Acids and Bases

Question 1

Who gave the Arrhenius Theory of Acids and Bases?

Answer 1

Svante Arrhenius, 1884

Question 2

What is an Arrhenius acid and an Arrhenius base?

Answer 2

Arrhenius acid- Releases H+ ions in water.
Arrhenius base- Releases OH- ions in water.

Question 3

Which acid base theory describes neutralization reaction?

Answer 3

Arrhenius Theory.

Question 4

What is neutralization reaction?

Answer 4

Acid and base react to give salt and water.

Question 5

How is water formed as a result of neutralization reaction?

Answer 5

Proton is given by the caid and OH- ion is given by the base that combine and form water.

Question 6

What is a Bronsted base and a Bronsted acid?

Answer 6

Bronsted acid- Proton donor
Bronsted base- Proton acceptor

Question 7

True or False: Organic acids are classified as Bronsted acids.

Answer 7

True.

Question 8

Why is ammonia considered a Bronsted base?

Answer 8

Nitrogen has three bonds with three hydrogen atoms, and one lone pair of e-, which accepts a proton from water, to release OH- ions.

Question 9

What is the difference between monoprotic and polyprotic acids?

Answer 9

Monoprotic acids- contain only one ionizable hydrogen.
Eg. HCl, HNO3
Polyprotic acids- contain more than one ionizable hydrogen.
Eg. H2SO4, H3PO4

Question 10

Organic acids have many hydrogens, yet they donate only ______ hydrogens.

Answer 10

Acidic.

Question 11

What determines whether a hydrogen atom is acidic?

Answer 11

If it is attached to a more electronegative atom like a halide or an oxygen.

Question 12

How does the Bronsted-Lowry theory explain acid base reactions?

Answer 12

1. Acid base reactions are a charge transfer process.
2. This transfer process usually involves the solvent.
3. Acid base reactions can be considered reversible. This leads to a possibility of a reversible, dynamic, equilibrium.

Question 13

What is a conjugate acid and a conjugate base?

Answer 13

Conjugate acid- Base that accepted a proton.
Conjugate base- Acid that donated a proton.

Question 14

What is the relationship between a conjugate acid-base pair?

Answer 14

• Conjugate acid- base pair differ by one proton.
• The stronger an acid, the weaker it’s conjugate base and vice versa.

Question 15

What are the characteristics of a strong acid/base?

Answer 15

• Strength is determined by degree of dissociation, not concentration.
• Good electrolytes.
• Donate or accept protons with ease

Question 16

What is the difference in strong acids and weak acids?

Answer 16

Strong acids:
* Dissociate completely.
* Reversibility is insignificant as equilibrium lies to the right of the reaction.

Weak acids:
* Partially dissociate.
* At equilibrium, it is present in molecular form.

Question 17

Why is water considered amphiprotic?

Answer 17

Because it shows acidic as well as basic properties.
In reaction with a base, it donates proton (Hydrogen atom)
In reaction with an acid, it accepts proton (Lone pair on Oxygen atom).

Question 18

Solute-solvent interactions of acids/bases and water promote __________ and ____________.

Answer 18

Solubility and dissociation.

Question 19

What are the uses of acids?

Answer 19

1. Ascorbic Acid- Vitamin C- Micronutrient and a reducing agent.
2. Gastric acid- HCl- Helps digest proteins; increased concentration can cause indigestion and heartburn.
3. Biochemical Reactions- Enzymes function only in specific pH/ acidity.
4. Cell reactions are based on specific acid- base composition.

Question 20

What acid gives flavor to Swiss cheese?

Answer 20

Propanoic acid.