Topic 3- Acids (paper 1)

Question 1

Hydrochloric acid

Answer 1

HCl

Question 2

Nitric acid

Answer 2

HNO3

Question 3

Sulphuric acid

Answer 3

H2SO4

Question 4

Phosphoric acid

Answer 4

H3PO4

Question 5

Ethanoic acid

Answer 5

CH3COOH

Question 6

Carbonic acid

Answer 6

H2CO3

Question 7

Citric acid

Answer 7

C6H8O7

Question 8

What ion causes a solution to be acidic?

Answer 8

Hydrogen

Question 9

What ion causes a solution to be alkaline?

Answer 9

Hydroxide ion

Question 10

What makes an acid strong/weak?

Answer 10

Whether the acid molecules have dissociated to make ions (stronger) or not (weaker).

Question 11

Define bases?

Answer 11

Bases are substances that can neutralise acids.

Question 12

metal + acid → ?

Answer 12

Metal salt + hydrogen

Question 13

Base (alkali) + acid → ?

Answer 13

Metal salt + water

Question 14

Metal carbonate + acid → ?

Answer 14

Metal salt + water + carbon dioxide

Question 15

Ammonia + acid → ?

Answer 15

Ammonium salts

Question 16

What is the pH of acids

Answer 16

Below 7

Question 17

What is the pH of alkalis?

Answer 17

Above 7

Question 18

What are alkalis?

Answer 18

Soluble bases

Question 19

What causes the pH of a solution to decrease by 1?

Answer 19

10 times more hydrogen ions

Question 20

metal oxide + acid → ?

Answer 20

metal oxide + acid → salt + water

Question 21

What would be done in order to create CuCl? (a soluable salt)

Answer 21

2HCL + CuO → CuCl2 +H2O

Question 22

How could a soluble salt be created?

Answer 22

• reacting an acid with an insoluble salt
• reacting an acid with an alkali

Question 23

Why must a titration be used when reacting an acid and an alkali to form a soluble salt

Answer 23

A titration mus be used in order to see how much acid is needed to neutralise an alkaline solution- and vice-versa- therefore preventing the solution from becoming too acidic or alkaline.