Acids Flashcards
What do all acids contain?
Hydrogen in their formula
What do all acids do in aqueous solutions?
Release H+ ions
What are the 4 most common acids and their formulas?
- Hydrochloric acid : HCl
- Sulfuric acid : H2SO4
- Nitric acid : HNO3
- Ethanoic acid : CH3COOH
What is a base?
A substance that neutralises an acid to form a salt
What is an alkali?
A base that releases hydroxide ions when is aqueous solution eg. NaOH (s) + aq -> Na + (aq) + OH - (aq)
What are metal oxides and carbonates classed as?
Bases
What are some common alkalis?
- Sodium hydroxide : NaOH
- Potassium hydroxide : KOH
- Ammonia : NH3
What is a strong acid?
An acid that releases all of its hydrogen atoms into solution as H+ ions and completely dissociates in aqueous solution
eg. HCl (aq) -> H+ (aq) + Cl- (aq)
What is a weak acid>
An acid that only releases a small proportion of its available hydrogen atoms into solution as H+ ions - it only partially dissociates in aqueous solution
eg. CH3COOH (aq) <=> H+ (aq) + CH3COO- (aq)
The <=> indicates that the forward reaction is incomplete
H+ (aq) + OH- (aq) ->
H2O (l)
Acid + base ->
Salt + water
HCl + NaOH -> NaCl + H2O
Acid + metal ->
Salt + hydrogen
2 HCl (aq) + Zn (s) -> ZnCl2 (aq) + H2 (g)
Acid + metal oxide ->
salt + water
2HCl (aq) + CaO (s) -> CaCl2 (aq) + H2O (l)
Acid + metal hydroxide ->
Salt + water
H2SO4 (aq) + Mg(OH)2 (s) -> MgSO4 (aq) + 2H2O (l)
Acid + metal carbonate ->
Salt + water + carbon dioxide
2HNO3 (aq) + CuCO3 (s) -> Cu(NO3)2 (aq) + H2O(l) + CO2 (g)
What is a titration?
A technique used to accurately measure the volume of one solution that reacts exactly with another that reacts exactly with another solution
What can a titration be used for?
- Finding the concentration for a solution
- Identification of unknown compounds
- Finding the purity of a substance
How do you prepare a standard solution?
How do you carry out a basic acid-base titration?
What are the steps in carrying out titration calculations?
1) Work out the amount, in mole, of the solute in the solution for which you know the concentrations and moles
2) Use the equation to work out the amount, in mole, of the solute in the other solution (using mole ratios/ stoichometry)
3) Work out the unknown information about the solute in the other solution
