Acids and Bases

Question 1

What is a solution?

Answer 1

It is a completely perfect mixture of a solute and a solvent, where the particles of the solute are homogenous.

Question 2

What is concentration?

Answer 2

It is the amount of solute that is dissolved in a given volume of a solution.

Question 3

What is molarity?

Answer 3

It is the number of moles of solute per litre of solution.

Question 4

What is an Arrhenius acid?

Answer 4

It is a substance that dissociates in water to produce H+ ions (protons).

Question 5

What is an Arrhenius base?

Answer 5

It is a substance that dissociates in water to produce OH- ions (hydroxide).

Question 6

What is a Bronsted Lowry acid?

Answer 6

It is a H+ ion (proton) donor.

Question 7

What is a Bronsted Lowry base?

Answer 7

It is a H+ ion (proton) Accepter.

Question 8

What is neutralisation?

Answer 8

It is the reaction between an acid and a base, forming a salt and water aqueous solution.

Question 9

What is a conjugate acid?

Answer 9

A base that has accepted a H+ ion (proton).

Question 10

What is a conjugate base?

Answer 10

A base that has donated a H+ ion (proton).

Question 11

What is a conjugate pair?

Answer 11

An acid and a base that differ by a H+ ion (proton).

Question 12

What is a primary standard?

Answer 12

It is a reagent that can be weighed easily, and which is so pure that its weight is truly representative of the number of moles of substance contained.

Question 13

What is a titration?

Answer 13

It is a laboratory experiment where a measured volume of one solution is added to a known volume of another solution until the reaction is complete.

Question 14

What is a base called when it donates 1 H+ ion (proton)? Give an example of one.

Answer 14

A monobasic acid; HCl

Notice there’s only one H

Question 15

What is a base called when it donates 2 H+ ions (proton)? Give an example of one.

Answer 15

A dibasic acid; H2SO4

Notice there’s two H’s

Question 16

What is a base called when it donates 3 H+ ions (proton)? Give an example of one.

Answer 16

A tribasic acid; H3PO4

Notice there’s three H’s

Question 17

How do you classify acids?

Answer 17

Acids are classified as monobasic, dibasic, tribasic depending on the number of hydrogen atoms per molecule that are removed by a reaction with a base.

Question 18

In 1887, Arrhenius designed a theory to explain how water allows acids to show their acidic properties.

Solve;
A.) HX —> ?
B.) HCl —> ?
C.) H2SO4 —> ?

Answer 18

A.) HX —> (H+) + (X-)
B.) HCl —> (H+) + (Cl-)
C.) H2SO4 —> (2H+) + (SO4^2-)

Question 19

In 1887, Arrhenius designed a theory to explain how water allows bases to show their basic properties.

Solve;
NaOH —> ?

Answer 19

NaOH —> (Na+) + (OH-)

Question 20

What did Arrehenius believe about dissociating acids and bases?

Answer 20

• In solution, weak acids and bases only slightly dissociate.
• In solution, strong acids and bases fully dissociate.

Question 21

What are the two limitations to Arrhenius?

Answer 21

• It is limited to acid-base reactions that take place in water.
• It is also limited to bases that contain OH- ions.

Question 22

What do these Bronsted Lowry acids and bases change to?

A.) HCl + H2O —> ?
B.) NH3 + H2O —> ?
C.) HCl + NH3 —> ?

Answer 22

A.) HCl + H2O —> (Cl-) + (H3O+)
B.) NH3 + H2O —> (NH4+) + (OH-)
C.) HCl + NH3 —> (Cl-) + (NH4+)

Question 23

What is an amphoteric substance? Name an example.

Answer 23

It is a substance that can act as both an acid and a base.

For example, Water; (A: H2O —> OH-) (B: H2O —> H3O+

Question 24

What conjugate base does a strong acid produce?

Answer 24

It produces a weak conjugate base.

Question 25

What conjugate base does a weak acid produce?

Answer 25

It produces a strong conjugate base.

Question 26

How is a hydronium ion formed? Give the chemical equation.

Answer 26

A H+ ion (proton) cannot exist independently in water so it combines with a water molecule to form a hydronium ion. (H+) + (H2O) —> H3O+.

Question 27

Give the chemical equation for the self-ionisation of water.

Answer 27

H2O ⇌ (H+) + (OH-)