Bronsted Lowry Theory

Q. Which of the following is incorrectly paired?

1. $HN{O}_3$ - acid
2. $Mg(OH{)}_2$ - base
3. $N{H}_3$ - acid
4. $N{H}_{4}OH$ - base

Q.

Ammonia gas dissolves in water to give ammonium ion.In this reaction water acts as:

1. A base

2. An acid

3. A salt

4. A conjugate base

Q. Question 20
Mineral acids are stronger acids than carboxylic acids because
(i) Mineral acids are completely ionised
(ii) Carboxylic acids are completely ionised
(iii) Mineral acids are partially ionised
(iv) Carboxylic acids are partially ionised

(a) (i) and (iv)
(b) (ii) and (iii)
(c) (i) and (ii)
(d) (iii) and (iv)

Q.

Which of the following anion is present in compound A when warmed with dilute sulphuric acid gives a colourless gas which turns acidified potassium dichromate solution green.

1. SO₄^2-

2. S^2-

3. SO₃^2-

4. None of these

Q. $N{H}_3$ cannot release $O{H}^{-}$ ions. Can it be called a base?

1. Yes, $N{H}_3$ can release $O{H}^{-}$ ions and hence is a base.
2. No, $N{H}_3$ has hydrogen and hence is an acid.
3. No, a base should ionize in water to form $O{H}^{-}$ ions.
4. Yes, $N{H}_3$ can accept a proton.

Q. Assertion: Acetic acid does not act as an acid in benzene.
Reason: Benzene does not accept a proton.

1. Both assertion and reason are true and the reason is the correct explanation of assertion.
2. Both assertion and reason are true but the reason is not the correct explanation of assertion.
3. The assertion is true but the reason is false.
4. Both assertion and reason are false.

Q. What is monobasic acid?

Q. What are strong and weak acids? Categorise the following into strong and weak acids.
Hydrochloric acid, citric acid, acetic acid, nitric acid, formic acid, sulphuric acid.

Q.

Which one is an acidic salt?

1. $N{H}_{4}Cl$

2. $C{H}_{3}COONa$

3. $KCl$

4. $NaCl$

Q.

A compound HA when react with S, it dissociates as shown below:

$HA+S\rightleftharpoons$ $A^{-}$ + $S{H}^{+}$

What is S and A?

1. S is Bronsted acid and A is Bronsted base

2. Both S and A are Bronsted lowry acid

3. Both S and A are Bronsted lowry base

4. S is Bronsted Lowry base and A is Bronsted Lowry acid

Q. Which of these is incorrectly matched?

1. $HN{O}_3$ - acid
2. $Mg(OH{)}_2$ - base
3. $N{H}_3$ - acid
4. $N{H}_{4}OH$ - base

Q. An aqueous solution of release ${\text{H}}^{+}$ ions.

1. acids
2. bases
3. alkalis

Q. Where does the equivalence point occur on a titration curve for a strong acid/strong base titration?

1. At the endpoint, after pH 7.
2. At pH 7, in the middle of the dramatic slope.
3. At the very end of titration, between pH 10-12.
4. Before the slope increases dramatically, between pH 2 and 4.

Q. Assertion: If ${\lambda }_{N{a}^{+}}^{\circ }+{\lambda }_{C{l}^{-}}^{\circ }$ are molar limiting conductivity of the sodium and chloride ions respectively, then the limiting molar conducting for sodium chloride is given by the equation: ${\lambda }_{NaCl}^{\circ }={\lambda }_{N{a}^{+}}^{\circ }+{\lambda }_{C{l}^{-}}^{\circ }$
Reason:This is according to Kohlrausch law of independent migration of ions.

1. If both assertion and reason are true and the reason is the correct explanation of the assertion.
2. If assertion is true but reason is false.
3. If both assertion and reason are true but reason is not the correct explanation of the assertion.
4. If the assertion and reason both are false.

Q. ${\text{NH}}_3$ cannot release ${\text{OH}}^{-}$ ions. It is .

1. a base
2. an acid
3. neutral

Q.

Calcium hydroxide is a

1. weak acid

2. weak base

3. strong acid

4. strong base

Q. Why is the Bronsted-Lowry definition of acids and bases more encompassing than the Arrhenius definition?

Q. Consider these two equations:
(i) $C{l}^{-}+H^{+}\to HCl$
(ii) $C{H}_{3}COOH\to C{H}_{3}CO{O}^{-}+H^{+}$
Which of the following statements is correct?

1. $C{l}^{-}$ is a Bronsted-Lowry base
2. $H^{+}$ is a Bronsted-Lowry base
3. $C{H}_{3}COOH$ is a Bronsted-Lowry base
4. None of the above

Q. $N{H}_3$ cannot release $O{H}^{-}$ ions. Can it be a base?

1. Yes, $N{H}_3$ can release OH- ions and hence is a base.
2. No, $N{H}_3$ has hydrogens and hence is an acid.
3. No, a base should ionize in water to form $O{H}^{-}$ ions.
4. Yes, $N{H}_3$ can accept a proton.

Q. Which feature of the ammonia molecule leads to the formation of the ammonium ion when ammonia dissolves in water.

Q. Match the type of acid/base with the corresponding example.

1. $NaOH$
2. $N{H}_{4}OH$
3. $C{H}_{3}COOH$
4. $HCl$

Q. Which of these is incorrectly matched?

1. $HN{O}_3$ - acid
2. $Mg(OH{)}_2$ - base
3. $N{H}_3$ - acid
4. $N{H}_{4}OH$ - base

Q. Consider these two equations:
(i) $HN{O}_3\left(aq\right)+H_{2}O\left(l\right)\to H_3{O}^{+}\left(aq\right)+N{O}_3{}^{-}\left(aq\right)$
(ii) $N{H}_3\left(g\right)+HCl\left(g\right)\to N{H}_4^{+}\left(s\right)+Cl{}^{-}\left(s\right)$
Which of the following statements is/are correct?

1. $H^{+}$ is a Bronsted-Lowry base
2. $C{l}^{-}$ s a Bronsted-Lowry base
3. $C{H}_{3}COOH$ is a Bronsted-Lowry base
4. None of the above

Q.

According to Bronsted Lowry theory, acids are defined as:

1. Proton acceptor

2. Proton donor

3. Electron donor

4. Electron acceptor

Q. An acid produces free $H+$ ions in aqueous solution.

1. True
2. False

Q.

A compound HA when reacting with S, it dissociates as shown below:

$HA+S\rightleftharpoons$ $A^{-}$ + $S{H}^{+}$

What are S and A?

1. Both S and A are Bronsted Lowry base.

2. Both S and A are Bronsted Lowry acid.

3. S is Bronsted acid and A is Bronsted base.

4. S is Bronsted Lowry base and A is Bronsted Lowry acid.

Q. $N{a}^{+},M{g}^{2+},A{l}^{3+}$ and $S{i}^{4+}$ are isoelectronic ions. Their ionic size will follow the order:

1. $N{a}^{+}<M{g}^{2+}<A{l}^{3+}<S{i}^{4+}$
2. $N{a}^{+}>M{g}^{2+}<A{l}^{3+}<S{i}^{4+}$
3. $N{a}^{+}<M{g}^{2+}>A{l}^{3+}>S{i}^{4+}$
4. $N{a}^{+}>M{g}^{2+}>A{l}^{3+}>S{i}^{4+}$

Q. Consider the two equations given below:
(i) $C{l}^{-}+H^{+}\to HCl$
(ii) $C{H}_{3}COOH\to C{H}_{3}CO{O}^{-}+H^{+}$
Which of the following statements is correct?

1. $C{l}^{-}$ is a Bronsted-Lowry base
2. $H^{+}$ is a Bronsted-Lowry base
3. $C{H}_{3}COOH$ is a Bronsted-Lowry base
4. None of the above

Q.

According to Bronsted Lowry theory, acids are defined as:

1. Proton acceptor

2. Electron acceptor

3. Proton donor

4. Electron donor

Q. Phosphorus pentoxide forms phosphates when fused with :

1. basic oxides
2. acidic sulphides
3. acidic oxides
4. basic sulphides