What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid.

a) HNO 3 +H 2 O  →

b) HSO 4 − +H 2 O  →

c) s H 3 O + +F − →

Interpretation:

The products of each of the acid –base reactions, the acid and its conjugate base and the base and its conjugate acid has to be written.

Concept Introduction:

Arrhenius Acids and Bases

Acid release hydrogen ion in water

Base release hydroxide ions in water.

HCl(aq) →H+(aq) + Cl-(aq).........AcidNaOH(aq) →Na+(aq)+ OH-(aq)...........Base

An acid is a substance that produces hydronium ions, H3O+ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair.

A Lewis base is a substance that can donate and share an electron pair.

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

The reaction of HNO3 and H2O is given below,

HNO3+H2O  ⇌H3O+    +    NO2-Acid     Base         acid            base                   

Acid and its conjugated base:

The products of the above reaction are as following

Interpretation:

The products of each of the acid –base reactions, the acid and its conjugate base and the base and its conjugate acid has to be written.

Concept Introduction:

Arrhenius Acids and Bases

Acid release hydrogen ion in water

Base release hydroxide ions in water.

HCl(aq) →H+(aq) + Cl-(aq).........AcidNaOH(aq) →Na+(aq)+ OH-(aq)...........Base

An acid is a substance that produces hydronium ions, H3O+ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair.

A Lewis base is a substance that can donate and share an electron pair.

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

Interpretation:

The products of each of the acid –base reactions, the acid and its conjugate base and the base and its conjugate acid has to be written.

Concept Introduction:

Arrhenius Acids and Bases

Acid release hydrogen ion in water

Base release hydroxide ions in water.

HCl(aq) →H+(aq) + Cl-(aq).........AcidNaOH(aq) →Na+(aq)+ OH-(aq)...........Base

An acid is a substance that produces hydronium ions, H3O+ when dissolved in water.

Bronsted –Lowry definitions:

A Bronsted –Lowry acid is a proton donor, it donates a hydrogen ion, H+

A Bronsted-Lowry base is a proton acceptor, it accepts a hydrogen ion H+.

Lewis definition:

A Lewis acid is a substance that can accept and share an electron pair.

A Lewis base is a substance that can donate and share an electron pair.

Bronsted –Lowry conjugate acid-Base pairs:

When an acid is dissolved in water, the acid (HA) donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).