Acids and Bases

Acid-Base Theories MCQs with Answers

Welcome to the Acid-Base Theories MCQs with Answers, it helps learners quickly identify areas for improvement in Acid-Base Theories Online Test.

Acid-base theories form the foundation of understanding chemical reactions involving acids and bases. In an acid-base theories quiz, MCQs (multiple choice questions) cover key concepts from different perspectives:

The Arrhenius theory MCQs focus on how acids dissociate to produce hydrogen ions (H+) in aqueous solutions and bases produce hydroxide ions (OH-).

Bronsted-Lowry theory MCQs expand this by defining acids as proton donors and bases as proton acceptors, broadening the scope beyond aqueous solutions to include non-aqueous systems.

Lewis theory exam questions explore acids as electron pair acceptors and bases as electron pair donors, emphasizing electron transfer in reactions.

Acid-base titrations MCQs assess skills in calculating concentrations of acids and bases involved in neutralization reactions, crucial in analytical chemistry and quantitative analysis.

Acid-Base Theories Online Quiz

By presenting 3 options to choose from, Acid-Base Theories Quiz which cover a wide range of topics and levels of difficulty, making them adaptable to various learning objectives and preferences. You will have to read all the given answers of Acid-Base Theories Questions and Answers and click over the correct answer.

  • Test Name: Acid-Base Theories MCQ Quiz Practice
  • Type: Quiz Test
  • Total Questions: 40
  • Total Marks: 40
  • Time: 40 minutes

Note: Answer of the questions will change randomly each time you start the test. Practice each quiz test at least 3 times if you want to secure High Marks. Once you are finished, click the View Results button. If any answer looks wrong to you in Quiz, simply click on question and comment below that question, so that we can update the answer in the quiz section.

Acid-Base Theories MCQs

Acid-Base Theories Quiz

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According to Bronsted-Lowry theory, an acid is a

2 / 40

According to Lewis theory, a base is

3 / 40

An example of a Lewis base is

4 / 40

The Lewis theory focuses on the transfer of

5 / 40

A solution with a pH of 2 is

6 / 40

According to Lewis theory, an acid is

7 / 40

The formula for calculating pH is

8 / 40

In the reaction NH3 + BF3 → NH3BF3, NH3 acts as a

9 / 40

The self-ionization of water produces

10 / 40

Water can act as both an acid and a base, making it

11 / 40

According to Arrhenius theory, an acid produces

12 / 40

The ionization constant of water (Kw) at 25°C is

13 / 40

A strong acid completely

14 / 40

In the reaction HCl + H2O → H3O+ + Cl-, H2O acts as a

15 / 40

A weak acid

16 / 40

In the reaction NH3 + H2O → NH4+ + OH-, NH3 acts as a

17 / 40

An acid with a pKa of 3 is

18 / 40

A substance that can accept more than one proton per molecule is called a

19 / 40

In the reaction H2O + H2O → H3O+ + OH-, water acts as

20 / 40

A substance that can act as both an acid and a base is called

21 / 40

A solution with a pH of 12 is

22 / 40

According to Bronsted-Lowry theory, a base is a

23 / 40

In the reaction NH3 + BF3 → NH3BF3, BF3 acts as a

24 / 40

The pH of a solution is a measure of

25 / 40

The conjugate acid of H2O is

26 / 40

The conjugate acid of NH3 is

27 / 40

According to Arrhenius theory, a base produces

28 / 40

The strength of a base depends on its ability to

29 / 40

The strength of an acid depends on its ability to

30 / 40

The conjugate base of HCl is

31 / 40

The relationship between pH and pOH in a solution at 25°C is

32 / 40

The Bronsted-Lowry theory focuses on the transfer of

33 / 40

The pOH of a solution is a measure of

34 / 40

A strong base completely

35 / 40

The formula for calculating pOH is

36 / 40

The pH and pOH of a neutral solution at 25°C are both

37 / 40

An example of a Lewis acid is

38 / 40

The conjugate base of H2SO4 is

39 / 40

A substance that can donate more than one proton per molecule is called a

40 / 40

A weak base

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Acid-Base Theories Flashcards

According to Arrhenius theory, an acid produces

H+ ions in solution

According to Arrhenius theory, a base produces

OH- ions in solution

According to Bronsted-Lowry theory, an acid is a

proton donor

According to Bronsted-Lowry theory, a base is a

proton acceptor

The conjugate base of HCl is

Cl-

The conjugate acid of NH3 is

NH4+

According to Lewis theory, an acid is

an electron pair acceptor

According to Lewis theory, a base is

an electron pair donor

Water can act as both an acid and a base, making it

amphoteric

In the reaction NH3 + H2O → NH4+ + OH-, NH3 acts as a

Bronsted-Lowry base

In the reaction HCl + H2O → H3O+ + Cl-, H2O acts as a

Bronsted-Lowry base

A substance that can donate more than one proton per molecule is called a

polyprotic acid

A substance that can accept more than one proton per molecule is called a

polybasic base

The strength of an acid depends on its ability to

donate protons

The strength of a base depends on its ability to

accept protons

The ionization constant of water (Kw) at 25°C is

1 x 10^-14

In the reaction NH3 + BF3 → NH3BF3, BF3 acts as a

Lewis acid

In the reaction NH3 + BF3 → NH3BF3, NH3 acts as a

Lewis base

The pH of a solution is a measure of

H+ ion concentration

The pOH of a solution is a measure of

OH- ion concentration

A strong acid completely

dissociates in water

A weak acid

partially dissociates in water

A strong base completely

dissociates in water

A weak base

partially dissociates in water

The conjugate base of H2SO4 is

HSO4-

The conjugate acid of H2O is

H3O+

The Bronsted-Lowry theory focuses on the transfer of

protons

The Lewis theory focuses on the transfer of

electron pairs

The formula for calculating pH is

-log[H+]

The formula for calculating pOH is

-log[OH-]

A solution with a pH of 2 is

strongly acidic

A solution with a pH of 12 is

strongly basic

An example of a Lewis acid is

AlCl3

An example of a Lewis base is

NH3

A substance that can act as both an acid and a base is called

amphiprotic

The self-ionization of water produces

H3O+ and OH- ions

The pH and pOH of a neutral solution at 25°C are both

7

An acid with a pKa of 3 is

stronger than an acid with a pKa of 5

The relationship between pH and pOH in a solution at 25°C is

pH + pOH = 14

In the reaction H2O + H2O → H3O+ + OH-, water acts as

both an acid and a base

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