1.8 Acids, Bases And Salts
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Universal indicator at acidic, neutral and alkaline
Acidic - red Neutral - green Alkaline - purple
Phenolphthalein indicator at acidic, neutral and alkaline
Acidic - colourless Neutral - colourless Alkaline - pink
Methyl Orange indicator at acidic, neutral and alkaline
Acidic - red Neutral - orange Alkaline - yellow
Red litmus paper at acidic, neutral and alkaline
Acidic - red Neutral - red Alkaline - blue
Blue litmus at acidic, neutral and alkaline
Acidic - red Neutral - blue Alkaline - blue
Where are strong acids on the PH scale
0-2. Examples are hydrochloric, sulfuric or nitric acid
Where are weak acids on in the pH scale
3-6. Examples are ethanoic or carbonic
Where is neutral on the pH scale
7
Where are weak alkalis on the pH scale?
8-11. Examples are ammonia
Where are strong alkalis on the pH scale
12-14. Examples are sodium hydroxide or potassium hydroxide
What do acids produce when dissolved?
H+ (aq) ions. The higher the concentration of hydrogen ions, the stronger the acid is
What do alkalis produce when dissolved?
OH- (aq) ions
What do weak acids and alkalis do in water?
Only partially ionise
What do strong acids and alkalis do in water?
Completely ionise
Dilute
contains a Small number of particles dissolved per unit volume
Concentration
A measure of the number of moles of acid/alkali molecules dissolved in 1dm3 of water. Measured in mol/dm3. The higher the concentration the more acid/alkali molecules that have been dissolved
Neutralisation
The reaction between an acid and an alkali which produces salt and water
What is the ionic equation for neturalisation
H+ (aq) + OH- (aq) = H2O (l)
Is neutralisation an exothermic reaction?
Yes
Base
Metal oxide/hydroxide which neutralises an acid
Alkali
A soluble base
Acid + metal =
Salt + hydrogen
Acid + base =
Salt + water
Acid + alkali =
Salt + water