$

Explanation

Basic buffer solution is prepared by mixing a weak base and its salt with strong acid.
In the mixture containing 100ml of 0.5 N

$NH_4OH$ + 100ml of 0.5 N-HCl, equal number of moles of ammonium hydroxide and hydrochloric acid are present.
They completely neutralize each other to form salt ammonium chloride. Thus weak base ammonium hydroxide is not present in the mixture.
Hence, this mixture is not a buffer solution.

Match List-1 with List-2.

List -1 List-2
A)

$CH_{3}COONa + CH_{3}COOH$ 1)Acidic due to cationic hydrolysis
B)

$NH_{4}Cl + NH_{4}OH$ 2)Basic due to anionic hydrolysis
C) aqueous

$AlCl_{3}$ 3) Basic buffer solution
D) aqueous

$Na_{2}CO_{3}$ 4)Acidic buffer solution

0%
A - 1 ; B - 2 ; C - 3 ; D - 4
0%
A - 4 ; B - 3 ; C - 1 ; D - 2
0%
A - 2 ; B - 3 ; C - 1 ; D - 4
0%
A - 4 ; B - 3 ; C - 2 ; D - 1

Explanation

Buffer solutions are a mixture of acid and its conjugate base or base and its conjugate acid.
The mixture of acid and conjugate base is called acidic buffer solutions
The mixture of base and conjugate acid is called basic buffer solutions.
Weak acid salts and weak basis salts suffer hydrolysis making their aqueous solutions acidic or basic depending on the type of salt.

$AlCl_3 + H_2O \rightarrow Al\left(OH\right)_3 + Cl^- + H^+$
Similarly for

$Na_2CO_3$ .

The

$K_{sp}$ for AgCl is

$2.8\times 10^{-10}$ at a given temperature. The solubility of AgCl in 0.01 molar HCl solution at this temperature will be :

0%
$2.8\times 10^{-12}mol L^{-1}$
0%
$2.8\times 10^{-8}mol L^{-1}$
0%
$5.6\times 10^{-8}mol L^{-1}$
0%
$2.8\times 10^{-4}mol L^{-1}$

Explanation

The chloride ion concentration in 0.01M HCl will be 0.01 M.
The chloride ion concentration due to dissociation of AgCl is neglected due to very low value of solubility product of AgCl.
The expression for the solubility product is as shown below.

$K_{sp}=[Ag^+][Cl^-]$
Substitute values in the above expression.

$2.8 \times 10^{-10}=[Ag^+] \times 0.01$
Hence,

$[Ag^+]= \frac {2.8 \times 10^{-10}} {0.01}=2.8 \times 10^{-8}$ mol/L.

$0.004$ M solution of

$Na_{2}SO_{4}$ is isotonic with a

$0.010$ M solution of glucose at same temperature. The apparent degree of dissociation of

$Na_{2}SO_{4}$ is:

0%
$25$ %
0%
$50$ %
0%
$75$ %
0%
$85$ %

Explanation

The reaction for the dissociation of isotonic solutions is as given below.

$\underset {0.004-x} {Na_2SO_4} \rightleftharpoons \underset {2x}{2Na^+}+ \underset {x} {SO_4^{2-}}$
Both the solutions are isotonic.
Hence,

$(0.004-x)+2x-x=0.01$ or

$x=3 \times 10^{-3}$ .
Percentage dissociation

$= \dfrac {3 \times 10^{-3}} {0.004} \times 100=75$ %.

Which of the following mixture will act as buffer?

0%
$H_{2}CO_{3}+NaOH ( 3 : 2 mole ratio)$
0%
$H_{2}CO_{3}+NaOH ( 3 : 4 mole ratio)$
0%
$NH_{4}OH +HCl ( 5 : 4 mole ratio)$
0%
$NH_{4}OH +HCl ( 4 : 5 mole ratio)$

Which of the following statements is/are correct about the ionic product of water?

0%
K (equilibrium constant of water) < K $_{w}$
0%
pK>pK $_{w}$
0%
At $100^{0}C$ $Kw = 7.5 \times10^{-14}$ $(moles/lit)^{2}$
0%
Ionic product of water at $25^{0}C is 10^{-14}$

Explanation

$H_2O + H_2O \leftrightharpoons H_3O^{+} + OH^{-}$
This equilibrium applies to pure water and any aqueous solution.
Approximating activities by concentrations, the chemical equilibrium constant, Keq, for this reaction is given by:

$K_{\rm{eq}} = \frac{[{\rm{H_3O^+}}] [{\rm{OH^-}}]}{[{\rm{H_2O}}]^2}$

$K_{\rm w}=[{\rm{H_3O^+}}][{\rm{OH^-}}] = K_{\rm{eq}} \cdot [{\rm{H_2O}}]^2$ So

$K_{\rm{eq}} < K_{\rm w}$

$25^0$ C Kw is equal to

$1.0\times10^{-14}.$ and as temperature increases its value increases. At

$100^0C$ its value becomes

$7.5 \times 10^{-14}$

$pK = -log_{10}K_w$ .

$\therefore$

$pK>pK_w$

Assertion: A mixture of $CH_3COOH$ and $CH_3COONH_4$ is not a buffer solution.

Reason: An acidic buffer contains the mixture of a weak acid and its salt with a strong base.

0%
Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
0%
Assertion is correct but Reason is not correct
0%
Assertion is not correct but Reason is correct
0%
Both Assertion and Reason are not correct

Bleaching powder is used :

0%
for bleaching cotton, wood pulp
0%
as a disinfectant and germicide
0%
for the manufacture of chloroform
0%
as a reducing agent in industries

Explanation

Bleaching powder + ethanol

$\rightarrow$ chloroform
Bleaching powder is used for bleaching cotton, wood pulp, it is also used as a disinfectant and germicide.

Assertion: pH of blood does not change in spite of taking acidic foods.
Reason: Blood behaves as a buffer solution.

0%
Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
0%
Assertion is correct but Reason is not correct
0%
Assertion is not correct but Reason is correct
0%
Both Assertion and Reason are not correct

Explanation

Blood contains a mixture of

$H_{2}CO_{3}$ and

$HCO_{3}^{-}$ which acts as acidic buffer solution.
Thus blood has the tendency to resist changes in pH when small quantities of acid or base are added.

What is the

$[OH^-]$ in the final solution prepared by mixing

$20.0\ mL$ of

$0.050\ M$

$HCl$ with

$30.0\; mL$ of

$0.10 \;M\; Ba(OH)_2$ ?

0%
$0.12\ M$
0%
$0.10\ M$
0%
$0.40\ M$
0%
$0.0050\ M$

Explanation

$Ba(OH)_2 + 2HCl \rightarrow BaCl_2 + 2H_2O$

2 m mol of HCl neutralize 1 m mole of

$Ba(OH)_2$

1 m mol of HCl neutralize 0.5 m mol of

$Ba(OH)_2$

$Ba(OH)_2$ left = 3 - 0.5 m mol = 2.5 m mol

$[Ba(OH)_2] = \frac{2.5}{50}\;M = 0.05\; M$

$[OH]^- = 2 \times 0.05 = 0.1\; M$

The degree of dissociation of an electrolyte depends on:

0%
nature of the electrolyte
0%
nature of solvent
0%
temperature
0%
all the above

Assertion:

The pH of the buffer solution does not change when an acid or a base is added.

Reason:

Buffer solution consists of a mixture of a weak acid and its salt with a strong base.

0%
Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
0%
Assertion is correct but Reason is not correct
0%
Assertion is not correct but Reason is correct
0%
Both Assertion and Reason are not correct

The degree of dissociation of an electrolyte does not depend on:

0%
nature of electrolyte
0%
catalytic action
0%
dilution
0%
temperature

Assertion: A buffer solution has a capacity to resist the change in pH value on an addition of a small amount of acid or base to it.
Reason: An aqueous solution of ammonium acetate can act as buffer.

0%
Both Assertion and Reason are correct and Reason is the correct explanation of Assertion
0%
Both Assertion and Reason are correct but Reason is not the correct explanation of Assertion
0%
Assertion is correct but Reason is not correct
0%
Assertion is not correct but Reason is correct
0%
Both Assertion and Reason are not correct

Buffer solution has the capacity to restore the pH of a solution if some minor changes occur in

$H^+$ concentration.

0%
True
0%
False

Explanation

Buffer solution is defined as a solution which can resist a change in pH on addition of a small amount of an acid or base. Hence buffer solution has the capacity to restore the pH of the solution if some minor changes occur in

$H^+$ concentration.

100ml of a buffer of

$1M NH_3(aq)\: and\: {1M NH_{4}}^{+}(aq)$ are placed in two half cells separately. A current of 1.5amp is passed through both half cells for 20min, if electrolysis of only water take place. The pH of :

0%
Anode half cell will decrease
0%
Cathode half cell will decrease
0%
Both half cell will decrease
0%
Both half cell remain same

Explanation

As only the electrolysis of water take place so the conc. of

$H^+$ ion in Anode compartment increases

What is the term for the positive and negative ions of a compound breaking apart in solution?

0%
Conglomeration
0%
Oxidation
0%
Dissociation
0%
None of the above

Explanation

Acids and bases go through a process of dissociation when they are put into solution. They break apart into positively and negatively charged particles.
Hence, option

$C$ is correct.

A basic buffer consists of a mixture of weak base and its salt with weak acid.

0%
True
0%
False

Which of the following are present in a dilute aqueous solution of

$HCl$ ?

0%
$H_{3}O^{+}+Cl^{-}$
0%
$H_{3}O^{+}+OH^{-}$
0%
$Cl^{-}+OH^{-}$
0%
Unionised $HCl$

Explanation

In the aqueous solution

$HCl$ gives a hydrogen as a proton which reacts with water to give hydronium ions. Hydroxyl ions are not formed in the case of strong acids but are formed when any base with hydroxyl ions dissociates from the base in its aqueous solution.

$HCl\left( g \right) \leftrightarrow { H }^{ + }+{ Cl }^{ - }\xrightarrow { Aqueous\ soln. } { H }_{ 3 }{ O }^{ + }+{ Cl }^{ - }$

Which one of the following can be used as an acid-base indicator by a visually impaired student?

0%
Litmus
0%
Turmeric
0%
Vanilla essence
0%
Petunia leaves

Mineral acids are stronger acids than carboxylic acids because :

(i) mineral acids are completely ionized.
(ii) carboxylic acids are completely ionized.
(iii) mineral acids are partially ionized.
(iv) carboxylic acids are partially ionized.

0%
(i) and (iv)
0%
(ii) and (iii)
0%
(i) and (ii)
0%
(iii) and (iv)

The minimum concentration of

$Ag^{+}$ ion at which precipitation of at least one anion starts is:

0%
$10^{-8}$ .
0%
$1.41 \times$ $10^{-6}$ .
0%
$2 \times$ $10^{-6}$ .
0%
$2 \times$ $10^{-10}$ .

Explanation

$K_{sp}(AgCl)=1 \times 10^{-10}$ and

$K_{sp}(Ag_2CrO_4)= 4 \times 10^{-14}$

$\therefore [Ag^+][Cl^-]= 1 \times 10^{-10}$

$[Ag^+]^2[CrO_4^{2-}]= 4 \times 10^{-14}$

So,

$Ag_2CrO_4$ will precipitate first due to lesser value of

$K_{sp}$ .

$[Ag^+]^2[CrO_4^{2-}]= 4 \times 10^{-14}$

$\Rightarrow [Ag^+]= \sqrt {\cfrac {4 \times 10^{-14}}{0.02}}= 1.41 \times 10^{-6}M$

$\therefore$ The minimum concentration of

$Ag^+$ ion

$1.41 \times 10^{-6} M$ .

Which is not a buffer solution:

0%
$NH_{4}Cl+NH_{4}OH$
0%
$CH_{3}COOH+CH_{3}COONa$
0%
$CH_{3}COONH_{4}$
0%
$NH_{4}NO_{3}$

Explanation

A buffer solution either is a mixture of a weak acid and its salt with strong base or a mixture of a weak base and its salt with strong acid. Hence, clearly

$CH_{3}COONH_{4}$ is not a buffer solution.

In a sample of pure water, which one of the following statements is always true at all conditions of temperature and pressure.

0%
$[OH^-] = 1.0\times10^{-14} M$
0%
$[H_3O^+] = 1.0\times10^{-7} M$
0%
$[OH^-] = 1.0\times10^{-7} M$
0%
$[H_3O^+]=[OH^-]$

The pH value of blood does not appreciably change by a small addition of an acid or a base, because the blood

0%
is a body fluid
0%
can be easily coagulated
0%
contains iron as a part of the molecule
0%
contains serum protein which acts as buffer

Explanation

The buffer system present in serum is

$H_{2}CO_{3}+NaHCO_{3}$ and as we know that a buffer solution resist the change in pH therefore pH value of blood does not change by a small addition of an acid or a base.

About buffer solution which is correct ?

0%
It contains a weak acid and its conjugate base
0%
It contains a weak base and its conjugate acid
0%
It shows change in pH on adding small amount of acid or base
0%
All of the above

Explanation

Weak acid + its conjugate base

$\rightarrow$ acid buffer
Weak base + its conjugate acid

$\rightarrow$ basic buffer
A buffer solution resist the change in pH on adding a drop of acid or a base.

The salt which does not react with acid or base is :

0%
sodium hydroxide
0%
sulphuric acid
0%
sodium chloride
0%
sodium acetate

Explanation

The salt which does not react with acid or base is Sodium chloride.
Salts having common acidic or basic radicals are said to belong to the same family. Sodium chloride (

$NaCl$ ) and Calcium chloride (

$CaCl_2$ ) belong to chloride family.

Salts produced because of reaction between a strong acid and strong base is neutral in nature. The pH of a value of such salts is equal to 7, i.e. neutral.

Example; Sodium chloride, sodium sulfate, potassium chloride, etc.

Sodium chloride ( $NaCl$ ) is formed after the reaction between a hydrochloric acid (a strong acid) and sodium hydroxide (a strong base).

Which of the following pairs constitutes a buffer?

0%
$NaOH and NaCl$
0%
$HNO_{3} and NH_{4}NO_{3}$
0%
$CH_{3}COOH+CH_{3}COONa$
0%
$HNO_{2} and NaNO_{2}$

Explanation

$CH_{3}COOH$ is a weak acid and

$CH_{3}COONa$ is salt of weak acid and strong base.

$HNO_{2}$ is a weak acid and

$NaNO_{2}$ is salt of that weak acid and strong base

$(NaOH).$

The degree of dissociation of weak electrolyte increases by :

0%
increasing the concentration of weak electrolyte solution
0%
adding a common ion
0%
dissolution in solvent of low dielectric constant
0%
adding more amount of solvent into the solution

Le- Chatelier's principle is applicable to both homogeneous and heterogeneous equilibria.

0%
True
0%
False

In which of the following salts, cation does not undergo hydrolysis but anion undergoes hydrolysis?

0%
$BaCO_{3}$
0%
$CaCl_{2}$
0%
$K_{2}CO_{3}$
0%
$NaNO_{3}$

Explanation

Cation from strong base does not undergo hydrolysis whereas anion of weak base undergoes hydrolyze. In

$K_{2}CO_{3} , CO_{3}^{2-}$ ion undergoes hydrolysis to form alkaline solution.

The unit of

$K_w$ is:

0%
$mol^2/L^2$
0%
$mol/L^2$
0%
$mol^2/L$
0%
$mol/L$

Explanation

${ K }_{ w }=\left[ { H }^{ + } \right] \left[ { OH }^{ - } \right] =[mol/L]\left[ mol/L\right]$

${ K }_{ w }=\dfrac { { mol }^{ 2 }}{ {L }^{ 2 } }$

Which of the following combinations will make a buffer solution?

(i)

$CH_3COONa\ (2 mol) + HCl\ (1 mol)$

(ii)

$CH_3COOH\ (2 mol) + NaOH\ (1 mol)$

(iii)

$CH_3COOH\ (1 mol) + CH_3COONa\ (1 mol)$

0%
$(iii)$
0%
$(i), (ii)$
0%
$(ii), (iii)$
0%
$(i), (ii), (iii)$

Identify the common property for a chemical reaction at dynamic equilibrium.

0%
The measurable properties like concentration, density, colour, pressure etc remain constant at constant temperature.
0%
The forward and backward reactions take place with the same rate.
0%
It can be achieved from both directions.
0%
All the above

Identity the false statements regarding ionic product of water:

0%
ionic product of water increases on the addition of acids
0%
ionic product of water is constant at a constant temperature
0%
ionic product of water at $0^{o}$ C can have a value of $10^{-11}$
0%
neutral pH depends on the value of ionic product of water

Explanation

Ionic product of water remains constant on addition of acid.

If an impurity is an acid or base, this will affect the concentrations of hydronium ion and hydroxide ion. If an acid is added to the sample, then concentration of

$OH^{-}$ will decrease in such a way that the product remains constant for fixed temperature and pressure. Thus these water samples will be slightly acidic.

What is meant by ionic product of water?

0%
Concentrations of $H^+$ ions
0%
Concentrations of $OH^-$ ions
0%
The product of concentrations of $H^+$ and $OH^-$ ions
0%
None of these

Explanation

The Ionic Product of Water, $K_w$ , is the equilibrium constant for the reaction in which water undergoes an acid-base reaction with itself. That is, water is behaving simultaneously as both an acid and a base.

In the reaction :

$NO_2+CO \leftrightharpoons NO+ CO_2$ , the equilibrium state may be recognized by the constancy of color.

0%
True
0%
False

State True or False.

$S^{2-}$ is the conjugate base of

$HS^-$ .

0%
True
0%
False

Explanation

$HS^{-}$ loses

$H^{+}$ to form the conjugate base

$S^{2-}$ .

Hence, option A is correct.

The

$pH$ of blood is:

0%
strongly acidic
0%
neutral
0%
strongly basic
0%
slightly basic

Explanation

Blood is normally slightly basic, with a normal

$pH$ range of

$7.35$ to

$7.45$ . Usually the body maintains the

$pH$ of blood close to

$7.40$ .

The degree of dissociation of water in a 0.1M aqueous solution of HCl at a certain temperature

$t\ ^oC$ is

$3.6\times 10^{-15}$ . The temperature

$t$ must be:

[density of water at

$t\ ^oC=1 gm/ml]$

0%
$< 25^oC$
0%
$=25^oC$
0%
$> 25^oC$
0%
Insufficient data to predict

Milk of magnesia used as a medicine for treating indigestion is a substance that -

0%
Helps in disintegration of food products leading to their facile metabolism.
0%
Combines with gastric hydrochloric acid thereby enhancing the latter's efficiency
0%
Improves the enzymatic activities inside the stomach.
0%
Neutralises excess acidity, providing a buffered medium inside the stomach.

A compound which is called microcosmic salt is:

0%
$Na_{2}HPO_{4}.2H_{2}O$
0%
$NaH_{2}PO_{4}.H_{2}O$
0%
$Na(NH_{4})HPO_{4}.4H_{2}O$
0%
$Na_{2}(NH_{4})PO_{4}.2H_{2}O$

Explanation

$Na(NH_4)HPO_4\cdot 4H_2O$ is called microcosmic salt. It is used to identify halides in qualitative analysis. It is formed as a byproduct of thermal decomposition of urine.

Superphosphate of lime mainly acts as :

0%
fungicide
0%
disinfectant
0%
fertiliser
0%
all of the above

Which among the following factors changes the value of ionic product of water?

0%
Change in temperature
0%
Addition of acid
0%
Addition of base
0%
Addition of either acid and base.

$pK_a$ for the acid

$HA$ is

$6$ . The value of

$K$ for the reaction

$A^-+H_3O^+\rightleftharpoons HA+H_2O$ is:

0%
$1\times 10^{-6}$
0%
$1\times 10^{8}$
0%
$1\times 10^{-8}$
0%
$1\times 10^6$

Explanation

The acid dissociation equilibrium is as shown below

$HA+H_2O\rightleftharpoons H_3O^++A^-$
The acid dissociation constant is

$K_a=10^{-6}$
The reaction

$HA+H_2O\rightleftharpoons H_3O^++A^-$ is the reverse of the reaction for the acid dissociation equilibrium.
Hence,

$K= \dfrac {1} {K_a}\dfrac {1}{10^{-6}}=10^6$

Which of the following salts can produce only two types of radicals?

0%
$NaKCO_3$
0%
$CaOCl_2$
0%
$NH_4HSO_4$
0%
$Na(NH_4)HPO_4$

Explanation

$NaKCO_3\rightarrow Na^++K^++CO_{3}^{-2}$

$CaOCl_2\rightarrow Ca^{+2}+OCl^-+Cl^-$

$NH_4HSO_4\rightarrow NH_{4}^{+}+HSO_{4}^{-}$
(2 types of radicals)

$Na(NH_4)HPO_4\rightarrow Na^++NH_{4}^{+}+HPO_{4}^{-}$

CBSE Questions for Class 11 Medical Chemistry Equilibrium Quiz 3 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Equilibrium Quiz 3 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

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