Acids and Bases

1. Properties

1.1. Bases

1.1.1. Bitter

1.1.2. high concentration of OH- ions

1.1.3. H^+ acceptor

1.1.4. slippery

1.2. Phenolphthalein - colourless (acid); pale pink (neutral); pink (base)

1.3. Acids

1.3.1. Sour

1.3.2. high concentration of H+ ions

1.3.3. H^+ donor

1.3.4. Sticky

1.4. amphoteric

1.4.1. can act as a base and an acid

2. Acids and base reaction

2.1. Acid + Metal ——-> Salt + Hydrogen (2HCl + Zn ——> ZnCl2 + H2

2.1.1. Acid + Carbonate ——-> Salt + water + Carbon Dioxide 2HCl + CaCO3 —-> Cacl2 H2O CO2

2.2. Acid + base ———> salt + water

2.2.1. ex. HCL(aq) + NaOH(aq) ————> NaCl(aq) + H2O(l)

3. Titration and indicators

3.1. litmus - red (acid); blue (alkali)

3.2. methyl orange - red (acid); yellow (alkali); orange (neutral)

3.3. universal indicator - red (acid), green (neutral), purple (alkali)

3.4. indicators change colour depending on the different concentrations of H+ ions

3.5. acid-base titrations are neutralisation reactions

3.6. Bromothymol Blue - yellow (acidic); green (neutral); blue (alkali)

3.7. titration involves reacting a measured volume of one of the solutions and adding the other solution gradually until the equivalence point is reached; exactly neutral

4. pH scale

4.1. The logarithm expression of the concentration of Hydrogen

4.1.1. E.g. The solution that has the [H+]=0.1mol/dm3 --> 10^-1 --> pH=1

4.2. 0 - 14 (0 most acidic, 7 neutral, 14 least acidic)

4.2.1. inversely related to H+

4.3. It can be measured by several pH indicators.

5. conjugated acids and base pairs

5.1. must have a receptor and donator

5.1.1. donation of H ions are not in isolation; it is reversible

5.2. acids; donate/loose H ions

5.3. base; acceptor/receive H ions

5.4. the pair differs in one proton

5.4.1. depending their acid and base nature