Acids and Bases

Question 1

Define an acid

Answer 1

proton donor

Question 2

define a base

Answer 2

proton acceptor

Question 3

define a strong acid

Answer 3

an acid which fully dissociates

Question 4

define a weak acid

Answer 4

an acid which only partially dissociates

Question 5

formula for pH

Answer 5

-Log10[H+]

Question 6

formula for [H+]

Answer 6

10^-pH

Question 7

The following are general equations you need to be able to recall and apply to real examples

Answer 7

Type 1 - Acid + Metal -> Salt + Hydrogen

Type 2 - Acid + Metal Oxide -> Salt + Water

Type 3 - Acid + Metal Hydroxide -> Salt + Water

Type 4 - Acid + Metal Carbonate -> Salt + CO2 + Water

Question 8

define monoprotic

Answer 8

acid is one which only releases one H+ ion

Question 9

As water can act as an acid or a base this property is called being

Answer 9

amphoteric

Question 10

A solution has a [H+] = 1.2x10-3 moldm-3. Calculate the pH

Answer 10

pH = -Log10[H+]

pH = -Log10[1.2x10-3]

pH = 2.92

Question 11

A solution has a pH of 12.33. Calculate [H+]

Answer 11

[H+] = 10-pH

[H+] = 10-12.33

[H+] = 4.68x10-13 moldm-3

Question 12

Recall 4 strong acids

Answer 12

Hydrochloric – HCl
Sulfuric - H2SO4
Nitric – HNO3
Phosphoric – H3PO4

Question 13

all carboxylic acids are

Answer 13

weak acids

Question 14

Explain why [H2O] is not shown in the Kw expression

Answer 14

water is almost constant