either weak or strong electrolyte

rapidly changes pH due to addition of an acid.

changes pH only with the addition of a strong base.

A solution that contains equal amounts of a weak acid and its conjugate base, or a weak base and its conjugate acid.

A solution that contains both a strong acid and a base.

A solution that contains an acid.

A solution that contains equal amounts of a strong acid and its conjugate base, or a strong base and its conjugate acid.

A solution that contains a base.

MCQ Questions for Class 11 Medical Chemistry Equilibrium Quiz 6

All salts are:

0%
strong electrolytes
0%
weak electrolytes
0%
non electrolytes
0%
either weak or strong electrolyte

Explanation

As, substances that give ions when dissolved in water are called

$electrolytes$ .They can be divided into acids, bases and salts, because they all give ions when dissolve in water.

$Strong$

$electrolytes$ completely ionize when dissolve in water, and no neutral molecules are formed in solution.

Example -

$NaCl$ ,

$HNO_{3}$ etc.

As we know, chemically, a salt is an ionic compound as it is composed of two oppositely charged ions - cation and anion. Due to the presence of ions, they are good conductors of heat and electricity in a molten state and in solutions.

So, all salts are strong electrolytes as they completely dissolve in water and dissociates into their component ions.

Hence, option

$A$ is correct.

When pH of rain water is less than 5.6, it is called:

0%
monsoon rain
0%
acid rain
0%
basic rain
0%
heavy rain

Tooth decay starts when the pH of the mouth is less than:

0%
4.5
0%
5.5
0%
6.5
0%
7.5

Why only

${As}^{+3}$ gets precipitated as

${As}_{2}{S}_{3}$ and not

${Zn}^{+2}$ as

$ZnS$ when

${H}_{2}S$ is passed through an acidic solution containing

${As}^{+3}$ and

${Zn}^{+2}$ ?

0%
Solubility product of ${As}_{2}{S}_{3}$ is less than that of $ZnS$
0%
Enough ${As}^{+3}$ are present in acidic medium
0%
Zinc salt does not ionise in acidic medium
0%
Solubility product changes in presence of an acid

Explanation

The species having minimum value of

${K}_{sp}$ will get precipitated first of all because ionic product will exceed the solubility product of such species.

${K}_{sp}$ of

${As}_{2}{S}_{3}$ is less than

$ZnS$ . In acid medium ionisation of

${H}_{2}S$ is suppressed (common ion effect) and

${K}_{sp}$ of

$ZnS$ does not exceed.

Match the following:

Natural source	Acid
Vinegar	a. Oxalic acid
Orange	b. Acetic acid
Tamarind	c. Citric acid
Tomato	d. Tartaric acid

0%
1-a, 2-b,3-d,4-c
0%
1-b, 2-c, 3-d, 4-a
0%
1-a, 2-c, 3-d, 4-a
0%
1-d, 2-a, 3-b, 4-c

The separation of

$H^{+}$ ion from the _______ molecules cannot occur in the absence of water.

0%
$HCl$
0%
$NaOH$
0%
$H_{2}SO_{4}$
0%
none of the above

Explanation

The separation of

$H^{+}$ ion from the

$HCl$ molecules cannot occur in the absence of water.

Example:

$HCl + H_{2}O \rightarrow H_{3}O^{+} + Cl^{-}$

Hence, the correct option is

$A$

Match the following

Natural source	Acid
1. Sour milk (Curd)	a. Lactic acid
2. Lemon	b. Citric acid
3. Ant sting	c. Methanoic acid

0%
1-a, 2-b, 3-c
0%
1-a, 2-c, 3-b
0%
1-c, 2-b, 3-a
0%
1-b, 2-a, 3-c

Why does survival of aquatic life becomes difficult because of acid rain?

0%
When acid rain falls into the river, it lowers the pH of the river water.
0%
When acid rain falls into the river, it increases the pH of the river water.
0%
Acid rain does not cause any change in the river water.
0%
None of the above

Which part of the tooth, made up of a crystalline form of calcium phosphate, is the hardest substance in the body?

0%
Root
0%
Body
0%
Enamel
0%
All

0.1 M acetic acid gets 1% ionised. If it ionise 10 times, then concentration of

$[H^+]$ will be

0%
0.001
0%
0.01
0%
0.05
0%
0.1

$80^{\circ} C$ , distilled water

$(H_{3}O^{+})$ has concentration equal to

$1\times 10^{-6}\ mol/ litre$ . The value of

$K_{w}$ at this temperature will be:

0%
$1\times 10^{-6}$
0%
$1\times 10^{-12}$
0%
$1\times 10^{-9}$
0%
$1\times 10^{-15}$

Explanation

$[H_{3}O^{+}] = [H^{+}] = 10^{-6}$

$K_{w} = [H^{+}] [OH^{-}]$

In pure water,

$[H^{+}] = [OH^{-}]$

So,

$[OH^{-}] = [H^{+}] = [H_{3}O^{+}] = 10^{-6}$

$K_{w} = [10^{-6}] [10^{-6}] = 10^{-12}$ .

$K_{w}$ increases with an increase in temperature.

Which of the following is a weak acid?

0%
Acetic acid
0%
Formic acid
0%
Carbonic acid
0%
All of the above

Explanation

A weak acid is an acid which on dissociation in an aqueous solution produces low concentration of H+ ions.

Acetic acid

$(CH_3COOH)$ , Formic acid

$(HCOOH)$ , Carbonic acid

$(H_2CO_3)$ are considered as weak acids.

An acid is a compound which when dissolved in water yields:

0%
hydroxide ions
0%
hydronium ions
0%
hydrogen
0%
none of the above

Explanation

Some of the general properties of acids are as follows :-

They are sour to taste.

They turn blue litmus paper red and the red litmus paper remains unaffected.

They dissociate into an anion and hydrogen ions when dissolved in water and these hydrogen ions combine with water to form hydronium ions. These ions were responsible for the acidity of the acids.

$H^+ + H_2O \rightarrow H_3O^+$

Hence, the correct answer is option (B).

$HCl+H_2O \longrightarrow$

0%
$H + Cl$
0%
$HOCl + Cl^-$
0%
$H_3O^+ + Cl^-$
0%
none of the above

Explanation

Hydrochloric Acid (Strong one) will easily dissociate into the consisting ions within aqueous medium.

$HCl\longrightarrow H^++Cl^-$

Gives,

$H^++H_2O\longrightarrow H_3O^+$

$HCl+H_2O\longrightarrow H_3O^++Cl^-$

Hence, option C is correct.

What are strong acids and weak acids?

0%
An acid which dissociates completely or almost completely in water are strong acids and an acid that dissociates only partially when dissolved in water are weak acids.
0%
An acid which dissociates completely in water are strong acids and an acid which dissociates almost completely in water are weak acids.
0%
An acid which do not dissociate completely in water are strong acids and an acid which dissociates almost completely in water are weak acids.
0%
An acid that dissociates only partially when dissolved in water are strong acids and an acid which do not dissociate completely in water are weak acids.

Explanation

An acid, which dissociates completely or almost completely in water are strong acids. An acid that dissociates only partially when dissolved in water are weak acids.

Strong acid like

$HCl, H_2SO_4$ etc.

Weak acid like

$CH_3COOH, HCOOH$ etc

Greater the number of hydronium ions present:

0%
greater is the strength of acid
0%
greater is the strength of base
0%
lower is the strength of base
0%
both $A$ and $B$

The strength of an acid depends on the concentration of the hydronium ions ________ present in a solution.

0%
$H^+$
0%
$H_3O^+$
0%
$OH^-$
0%
All of the above

Explanation

$HCl+H_2O\longrightarrow H_3O^++Cl^-$

$\rightarrow$ Strength at acid depends on extent of dissociation

$\rightarrow$ Extent of dissociation depends on product's concentration.

Thus,

$[H_3O^+]$ is dependent on strength of the acid and vice-versa.

$NaOH+H_2O \longrightarrow$

0%
$NaO+H_2$
0%
$Na^+ + H^-$
0%
$Na^+ +OH^-$
0%
none of the above

Explanation

Alkalis when dissolved into water dissociates into ions so the reaction is as follows:

$NaOH+H_2O \longrightarrow Na^+ +OH^-$

The product of molar concentrations of hydrogen ions and hydroxide ions in a

$0.01 M$ aqueous solution of sodium chloride is known as

0%
Hydrolysis constant of salt
0%
Dissociation constant of acid
0%
Dissociation constant of base
0%
Ionic product of water

Explanation

Sodium chloride is a salt of strong base

$NaOH$ and strong acid

$HCl$ . In its aqueous solution, following equilibrium is observed.

$NaCl+{ H }_{ 2 }O\rightleftharpoons { Na }^{ + }+{ Cl }^{ - }+{ H }_{ 2 }O$
Hence, no hydrolysis takes place in this case, and the solution remains neutral. Thus, here the product of molar concentrations of hydrogen ions and hydroxide ions is ionic product of water.

A salt is a general name given to the chemical produced during _______ reaction between an acid and a base

0%
decomposition
0%
neutralization
0%
displacement
0%
double decomposition

The properties of alkalis are due to the presence of ________ ions.

0%
positive
0%
negative
0%
hydroxyl
0%
both $B$ and $C$

The decreasing acidic strength of a few of the acids

$HCOOH, {CH}_{3}COOH, {C}_{2}{H}_{5}COOH$ and

${C}_{3}{H}_{7}COOH$ is due to

0%
increase in $+I$ effect due to alkyl group
0%
increase in $-I$ effect due to alkyl group
0%
decrease in $+I$ effect due go alkyl group
0%
increase in $+M$ effect

Explanation

Electron releasing groups (

$+I$ groups) destabilizes conjugate base
so acidic strength

$\propto \cfrac{1}{+I\quad groups}$

$0.1\ M$ aqueous solution of a weak acid is

$2\%$ ionized. If the ionic product of water is

$1\times 10^{-14}$ , the

$[OH^-]$ is:

0%
$5\times 10^{-12}$ M
0%
$2\times 10^{-3}$ M
0%
$1\times 0^{-14}$ M
0%
none of these

Explanation

Degree of dissociation of weak acid,

$\alpha=\dfrac{2}{100}=0.02$

Concentration of acid is

$[H^+]=C\alpha =0.1\times0.02=0.002$

Ionic product of water

$=1\times10^{-14}$

$[H^+][{OH}^-]=1\times10^{-14}$

$[{OH}^-]=\dfrac { 1\times{ 10 }^{ -14 } }{ 0.002 } =5\times{ 10 }^{ -12 }$

In III group precipitation,

$NH_4Cl$ is added before adding

$NH_4OH$ to.

0%
Decrease conc. of $OH^-$
0%
Prevent interference of $PO^{3-}_4$
0%
Increase conc. of $Cl^-$
0%
Increase conc. of $OH^-$ ion.

Explanation

The common ion effect is responsible for the reduction in the solubility of an ionic precipitate when a soluble compound containing one of the ions of the precipitate is added to the solution in equilibrium with the precipitate.

Due to Common ion effect, the concentration of

${OH}^-$ decreases when

$NH_4Cl$ is added to

$NH_4OH$

In acid rain, pH of rain water is:

0%
7
0%
9.0
0%
more than 9.6
0%
below 5.6

Explanation

When pH of rain water drops anywhere below 5.6, it is said to be acid rain.

The main cause for acid rain is the presence of high levels of oxides of sulphur and nitrogen, which form acids with water.

Hence, the correct option is $D$ .

Which buffer solution comprising of the following has its

$pH$ value greater than 7?

0%
${ CH }_{ 3 }COOH$ + ${ CH }_{ 3 }COONa$
0%
$HCOOH + HCOOK$
0%
${ CH }_{ 3 }COO{ NH }_{ 4 }$
0%
${ NH }_{ 4 }OH+{ NH }_{ 4 }Cl$

Explanation

The

$pH$ value of a basic buffer is always greater than

$7.$

Among the given options,

$NH_4OH+NH_4Cl$ is the only mixture which consists of a mixture of a weak base and its conjugated salt and thus, has a

$pH$ greater than 7.

Hence, option

$D$ is correct.

Which is a general process in which molecules separate or split into smaller particles?

0%
Association
0%
Ionisation
0%
Dissociation
0%
Recombination

If the dissociation constants of two substances are

${K}_{1}$ and

${K}_{2}$ respectively, then the ratio of degree of dissociation for a given concentration, is given by

0%
$\cfrac{{K}_{1}}{{K}_{2}}$
0%
$\sqrt{\cfrac{{K}_{1}}{{K}_{2}}}$
0%
$\cfrac { { \left( { K }_{ 1 } \right) }^{ 2 } }{ { K }_{ 2 } }$
0%
$\cfrac { { K }_{ 1 }.{ K }_{ 2 } }{ { K }_{ 2 } }$

Explanation

From OStwald dilution formula

$K={\alpha}^{2}C$
where

$K$ is dissociation constant and

$\alpha$ is degree of dissociation or ionisation

$\cfrac{{K}_{1}}{{K}_{2}}=\cfrac{{\alpha}_{1}^{2}}{{\alpha}_{2}^{2}}$

$\cfrac{{\alpha}_{1}}{{\alpha}_{2}}=\sqrt {\cfrac{{K}_{1}}{{K}_{2}}}$

When an acid dissolves in water, it gives:

0%
proton
0%
negative ion
0%
hydroxide ion
0%
both $A$ and $B$

Explanation

When an acid dissolves in water, a covalent bond between an electronegative atom and a hydrogen atom is broken by heterolytic fission, which gives a proton (

$H^+$ ) and a negative ion.

$H_2SO_4 + H_2O \rightarrow$

The product of the reaction is:

0%
$H^{+} + HSO_4{^-}$
0%
$H_3O^{+} + {HSO_4}^{-}$
0%
$H_3O^{+} + SO_4^{-2}$
0%
None of the above

Explanation

$H_2SO_4 + H_2O \rightarrow H_3O^{+} + {HSO_4}^{-}$

$H_2SO_4$ dissociates to gives hydronium ions in water.

Hence, option

$(B)$ is correct.

Why does

$HCl$ ionize in solution if they are covalently bonded?

0%
Many bonds can be covalent in one situation and ionic in another
0%
It does not ionize
0%
They are not covalently bonded
0%
None of the above

Explanation

Many bonds can be covalent in one situation and ionic in another. Hydrogen chloride,

$HCl$ , is a gas in which the hydrogen and chlorine are covalently bound, but if

$HCl$ is bubbled into the water, it ionizes completely to give the

$H^+$ and

$Cl^-$ of a hydrochloric acid solution.

Which bond is broken when an acid dissolves in water?

0%
Covalent
0%
Recombination bond
0%
Ionic
0%
All of the above

Explanation

When an acid dissolves in water, a covalent bond between an electronegative atom and a hydrogen atom is broken by heterolytic fission, which gives a proton (

$H^+$ ) and a negative ion. A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms.

The

$pH$ of boiling water is

$6.4$ . This implies that boiling water is:

0%
slightly basic
0%
slightly acidic
0%
neutral
0%
amphoteric

Explanation

The ph of boiling water is 6.4. This implies that boiling water is neutral. When water is boiled, both hydrogen ion and hydroxide ion concentration increases to same extent. Hence it is neutral. With increase in the hydrogen ion concentration, pH decreases from 7 to 6.4. Also, the value of

$\displaystyle K_w$ also increases as the degree of dissociation of water increases with increase in temperature.

Protons (

$H^+$ ions ) are found when a substance is dissolved in water. The substance is ___________.

0%
$KOH$
0%
$NaH$
0%
$H_{2}SO_{4}$
0%
$NH_{3}$
0%
$CH_{4}$

Explanation

An acid is a proton

$(H^+)$ donor. A base is a proton (hydrogen ion) acceptor. Acids dissociate into

$H^+$ ions in water. The acid

$H_2SO_4$ dissociates into

$H^+$ and

$SO_4^{2-}$ will show the presence of

$H^+$ even after they dissolve in water.

$KOH$ gives

$OH^-$ ion.

$NaH$ gives

$H^-$ ions while

$NH_3$ is also a base forms

$NH_4^+$ in water.

$CH_4$ is not react as acid nor like a base.

Why

$HF$ is a weak acid while

$HCl$ is a strong acid?

0%
$HF$ produces very few $H^{+}$ ions in water
0%
$HCl$ dissociates completely to produce many $H^{+}$ ions in water
0%
Both $A$ and $B$
0%
None of the above

Explanation

Acids which ionises completely into its ions are called strong acids. A strong acid is one which is virtually 100% ionised in solution.

$HCl$ dissociates completely to produce many

$H^{+}$ ions in water whereas

$HF$ produces very few

$H^{+}$ ions in water due to the lesser stability of

$F^-$ as compared to

$Cl^-$ . Hence,

$HF$ is a weak acid while

$HCl$ is a strong acid.

$H_3O^{+}$ is a:

0%
hydrated negative ion
0%
negative ion
0%
dehydrated proton
0%
hydrated proton

Explanation

An acid is a substance which ionizes and gives hydrogen ions when dissolved in water. A hydrogen ion cannot exist on its own, so it combines with a water molecule to form a hydronium ion.

$H_3O^+$ is the hydronium ion, a hydrated proton:

$H^{+} + H_2O \rightarrow H_3O^{+}$
It is referred to as a hydrated proton because it is really a water molecule with one extra proton.

Which of the following is a strong acid?

0%
$CH_3COOH$
0%
$HNO_3$
0%
$H_2CO_3$
0%
All of the above

Explanation

$Explanation:$

An acid that dissociates almost completely and gives

$H^+$ in water is called a strong acid.

Weak acids are those which are partially dissociated.

$HNO_3$ dissociates completely in water to give

$H^+$ and

$NO_3^-$ ions, therefore,

$HNO_3$ is strong acid.

$CH_3COOH$ and

$H_2CO_3$ do not dissociate completely in water. Therefore they are weak acids.

$Final\ Answer:$ Option

$B$ .

Mixing a concentrated acid with water reduces the concentration of:

0%
hydronium ions
0%
hydrogen atoms
0%
oxygen atom
0%
none of the above

In order to make a buffer solution, a weak monoprotic acid could be added to :

0%
another acid
0%
another base
0%
its conjugate base
0%
its conjugate acid
0%
a strong base

Explanation

In order to make a buffer solution, a weak monoprotic acid could be added to its conjugate base.
Thus, we can add acetic acid (a weak monoprotic acid ) to acetate ion (conjugate base).

$\displaystyle CH_3COOH + CH_3COO^-$
An acidic buffer solution is a mixture of weak acid and its salt with strong base.

What is the common ion effect?

0%
When the addition of an ion common to two solutes causes precipitation or reduces ionization.
0%
When a molecule is added to a solution and causes precipitation or reduces ionization
0%
When the subtraction of an ion common to two solutes causes precipitation or reduces ionization.
0%
The effect of adding ions to a solution.
0%
When any ion is added to a solution and causes precipitation or reduces ionization.

A buffer solution:

0%
rapidly changes pH due to addition of an acid.
0%
resists changes in pH.
0%
does not change pH at all.
0%
changes pH only with the addition of a strong base.

Explanation

The solution of buffer resists changes in

$pH$ .

A buffer solution is defined as a solution which resists drastic changes in

$pH$ upon the addition of a small amount of either an acid or a base.

Hence, te correct option is

$\text{B}$

Which of the following pairs of species could be a buffer?

0%
H $^+$ and Cl $^-$
0%
H $_2$ CO $_3$ and HCO $_3^-$
0%
Na $^+$ and NO $_3^-$
0%
Na $^+$ and OH $^-$
0%
HNO $_3$ and NO $_3^-$

Explanation

$\displaystyle H_2CO_3 + HCO_3^-$ constitutes a buffer solution. An acidic buffer solution is a mixture of weak acid (such as carbonic acid) and its salt (bicarbonate) with strong base (such as NaOH or KOH).

Hence option B is correct.

Which of the following statements are correct about dissociation?

0%
Dissociation generally refers to breaking a compound into smaller pieces, usually reversibly.
0%
Dissociation can happen without the formation of charged species
0%
Both $A$ and $B$
0%
None of these

Explanation

Dissociation in chemistry and biochemistry is a general process in which molecules (or ionic compounds such as salts, or complexes) separate or split into smaller particles such as atoms, ions or radicals, usually in a reversible manner. It may or may not form charged species as shown below.

i). $NaCl \leftrightharpoons Na^++Cl^-$

ii). $N_2O_4 \leftrightharpoons 2NO_2$

For the preparation of saturated

$PbS{ O }_{ 4 }$ solution of 1 litre at 25 degrees, the minimum number of moles of

$PbS{ O }_{ 4 }$ that must be added (

${ K }_{ sp }$ at

$25$ for

$PbS{ O }_{ 4 }=1\times { 10 }^{ -8 }$ ) is :

0%
$1\times { 10 }^{ -16 }mol$
0%
$1\times { 10 }^{ -8 }mol$
0%
$1\times { 10 }^{ -4 }mol$
0%
$1\times { 10 }^{ -2 }mol$
0%
$1\times { 10 }^{ -1 }mol$

Explanation

$\displaystyle K_{sp, PbS{ O }_{ 4 } } =1\times { 10 }^{ -8 } = [Pb^{2+}] [SO_4^{2-}]$

$\displaystyle [Pb^{2+}]= [SO_4^{2-}]= [PbSO_4]=S$ M

$\displaystyle K_{sp, PbS{ O }_{ 4 } } =1\times { 10 }^{ -8 } = S \times S =S^2$

$\displaystyle S = \sqrt {1\times { 10 }^{ -8 } } = 1\times { 10 }^{ -4 } M$
Hence, to 1 L of solution,

$\displaystyle 1\times { 10 }^{ -4 }$ moles of

$\displaystyle PbSO_4$ should be added.

Which of the following is a correct statement?

0%
The number of positive ions in solution equals the number of negative ions.
0%
The total positive charge and total negative charge are equal in the solution.
0%
The positive ions are known as cathodes.
0%
The positive ions are known as anions.
0%
None of the above

Explanation

The total positive charge and total negative charge are equal in the solution. Due to this, the solution is electrically neutral.

For example, a solution of NaCl in water contains equal number of

$\displaystyle Na^+$ ions and

$\displaystyle Cl^-$ ions.

Hence option B is correct.

A beaker contains a saturated solution of copper(I) chloride. Copper(I) chloride is slightly soluble salt with a solubility product of

$1.2 \times 10^{−6}$ .
Which of the following salts when added to the solution would precipitate copper(I) chloride?

0%
Sodium chloride
0%
Potassium bromide
0%
Silver(I) nitrate
0%
Lead(II) acetate
0%
Magnesium iodide

Explanation

A beaker contains a saturated solution of copper(I) chloride. Copper(I) chloride is slightly soluble salt with a solubility product of

$1.2 \times 10^{−6}$ .
The addition of sodium chloride to the solution would precipitate copper(I) chloride.
Sodium chloride is a strong electrolyte. It completely dissociates to provide chloride ions.
Chloride ion is a common ion. It suppresses the solubility of copper(I) chloride.
With increase in chloride ion concentration, the the ionic product of copper(I) chloride exceeds its solubility product. This results in precipitation of copper(I) chloride.

What is the relationship between

$[OH^-]$ and

$[H_3O^+]$ in a water solution?

0%
When multiplied together, they equal a constant, $K_w$ .
0%
When multiplied together, they equal each other.
0%
When divided, they equal a constant, $K_w$ .
0%
When one increases, the other increases.
0%
They explain the acidity of a solution.

Explanation

When

$[OH^-]$ and

$[H_3O^+]$ (in a water solution) are multiplied together, they equal a constant,

$K_w$ which is ionic product of water with a value of

$\displaystyle 1 \times 10^{-14}$ at

$\displaystyle 25^oC$ .

Hence, the correct option is A.

What is a buffer?

0%
A solution that contains equal amounts of a weak acid and its conjugate base, or a weak base and its conjugate acid.
0%
A solution that contains both a strong acid and a base.
0%
A solution that contains an acid.
0%
A solution that contains equal amounts of a strong acid and its conjugate base, or a strong base and its conjugate acid.
0%
A solution that contains a base.

Which among the following resists a rapid change of pH?

0%
Buffer
0%
Indicator
0%
Arrhenius acid
0%
Arrhenius base
0%
Neutral condition

Addition of water to

$X$ solution will not change concentration of

$H_{3}O^{+}$ .

$X$ is:

0%
chemical pH indicator
0%
acid/base buffer
0%
anhydrous solution
0%
hypotonic solution
0%
supersaturated solution

Explanation

Addition of water to

$X$ solution does not change the

$pH$ of the solution, which means the concentration of the species present changes in such a way that the

$pH$ remains the same. This is possible for acid/base buffer.

$pH=pk_a+\log \cfrac{[salt]}{[acid]}$

Since the volume changes the same for both salt and acid, the ratio

$\cfrac{[salt]}{[acid]}$ remains the same and hence

$pH$ also remains the same. Same in the case of basic buffer solution.

CBSE Questions for Class 11 Medical Chemistry Equilibrium Quiz 6 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Equilibrium Quiz 6 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

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