p H calculations p H calculations CONTENTS What
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p. H calculations
p. H calculations CONTENTS • What is p. H? - a reminder • Calculating the p. H of strong acids and bases • Calculating the p. H of weak acids • Calculating the p. H of mixtures - strong acid and strong alkali
p. H calculations Before you start it would be helpful to… • know the differences between strong and weak acid and bases • be able to calculate p. H from hydrogen ion concentration • be able to calculate hydrogen ion concentration from p. H • know the formula for the ionic product of water and its value at 25°C
What is p. H? p. H = - log 10 [H+(aq)] where [H+] is the concentration of hydrogen ions in mol dm-3 to convert p. H into hydrogen ion concentration IONIC PRODUCT OF WATER [H+(aq)] = antilog (-p. H) Kw = [H+(aq)] [OH¯(aq)] mol 2 dm-6 = 1 x 10 -14 mol 2 dm-6 (at 25°C)
Calculating p. H - strong acids and alkalis WORKED EXAMPLE Strong acids and alkalis completely dissociate in aqueous solution It is easy to calculate the p. H; you only need to know the concentration Calculate the p. H of 0. 02 M HCl completely dissociates in aqueous solution HCl H+ + Cl¯ One H+ is produced for each HCl dissociating so [H+] = 0. 02 M = 2 x 10 -2 mol dm-3 p. H = - log [H+] = 1. 7
Calculating p. H - strong acids and alkalis WORKED EXAMPLE Strong acids and alkalis completely dissociate in aqueous solution It is easy to calculate the p. H; you only need to know the concentration Calculate the p. H of 0. 02 M HCl completely dissociates in aqueous solution HCl H+ + Cl¯ One H+ is produced for each HCl dissociating so [H+] = 0. 02 M = 2 x 10 -2 mol dm-3 p. H = - log [H+] = 1. 7 Calculate the p. H of 0. 1 M Na. OH completely dissociates in aqueous solution Na. OH One OH¯ is produced for each Na. OH dissociating [OH¯] = 0. 1 M = 1 x 10 -1 mol dm-3 Kw = [H+][OH¯] = 1 x 10 -14 mol 2 dm-6 The ionic product of water (at 25°C) therefore Na+ + OH¯ [H+] = Kw / [OH¯] = 1 x 10 -13 mol dm-3 p. H = - log [H+] = 13
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) H+(aq) + A¯(aq) (1)
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) Applying the Equilibrium Law Ka = H+(aq) + A¯(aq) [H+(aq)] [A¯(aq)] [HA(aq)] mol dm-3 (1) (2)
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) Applying the Equilibrium Law Ka = H+(aq) + A¯(aq) [H+(aq)] [A¯(aq)] mol dm-3 (1) (2) [HA(aq)] The ions are formed in equal amounts, so therefore [H+(aq)] = [A¯(aq)] Ka = [H+(aq)]2 [HA(aq)] (3)
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) Applying the Equilibrium Law Ka = H+(aq) + A¯(aq) [H+(aq)] [A¯(aq)] mol dm-3 (1) (2) [HA(aq)] The ions are formed in equal amounts, so therefore [H+(aq)] = [A¯(aq)] Ka = [H+(aq)]2 [HA(aq)] Rearranging (3) gives therefore [H+(aq)]2 = [H+(aq)] = [HA(aq)] Ka (3)
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) Applying the Equilibrium Law Ka = H+(aq) + A¯(aq) [H+(aq)] [A¯(aq)] mol dm-3 (1) (2) [HA(aq)] The ions are formed in equal amounts, so therefore [H+(aq)] = [A¯(aq)] Ka = [H+(aq)]2 [HA(aq)] Rearranging (3) gives therefore [H+(aq)]2 = [H+(aq)] = p. H [HA(aq)] Ka = [H+(aq)] (3)
Calculating p. H - weak acids A weak acid is one which only partially dissociates in aqueous solution A weak acid, HA, dissociates as follows HA(aq) Applying the Equilibrium Law Ka = H+(aq) + A¯(aq) [H+(aq)] [A¯(aq)] mol dm-3 (1) (2) [HA(aq)] The ions are formed in equal amounts, so therefore [H+(aq)] = [A¯(aq)] Ka = [H+(aq)]2 (3) [HA(aq)] Rearranging (3) gives therefore [H+(aq)]2 = [H+(aq)] = p. H ASSUMPTION [HA(aq)] Ka = [H+(aq)] HA is a weak acid so it will not have dissociated very much. You can assume that its equilibrium concentration is approximately that of the original concentration.
WORKED EXAMPLE Calculating p. H - weak acids Calculate the p. H of a weak acid HX of concentration 0. 1 M ( Ka = 4 x 10 -5 mol dm-3 ) HX dissociates as follows HX(aq) H+(aq) + X¯(aq)
WORKED EXAMPLE Calculating p. H - weak acids Calculate the p. H of a weak acid HX of concentration 0. 1 M ( Ka = 4 x 10 -5 mol dm-3 ) HX dissociates as follows Dissociation constant for a weak acid HX(aq) Ka H+(aq) = + X¯(aq) [H+(aq)] [X¯(aq)] [HX(aq)] mol dm-3
WORKED EXAMPLE Calculating p. H - weak acids Calculate the p. H of a weak acid HX of concentration 0. 1 M ( Ka = 4 x 10 -5 mol dm-3 ) HX dissociates as follows Dissociation constant for a weak acid HX(aq) Ka H+(aq) = + X¯(aq) [H+(aq)] [X¯(aq)] mol dm-3 [HX(aq)] Substitute for X¯ as ions are formed in equal amounts and then rearrange equation [H+(aq)] = [HX(aq)] Ka mol dm-3
WORKED EXAMPLE Calculating p. H - weak acids Calculate the p. H of a weak acid HX of concentration 0. 1 M ( Ka = 4 x 10 -5 mol dm-3 ) HX dissociates as follows Dissociation constant for a weak acid HX(aq) Ka H+(aq) = + X¯(aq) [H+(aq)] [X¯(aq)] mol dm-3 [HX(aq)] Substitute for X¯ as ions are formed in equal amounts and the rearrange equation [H+(aq)] = [HX(aq)] Ka mol dm-3 ASSUMPTION HA is a weak acid so it will not have dissociated very much. You can assume that its equilibrium concentration is approximately that of the original concentration
WORKED EXAMPLE Calculating p. H - weak acids Calculate the p. H of a weak acid HX of concentration 0. 1 M ( Ka = 4 x 10 -5 mol dm-3 ) HX dissociates as follows HX(aq) Dissociation constant for a weak acid Ka H+(aq) = + X¯(aq) [H+(aq)] [X¯(aq)] mol dm-3 [HX(aq)] Substitute for X¯ as ions are formed in equal amounts and the rearrange equation [H+(aq)] = [HX(aq)] Ka mol dm-3 ASSUMPTION HA is a weak acid so it will not have dissociated very much. You can assume that its equilibrium concentration is approximately that of the original concentration [H+(aq)] ANSWER = 0. 1 x 4 x 10 -5 mol dm-3 = 4. 00 x 10 -6 mol dm-3 = 2. 00 x 10 -3 mol dm-3 p. H = - log [H+(aq)] = 2. 699
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