IB Chemistry - Acids and bases (8)
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Last updated 1:35 PM on 12/15/22
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48 Terms
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Brønsted-Lowry acid
proton donor
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Brønsted-Lowry base
proton acceptor
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Lewis acid
electron pair acceptor
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Lewis base
electron pair donor
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Conjugate acid-base pair
consists of two substances related to each other by the donating and accepting of a single hydrogen ion
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Amphiprotic
A species that can either accept or donate a proton.
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Amphoteric
A species that can react as either an acid or a base
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Acid + Metal
salt + hydrogen gas
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Acid + carbonates/hydrogencarbonates
salt + carbon dioxide + water
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Acid + base/alkali
salt + water
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Alkali
A base that dissolves in water or when a certain base reacts with water
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Neutralization
Acid + base
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Neutralization reaction: endothermic or exothermic?
Exothermic
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Dissociation of strong acids and bases in aqueous solution
dissociate/ionise completely
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Dissociation of weak acids and bases in aqueous solution
dissociate/ionise partly
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Monoprotic acid
an acid that can donate one proton per molecule
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Diprotic acid
an acid that can donate two protons per molecule
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The stronger an acid
the weaker its conjugate base
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The stronger the base
the weaker its conjugate acid
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Conductivity of strong acids and bases
good conductors
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Conductivity of weak acids and bases
bad conductors
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Strong acids react \___ with metals and carbonates
violently
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The equation for pH
pH = -log10 [H+]
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The equation for [H+]
\[H+] = 10^-pH
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Kw = 1.0*10^-14 =
\[H+][OH-]
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Ka (anti dissociation constant)
Ka = Kc*[H2O] (products over reactants - H2O)
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pKa
-logKa
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Ka
10^-pKa
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pKa + pKb =
pKw = 14 at 25C
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Strong acid + weak base
acidic salt
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Strong base + weak acid
basic salt
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Strong base + strong acid
neutral salt
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Weak acid + weak base
depends on relative strengths (compare pKa and pKb - the smaller the stronger)
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High charge density
high tendency to polarise water molecules
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Larger ion
the lower its charge
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Weak acid-weak base titration
pH at equivalence point = depending on the relative strengths of the substances. (compare Ka and Kb - the bigger the stronger)
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Strong acid-strong base titration
pH at equivalence point = 7
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Strong acid-weak base titration
pH at equivalence point =
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Strong base-weak acid titration
pH at equivalence point = \>7
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Half equivalence point
pH = pKa
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pKw
pH + pOH
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pH range of an indicator
the pH range over which intermediate colours for an indicator can be seen
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pKa of indicator =
pH at midpoint of pH range
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Equation for an acidic indicator:
HIn ⇌ H+ + In-
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Equation for a basic indicator:
In- + H2O ⇌ HIn + OH-
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Rough pH range of an indicator
pKa +/- 1
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Definition of a buffer solution
a solution that resists changes when small amounts of acid or alkali is added
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No. of moles =
concentration * volume (in dm3)
