Acid Bases and Salts MCQ Questions

Food has sour and bitter flavours because of acids and bases in it. Acids have a sour taste and cause blue litmus to turn red, whereas bases have a bitter taste and cause red litmus to turn blue. Turmeric is another natural indicator, similar to litmus. The reaction of an acid with a base produces a salt, which is a neutral chemical.

Definition: A material that contributes protons or absorbs electrons is known as an acid. In an aqueous solution, it dissociates into H+ ions. A base is a chemical that provides electrons or extracts protons. In an aqueous solution, it dissociates into OH ions.

Acid Bases and Salts MCQ Chemistry Questions with Solutions

Q-1: Which of the following is the correct classification of Dolomite?

  1. An acid salt
  2. A mixed salt
  3. A normal salt
  4. A double salt

Answer: d) double salt

Explanation: A double salt is a crystalline salt with the content of a mixture of two simple salts but a distinct crystal structure.

Dolomite is a double salt consisting of calcium carbonate (CaCO3) and magnesium carbonate (MgCO3) salts.

Q-2: Acetic acid is weak acid because

  1. Its aqueous solution is acidic
  2. It is highly ionised
  3. It is weakly ionised
  4. It contains the COOH group.

Answer: c) It is weakly ionised


In an aqueous solution, a weak acid is one that ionises just minimally. Acetic acid (found in vinegar) is a highly common weak acid because it doesn’t dissociate much in solution, Its ionisation may be seen below.


As a result, it is less effective at donating protons.

Because acetic acid’s ionisation is incomplete, the equation is shown with a double arrow.

Q-3: What will be the pH of the solution on mixing a 50 mL solution of a strong acid of pH=1 with a 50 mL solution of strong acid of pH =2.

  1. 0.74
  2. 1.76
  3. 1.5
  4. 1.26

Answer: d) 1.26


We know that pH= -log[H+]

Molarity= number of moles/V(L)

Step-1: Calculate the [H+] for a strong acid with pH =1

1=-log [H+] [H+]= 10-1M

Step-2: Calculate the [H+] for a strong acid with pH= 2

2=-log[H+] [H+]= 10-2M

Step-3: Calculate the moles of H+ for a strong acid with pH =1

Moles of H+= [H+] ×V(L)

= 10-1M × 0.050

= 0.005moles

Step-4: Calculate the moles of H+ for a strong acid with pH =2

Moles of H+= [H+] ×V(L)

= 10-2M × 0.050

= 0.0005 moles

Step-5 Calculate the total moles of H+ in the solution

Total moles of H+ = (0.005+ 0.0005) moles

= 0.0055 mol

Total volume of mixture = (0.05 +0.05)L

= 0.1L

Step-6 Calculate the total concentration of H+ in the solution.

[H+] = Total moles of H+/ Total volume

= 0.0055 mol /0.1L

= 0.055 M

Now, pH of the solution = -log[H+]


= 1.26

Q-4: Which of the following is not an amphiprotic species?

  1. HCO3
  2. HPO42-
  3. OH
  4. H2PO42-

Answer: c) OH

Explanation: Amphiprotic ions are those ions which can gain or lose hydrogen ions.

Except OH, all other species are amphiprotic in nature. OH can gain a proton to form H2O but it cannot lose. Hence it is not amphiprotic.

Q-5: Three reactions involving H2PO4 are given below :

i) H3PO4 + H2O → H3O+ + H2PO4

ii) H2PO4+ H2O → HPO42- + H3O+

iii) H2PO4 + OH→ H3PO4 + O2-

In which of the following above H2PO4 act as an acid?

  1. ii only
  2. i) and ii)
  3. iii) only
  4. i) only

Answer: a) ii only

Explanation: An acid is a material that loses protons and we can clearly see that, only in ii) H2PO4 is donating a proton to water . Thus it acts as an acid.

Q-6: Which of the following compound is most acidic?

  1. Cl2O7
  2. P4O10
  3. SO3
  4. B2O3

Answer: a) Cl2O7

Explanation: Acidic strength is the tendency of a molecule/compound to liberate protons. In case of proton deficient compounds, acidic strength is governed by the positive oxidation state of the central atom. More is the value of positive oxidation state, more is the acidic strength.

The oxidation states of Cl,P,S and B are +7,+5,+6 and +3 respectively.

This shows that Cl2O7 is the most acidic.

Q-7: Identify the basic salt from the following.

  1. Na2CO3
  2. NaNO3
  3. KCl
  4. NH4Cl

Answer: a) Na2CO3

Explanation: There are three main classification of salts:

Acidic Salt: A salt that is formed by the neutralisation of strong acid and weak base.

Basic Salt: A salt that is formed by the neutralisation of strong base and weak acid.

Neutral Salt: A salt that is formed by the neutralisation of strong acid and strong base.

The hydrolysis of salt can let us know the acid and base from which it is made up.

On hydrolysis of Na2CO3 , we will get NaOH(strong base) and H2CO3 (weak acid). Since the effect of strong things is always taken into account, hence it is a basic salt.

Q-8: Which of the following can be considered as an example of olfactory indicators?

  1. Onion
  2. Methyl orange
  3. Turmeric
  4. China rose

Answer: a) Onion

Explanation: A substance whose smell varies when it is mixed with an acidic or basic solution is said to be an olfactory indicator. In the laboratory, olfactory indicators can be used to determine whether a solution is a basic or an acid, a procedure known as olfactory titration.

Some common examples are Onion, vanilla, clove oil etc.

Q-9: The pH of a solution obtained by mixing 50.00 mL of 0.20 M weak acid HA (Ka = 10-5) and 50.00 mL of 0.20M NaOH at room temperature is

  1. 2
  2. 3
  3. 5
  4. 9

Answer: d) 9

Explanation: Salt is formed when equal amounts of acids and bases react neutralising the effect of each other.

Here, weak acid(HA) reacts with strong base(NaOH) in the same proportion, thus a basic salt is formed.

Step-1- Calculate the moles of acid

Moles of acid = Molarity × V(L)

= (0.20 mol/L)×(0.05L)

= 0.01 mol

Step-2- Calculate the moles of base

Moles of acid = Molarity × V(L)

= (0.20 mol/L)×(0.05L)

= 0.01 mol

The formula used for calculating pH of a basic salt is:

pH= ½( pKa + pKw + log c)

As pKa = -logKa

= -log(10-5)

= 5

At room temperature, pKw = 14

‘C’ is the concentration of the salt (NaA)

Let us consider a reaction,

HA          +   NaOH → NaA + H2O
  Initial  0.01mol  0.01mol
After reaction 0.01 mol

Total volume(L)= (0.05+0.05)L= 0.1L

C= Moles of NaA/Total volume

= 0.01/0.1

= 0.1M

Substituting the values in the formula,

pH= ½(5+14+log(0.1)

= 9

Hence, the pH of the solution is 9.

Q-10: The pH of a solution prepared from 0.005 mole of Ca(OH)2 in 100cc water is


b) 12

c) 11

d) 13

Answer: d) 13


Step-1-Calculate the [OH] in the solution

We know that,

Molarity = Number of moles/Volume(in L)

[OH] = 0.005 mol /0.1L

= 0.05 M

Since there are two OH ions, therefore [OH] = 2× 0.05

= 0.1 M

Note: 100cc =100mL = 0.1L

Step-2– Calculate pOH

pOH = -log[OH]

= -log(0.1)

= 1

As, pKw = pH +pOH

Also, at room temperature, pKw = 14

Substituting the values,

14= pH+1

pH= 13

Hence, the pH of the solution is 13.

Q-11: The pH of 0.1 M solution of the following salts increases in the order

  1. NaCl<NH4Cl<NaCN<HCl
  2. HCl< NH4Cl<NaCl<NaCN
  3. NaCN<NH4Cl<NaCl<HCl
  4. HCl<NaCl<NaCN<NH4Cl

Answer: HCl< NH4Cl<NaCl<NaCN

Explanation: pH is the measure of whether the solution is acidic, basic or neutral on the basis of its value.

With a pH of 7, salts of a strong acid and a strong base are neutral. Salts of a strong acid and weak base, on the other hand, are acidic with a pH less than 7, and salts of a strong base and weak acid are basic with a pH greater than 7.

NaCl is the salt of strong acid( HCl) and strong base (NaOH) which makes it overall neutral

NH4Cl is the salt of strong acid (HCl) and weak base(NH4OH ) which makes it acidic but not more than HCl.

NaCN is the salt of weak acid (HCN) and strong base (NaOH) which makes it basic.

HCl is a strong acid.

Thus, the correct order of pH is

HCl< NH4Cl<NaCl<NaCN

Q-12: Which of the following is not a use of Bleaching powder?

  1. Bleaching agent
  2. Oxidising agent
  3. Used in soda-acid fire extinguishers.
  4. Disinfectant

Answer: c) Used in soda-acid fire extinguishers

Explanation: Bleaching powder is represented as CaOCl2.

There are many applications of Bleaching powder:

(i) It is used for bleaching cotton and linen in the textile industry.

(ii) bleaching wood pulp in paper factories and for bleaching washed clothes in laundry.

(iii) as an oxidising agent in many chemical industries.

(iv) to make drinking water free from germs.

Q-13: What is the correct formula of Plaster of Paris?

  1. CaSO4
  2. CaSO4.1/2H2O
  3. CaSO4.2H2O
  4. Ca(OH)2

Answer: b) CaSO4.1/2H2O


Plaster of Paris is a material used by doctors to maintain shattered bones in the proper position. Plaster of Paris is a white powder that transforms into gypsum when mixed with water, resulting in a hard solid mass.

Its chemical name is calcium sulphate hemihydrate with the chemical formula of CaSO4.1/2H2O.

Q-14: If a solution of sodium hydrocarbonate is heated, the product formed is

  1. NH4Cl
  2. NaNO3
  3. Na2CO3
  4. Na2CO3.10H2O

Answer: c) Na2CO3

Explanation: The following reaction takes place:

\(\begin{array}{l}2NaHCO_{3}\overset{\Delta }{\rightarrow}Na_{2}CO_{3}+H_{2}O + CO_{2}\end{array} \)

Q-15: Which of the following salts do not contain water of crystallisation?

a) Baking Soda

b) Gypsum

c) Red vitriol

d) Copper sulphate

Answer: a) Baking soda

Explanation: Water molecules found inside crystals are known as water of crystallisation or water of hydration in chemistry.

Gypsum has a chemical formula of CaSO4.2H2O

Baking soda has a chemical formula of Na2CO3

Red vitriol has a chemical formula of CoSO4.7H2O

Copper sulphate has a chemical formula of CuSO4.5H2O

Practise Questions on Acid Bases and Salts

Q-1: What happens when an acid solution is combined with a base solution in a test tube?

  1. the solution’s temperature rises.
  2. The temperature of the solution drops.
  3. The solution’s temperature remains constant.
  4. The production of salt occurs

Select the correct option from below:

(A) (a) only

(B) (a) and (c)

(C) (b) and (d)

(D) (a) and (d)

Q-2: To make Plaster of Paris, what temperature is gypsum heated to?

  1. 25oC
  2. 75oC
  3. 80oC
  4. 100oC

Q-3: The pH of a 2.0 M solution of NH4Cl is

(Kb(NH3) = 1.8× 10-5)

  1. 4.48
  2. 6
  3. 8
  4. 3

Q-4: The salt having pH dependent of its concentration is


b) NH4CN

c) NaCl

d) K2CO3

Q-5: In a dilute aqueous solution of ammonia, which of the following is present?

  1. OH + NH3
  2. OH + NH4+
  3. H3O+ + NH2
  4. None of these

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