Acid-base Equilibria

Brønsted-Lowry Acids and Bases and pHSign up

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 · be able to identify Brønsted-Lowry conjugate acid-base pairs · be able to define the term 'pH' · be able to calculate pH from hydrogen ion concentration · 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

Strong and Weak Acids and Bases (Ka, Kw)Sign up

understand the difference between a strong acid and a weak acid in terms of the degree of dissociation · be able to calculate the pH of a strong acid · be able to deduce the expression for the acid dissociation constant, Ka, for a weak acid · be able to calculate the pH of a weak acid from Ka or pKa values, making relevant assumptions (students will not be expected to solve quadratic equations) · be able to define the ionic product of water, Kw · be able to calculate the pH of a strong base from its concentration, using Kw or pKw · be able to define the terms 'pKa' and 'pKw' · be able to analyse data from the following experiments: (i) measuring the pH of a variety of substances, including equimolar solutions of strong and weak acids, strong and weak bases, and salts; (ii) comparing the pH of a strong and weak acid after dilution 10, 100 and 1000 times · be able to calculate Ka for a weak acid from experimental data given the pH of a solution containing a known mass of acid

Titration Curves and IndicatorsSign up

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 · be able to select a suitable indicator for a titration, using a titration curve and appropriate data

Buffer SolutionsSign up

know what is meant by the term 'buffer solution' · understand the action of a buffer solution · be able to calculate the pH of a buffer solution given appropriate data · be able to calculate the concentrations of solutions required to prepare a buffer solution of a given pH · understand how to use a weak acid-strong base or strong acid-weak base titration curve to: (i) demonstrate buffer action; (ii) determine Ka from the pH at the point where half the acid is neutralised/equivalence point · understand the importance of buffer solutions in biological environments: (i) buffers in cells and in blood (H2CO3/HCO3-); (ii) in foods to prevent deterioration due to pH change (caused by bacterial or fungal activity) · CORE PRACTICAL 11: Finding the Ka value for a weak acid