14.1
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understand that a Brønsted–Lowry acid is a proton donor and a Brønsted–Lowry base is a proton acceptor and that acid-base reactions involve proton transfer
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14.2
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be able to identify Brønsted–Lowry conjugate acid-base pairs
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14.3
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be able to define the term ‘pH’
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14.4
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be able to calculate pH from hydrogen ion concentration
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14.5
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be able to calculate the concentration of hydrogen ions in a solution, in mol dm-3, from its pH, using the expression [H+] = 10-pH
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14.6
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understand the difference between a strong acid and a weak acid in terms of the degree of dissociation
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14.7
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be able to calculate the pH of a strong acid
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14.8
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be able to deduce the expression for the acid dissociation constant, Ka, for a weak acid
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14.9
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14.10
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be able to define the ionic product of water, Kw
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14.11
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be able to calculate the pH of a strong base from its concentration, using Kw or pKw
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14.12
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be able to define the terms ‘pKa’ and ‘pKw’
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14.13
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be able to analyse data from the following experiments:
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14.14
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be able to calculate Ka for a weak acid from experimental data given the pH of a solution containing a known mass of acid
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14.15
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be able to draw and interpret titration curves, using all combinations of strong and weak monoprotic and diprotic acids with bases, and apply these principles to diprotic acids and bases
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14.16
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be able to select a suitable indicator for a titration, using a titration curve and appropriate data
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14.17
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know what is meant by the term ‘buffer solution’
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14.18
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understand the action of a buffer solution
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14.19
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be able to calculate the pH of a buffer solution given appropriate data
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14.20
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be able to calculate the concentrations of solutions required to prepare a buffer solution of a given pH
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14.21
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understand how to use a weak acid-strong base or strong acid-weak base titration curve to:
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14.22
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understand the importance of buffer solutions in biological environments:
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14.23
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CORE PRACTICAL 11
Finding the Ka value for a weak acid. |
Further suggested practicals:
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