1
Q
What are buffer solutions?
A
Solutions which resist changes in pH when small amounts of acid / base are added
In the solution there must be lareg amounts of the base and acid for the buffer to work effectively
2
Q
What are acidic buffers?
A
Weak acids
pH is lower than 7
3
Q
What are alkali buffers?
A
Solutions of weak bases and conjugate acids
pH is higher than 7
4
Q
What does the pH at which a buffer operates depend on?
A
The pka of the acidic component present
5
Q
How do you work out the pKa value?
A
pKa = -log 10 (Ka) Ka = 10 to the power of (-pKa)
AQA A Level Chemistry
flashcards
Decks in class (88)
# Cards
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General + Practical knowledge38
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3.1.1.1 Atomic Structure12
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3.1.1.2 Mass Number And Isotopes6
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3.1.1.3 Electron Configuration20
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3.1.2.1 Relative Atomic Mass And Relative Molecular Mass5
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3.1.2.2 The Mole And The Avogadro Constant4
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3.1.2.3 The Ideal Gas Equation5
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3.1.2.4 Empirical Formula And Molecular Formula4
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3.1.2.5 Balanced Equations And Associated Calculations21
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3.1.3.1 Ionic Bonding12
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3.1.3.2 Nature of Covalent and Dative Covalent Bonds17
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3.1.3.3 Metallic Bonding12
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3.1.3.4 Bonding and Physical Properties13
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3.1.3.5 Shapes of Simple Molecules and Ions7
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3.1.3.6 Bond Polarity10
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3.1.3.7 Forces Between Molecules6
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3.1.4.1 Enthalpy Change6
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3.1.4.2 Calorimetry3
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3.1.4.3 Applications Of Hess's Law8
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3.1.4.4 Bond Enthalpies2
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3.1.5.1 Collision Theory2
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3.1.5.2 Maxwell Boltzmann Distribution2
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3.1.5.3 Effect of Temperature on Reaction Rate3
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3.1.5.4 Effect of Concentration and Pressure2
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3.1.5.5 Catalysts4
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3.1.6.1 Chemical Equilibria and Le Chatelier's Principle10
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3.1.6.2 Equilibrium constant Kc for homogenous systems4
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3.1.7 Oxidation, reduction and redox equations21
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3.1.8.1 Born-Haber Cycles17
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3.1.8.2 Gibbs Free-energy Change, /\G, and Entropy Change, /\S18
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3.1.9.1 Rate Equations8
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3.1.9.2 Determining The Rate Equation5
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3.1.10 Equilibrium Constant Kp for Homogenous Systems8
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3.1.11.1 Electrode Potentials and Cells13
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3.1.11.2 Commercial Applications of Electrochemical Cells7
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3.1.12.1 Bransted-Lowry acid-base equilibria in aqueous solution15
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3.1.12.2 Definition and Determination of pH2
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3.1.12.3 The Ionic Product of Water, Kw2
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3.1.12.4 Weak Acids and Bases Ka for Weak Acids2
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3.1.12.5 pH Curves, Titrations and Indicators5
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3.1.12.6 Buffer Action5
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3.2.1.1 Classification1
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3.2.1.2 Physical properties of Period 3 elements7
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3.2.2 Group 2, the alkaline earth metals37
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3.2.3.1 Trends in properties20
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3.2.4 Properties of Period 3 elements and their oxides34
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3.2.5.1 General Properties of Transition Metals12
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3.2.5.2 Substitution Reactions15
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3.2.5.3 Shapes of Complex Ions11
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3.2.5.4 Formation of Coloured Ions12
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3.2.5.5 Variable Oxidation States5
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3.2.5.6 Catalysts12
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3.2.6 Reactions of Ions in Aqueous Solution24
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3.3.1.1 Nomenclature28
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3.3.1.2 Reaction mechanisms4
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3.3.1.3 Isomerism10
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3.3.2.1 Fractional distillation of crude oil plus general alkanes7
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3.3.2.2 Modification of alkanes by cracking6
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3.3.2.3 Combustion of alkanes11
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3.3.2.4 Chlorination of alkanes4
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3.3.3.1 Nucleophilic substitution12
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3.3.3.2 Elimination6
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3.3.3.3 Ozone depletion4
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3.3.4.1 Structure, bonding and reactivity5
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3.3.4.2 Addition reactions of alkenes10
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3.3.4.3 Addition polymers5
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3.3.5.1 Alcohol production16
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3.3.5.2 Oxidation of alcohols9
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3.3.5.3 Elimination4
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3.3.6.1 Identification of functional groups by test-tube reactions6
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3.3.6.2 Mass spectrometry8
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3.3.6.3 Infrared spectroscopy4
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3.3.7 Optical Isomerism16
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3.3.8 Aldehydes and Ketones21
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3.3.9.1 Carboxylic Acids and Esters11
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3.3.9.2 Acylation8
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3.3.10.1 Bonding11
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3.3.10.2 Electrophilic Substitution25
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3.3.11 Amines20
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3.3.12 Condensation Polymers12
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3.3.13.1 Amino Acids16
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3.3.13.2 Proteins21
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3.3.13.3 Enzymes6
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3.3.13.4 DNA3
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3.3.13.5 Action of Anticancer Drugs5
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3.3.14 Organic Synthesis22
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3.3.15 Nuclear Magnetic Resonance Spectroscopy30
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3.3.16 Chromatography12
