Acids, Bases, Salts

Question 1

Acid

Answer 1

A H+ donator.

Question 2

Weak Acid

Answer 2

partially dissociates (only some H+ ions dissosisted)

Question 3

Examples of weak acids

Answer 3

ethanoic acid CH3COOH
citric acid C6H8O7
formic acid CHOOH
phosphoric acid H3PO4

Question 4

Strong acid

Answer 4

Fully dissosisted in aqueous solution

Question 5

Examples of strong acids

Answer 5

Hydrochloric Acid HCl
Sulfuric Acid H2SO4
Nitric Acid HNO3

Question 6

Base

Answer 6

A h+ ion acceptor

Question 7

Alkali

Answer 7

A soluble base and release OH- ions in solution

Question 8

Salt

Answer 8

An ionic substance formed when the H+ ions of an acid are replaced by metal ions or ammonium ions.

Question 9

Concentration

Answer 9

The amount in moles of acid per until vol of solution.

Question 10

Strength (of acid)

Answer 10

Related to the proportion of the acid that is dissosisted in aqueous solution.

Question 11

Test for sulfate ions

Answer 11

Add barium nitrate

White precipitate formed

Question 12

Test for Carbonate ions

Answer 12

Add dilute HCl
Effervescent occurs
Bubble gas through limewater
White precipitate formed

Question 13

Test for ammonia ions

Answer 13

Add sodium hydroxide 
Ammonia gas formed
Warm solution in water bath
Place damp red litmus in mouth if test tube 
Litmus paper will turn blue

Question 14

Test for Chloride ions

Answer 14

Add silver nitrate
White precipitate formed
When added to dilute and concentrated ammonia precipitate redesolves

Question 15

Test for bromide ions

Answer 15

Add silver nitrate
Cream precipitate forms
When added to dilute ammonia precipitate remains
When added to concentrated ammonia precipitate redesolves

Question 16

Test for iodide ions

Answer 16

Add silver nitrate
Yellow precipitate formed
When added to dilute and concentrated ammonia precipitate remains

Question 17

How does the equation showing the dissociation of acids

Answer 17

strong acids fully dissociate so reaction is one way:
HCl –> H+ + Cl-
weak acids partially dissociate so reaction is reversible:
CH3COOH CH3COO- + H+

Question 18

Coomon Alkalis

Answer 18

Sodium Hydroxide NaOH
Potassium Hydroxide KOH
Ammonia NH3

Question 19

Types of bases

Answer 19

Metal Hydroxides - OH- can accept 1 H+ ion to form water

Metal Oxides - Can accept 1 H+ ion to form a hydroxide or 2 to form water

Question 20

Ammonia as a base and alkali

Answer 20

Ammonia is an alkali as it’s soluble in water however can act as a base as it contains a nitrogen with a lone pair of electrons which can form a bond with a H+ ion to form NH4+

Question 21

how can water act as an acid and a base

Answer 21

Water can act as an acid as it can donate a H+ ion:
H2o -> OH- + H+

Water can also act as a base by accepting a H+ ion:
H2O + H+ -> H3O+ (hydronium ion)

Question 22

Acid + Alkali

Answer 22

Salt + Water

Question 23

Acid + Metal Oxide

Answer 23

Salt + Water

Question 24

Acid + Metal carbonate

Answer 24

Salt + Carbon Dioxide + Water

Question 25

Acid+ Metal hydrogen carbonate

Answer 25

Salt + Carbon Dioxide + Water

Question 26

Acid + Metal Hydroxide

Answer 26

Salt + Water

Question 27

Acid + Reactive Metal

Answer 27

Salt+ Hydrogen

Question 28

Always soluble ions

Answer 28

Group 1 ions Ammonium NH4+ Nitrate NO3- Hydrogen carbonate HCO3-

Question 29

Soluble ions with exeption

Answer 29

``` Halide ions ( Cl- Br- I-) expect when combined with Ag+ Pb2+ Hg2+(mercury) Sulfate SO42- except when combined with Ag+ Pb2+ Ca2+ Sr2+ Ba2+ ```

Question 30

insoluble ions

Answer 30

oxide unless combined with group 1 metal or Ca2+ or Ba2+ Carbonate unless combined with group 1 metal or ammonium phosphate unless combined with group 1 metal or ammonium

Question 31

insoluble ions

Answer 31

hydroxide unless combined with group 1 metal or ammonium or Ca2+ Mg2+ Sr2+ or Ba2+ Sulfide unless combined with group 1 metal or ammonium Dichromate (cr2O72-) unless combined with group 1 metal or ammonium or Ca2+ or Mg2+