381946
Descripción
Mapa Mental por noahsark275, actualizado hace más de 1 año
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Creado por noahsark275
hace más de 10 años
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acid/base equilibria
- a substance with a sour taste to a
substance which produces an
excess of hydrogen ions in solution
(Arrhenius theory) to the
Brønsted-Lowry theory
- understanding of the Brønsted–Lowry theory of
acid-base behaviour, and use it to identify
conjugate acid-base pairs
- a Brønsted–Lowry acid is a proton
donor and a base a proton acceptor
- acid-base equilibria
involve transfer of protons
- acid-base equilibria
involve transfer of protons
- a Brønsted–Lowry acid is a proton
donor and a base a proton acceptor
- terms:pH,
Ka and
Kw , pKa
and pKw
- weak acids and bases
are only slightly
dissociated in aqueous
solution
- apply the equilibrium law to
deduce the expressions for the
equilibrium constants Ka and Kw
- apply the equilibrium law to
deduce the expressions for the
equilibrium constants Ka and Kw
- experiments: measuring the pH of a variety
of substances, eg equimolar solutions of
strong and weak acids, strong and weak
bases and salts. Comparing the pH of a
strong acid and a weak acid after dilution
10, 100 and 1000 times
- determine Ka for a
weak acid by
measuring the pH of
a solution
- discuss the
assumptions made
in this calculation
- discuss the
assumptions made
in this calculation
- determine Ka for a
weak acid by
measuring the pH of
a solution
- calculate the pH of a solution of a
weak acid based on data for
concentration and Ka
- discuss the
assumptions made
in this calculation
- discuss the
assumptions made
in this calculation
- measure the pH change during titrations and draw titration
curves using different combinations of strong and weak
monobasic acids and bases
- use data about indicators, together with
titration curves, to select a suitable indicator
and the use of titrations in analysis
- explain the action of buffer solutions and carry out calculations
on the pH of buffer solutions, eg making buffer solutions and
comparing the effect of adding acid or alkali on the pH of the
buffer
- use titration curves to show the buffer action
and to determine Ka from the pH at the point
where half the acid is neutralised
- explain the importance of buffer
solutions in biological environments,
eg buffers in cells and in blood (H2
CO3 /HCO3 - ) and in foods to prevent
deterioration due to pH change
(caused by bacterial or fungal activity)
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