1. Acid-Base Equilibria L.O.: To be able to explain how an indicator works.

2. Acid-base indicators Most indicators are weak acids that partially dissociate in aqueous solution HIn (aq) H + (aq) + In¯ (aq) The un-ionised form (HIn) is a different colour to the anionic form (In¯). You can apply Le Chatelier’s Principle to predict any colour change In acid the increase of [H + ] causes the equilibrium to move to the left to give red undissociated form In alkali the increase of [OH¯] causes the OH¯ ions to remove H + ions to form water; H + (aq) + OH¯(aq) H 2 O(l) Therefore the equilibrium will move to the right, producing more H+ ions and giving a blue colour Overall: In acidic solution HIn (aq) H + (aq) + In¯ (aq) In alkaline solution

3. COLOUR CHANGES OF SOME COMMON INDICATORS They must have an easily observed colour change. They must change immediately in the required pH range over the addition of ‘half’ a drop of reagent. Acid-base indicators PHENOLPHTHALEIN LITMUS METHYL ORANGE 1234567891011121314 CHANGE pH

4. To be useful, an indicator must change over the “vertical” section of the curve where there is a change in pH of MORE THAN 2 pH units for the addition of a very small volume of alkali. The indicator used depends on the pH changes around the end point - the indicator must change during the ‘vertical’ portion of the curve. In the example, the only suitable indicator is PHENOLPHTHALEIN. Acid-base indicators PHENOLPHTHALEIN LITMUS METHYL ORANGE

5. pH curves There are four types of acid-base titration; each has a characteristic curve. strong acid (HCl) v. strong base (NaOH) weak acid (CH 3 COOH) v. strong alkali (NaOH) strong acid (HCl) v. weak base (NH 3 ) weak acid (CH 3 COOH) v. weak base (NH 3 ) In the following examples, alkali (0.1M) is added to 25cm 3 of acid (0.1M) End points need not be “neutral‘ due to the phenomenon of salt hydrolysis (see buffer notes if not sure about this!)

6. Very little pH change during the initial 20cm 3 Very sharp change in pH over the addition of less than half a drop of NaOH Curve levels off at pH 13 due to excess 0.1M NaOH (a strong alkali) strong acid (HCl) v. strong base (NaOH) pH 1 at the start due to 0.1M HC l (strong monoprotic acid)

7. strong acid (HC l ) v. strong base (NaOH) Any of the indicators listed will be suitable - they all change in the ‘vertical’ portion PHENOLPHTHALEIN LITMUS METHYL ORANGE

8. Very little pH change during the initial 20cm 3 Sharp change in pH over the addition of less than half a drop of NH 3 Curve levels off at pH 10 due to excess 0.1M NH 3 (a weak alkali) pH 1 at the start due to 0.1M HC l strong acid (HC l ) v. weak base (NH 3 )

9. PHENOLPHTHALEIN LITMUS METHYL ORANGE strong acid (HCl) v. weak base (NH 3 ) Only methyl orange is suitable - it is the only one to change in the ‘vertical’ portion

10. Steady pH change Sharp change in pH over the addition of less than half a drop of NaOH Curve levels off at pH 13 due to excess 0.1M NaOH (a strong alkali) pH 4 due to 0.1M CH 3 COOH (weak monoprotic acid) weak acid (CH 3 COOH) v. strong base (NaOH)

11. PHENOLPHTHALEIN LITMUS METHYL ORANGE Only phenolphthalein is suitable - it is the only one to change in the ‘vertical’ portion weak acid (CH 3 COOH) v. strong base (NaOH)

12. weak acid (CH 3 COOH) v. weak base (NH 3 ) Steady pH change pH 4 due to 0.1M CH 3 COOH (weak monoprotic acid) NO SHARP CHANGE IN pH Curve levels off at pH 10 due to excess 0.1M NH 3 (a weak alkali)

13. PHENOLPHTHALEIN LITMUS METHYL ORANGE NOTHING SUITABLE There is no suitable indicator- none change in the ‘vertical’ portion. The end point can be detected by plotting a curve using a pH meter. weak acid (CH 3 COOH) v. weak base (NH 3 )