Acids, Bases and Salts 1 Flashcards
State the formula for ethanoic acid.
CH3COOH
State the ions produced in aqueous solution of the following acids:
1: hydrochloric acid
2: nitric acid
3: sulfuric acid
4: ethanoic acid
1: H+ (aq), Cl- (aq)
2: H+ (aq), NO3 ^- (aq)
3: H+ (aq), SO4 ^2- (aq)
4: H+ (aq), CH3COOH ^- (aq)
Define an acid.
An acid is a substance in which its molecules dissociate in water to produce hydrogen ions.
What factor is responsible for the properties of acids?
The presence of hydrogen ions.
Ammonia and ethanol are hydrogen-containing compounds. Why are they not acids?
They do not produce hydrogen ions when dissolved in water.
Define the basicity of an acid.
The number of ionisable hydrogen ions that can be produced by a molecule of the acid.
State the number of hydrogen ions that can be yielded when
1: a molecule of a monobasic acid is dissociated.
2: a molecule of a dibasic acid is dissociated.
3: a molecule of a tribasic acid is dissociated.
1: 1 H+ ion
2: 2 H+ ions
3: 3 H+ ions
Define the strength of an acid.
The extent of an acid’s dissociation in water.
Define a strong acid and a weak acid respectively.
A strong acid is one in which its molecules dissociate completely in water to produce a high concentration of hydrogen ions.
A weak acid is one in which its molecules dissociate partially in water to produce a low concentration of hydrogen ions.
Name two types of uses for the following acids.
1: H2SO4
3: HCl
5: CH3CO2H
Name one type of use for the following acids.
4: HNO3
5: H3PO4
6: H2CO3
1: fertiliser / car batteries / detergents
2: cleaning of metals / leather processing
3: vinegar / glue
4: fertiliser / explosives
5: fertiliser / food additives
6: soft drinks
State the difference between a dilute acid solution and a concentrated acid solution.
A dilute acid solution contains a small amount of dissolved acid per unit volume of water, while a concentrated acid solution contains a large amount of dissolved acid per unit volume of water.
What does pH measure?
pH measures the concentration of H+ ions in an aqueous solution of an acid.
State the formula of pH.
pH = -lg [H+], where H+ refers to the concentration of H+ ions in water
State the factors affecting pH of an acid solution.
Its strength, concentration and basicity.
List all the properties of an acid.
1: It has a sour taste.
2: It dissolves in water to form solutions that conduct electricity.
3: It turns blue litmus paper red.
4: It reacts with reactive metals to form hydrogen gas and a salt.
5: It reacts with all carbonates to form carbon dioxide, water and a salt.
6: It reacts metal oxides and metal hydroxides to form salt and water.
Identify the unreactive metals.
calcium (Ca)
zinc (Zn)
copper (Cu)
tin (Sn)
silver (Ag)
gold (Au)
lead (Pb)
platinum (Pl)
aluminium (Al)
iron (Fe)
Cu, Ag, Au, Pl
Identify the metals that can be displaced from their oxide using carbon.
tin (Sn)
magnesium (Mg)
zinc (Zn)
gold (Au)
lead (Pb)
silver (Ag)
aluminium (Al)
copper (Cu)
Sn, Zn, Au, Pb, Ag, Cu
Complete the chemical reaction.
CuO (s) + H2 (g) -> ?
CuO (s) + H2 (g) -> Cu (s) + H2O (l)
Predict the observation when a magnesium ribbon is added to hydrochloric acid.
Brisk effervescence of colourless, odourless gas that extinguished a lighted splint is observed.
Define a salt.
A salt is the ionic compound formed when the hydrogen ions from an acid are displaced by metals or ammonium ions. The anion of salt comes from an acid.