The change in concentration of a reactant or product in a given time
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Initial Rate of Reaction
Is the change in concentration of a reactant or product per unit time at the start of the reaction when time = 0
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Order of Reaction
The power to which its concentration is raised in the rate equation
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Overall Order
Is the sum of all the individual orders
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Rate Constant, k
Is the constant that links the rate of reaction with the concentrations of the reactants raised to the powers of their orders in the rate equation
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Half-Life
The time taken for the concentration of the reactant to reduce by half
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Reaction Mechanism
Is a series of steps that together make up the overall reaction
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Rate-Deterimining Step
Is the slowest step in the reaction mechanism of a multistep reaction
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Intermediate
Is a species formed in one step of a multistep reaction that is used up in a subsequent step and is not seen as either a reactant or a product of the overall equation
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Equilibrium Law
aA+bB⇌cC+dD Kc=[C]c[D]d / [A]a[B]b
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Dynamic Equilibrium
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
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Homogeneous Equilibrium
Is an equilibrium in which all the species making up the reactants and products are in the same physical state
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Heterogeneous Equilibrium
Is an equilibrium in which species making up the reactants and products are in different physical states
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Bronsted-Lowry Acid
Proton donor
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Bronsted-Lowry Base
Proton acceptor
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Neutralisation
A chemical reaction that occurs when an acid is added to a base and a salt and water are formed
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Acid Base Pair
Is a pair of two species that transform into each other by gain or loss of a proton
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How to Calculate pH
-log10[H+(aq)]
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[H+(aq)]
10^-pH
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Strong Acid
An acid that completely dissociates/ionises in aqueous solution
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Weak Acid
An acid that partially dissociates/ionises in aqueous solution
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Acid Dissociation Constant
Ka = [H+(aq)][A-(aq)] / [HA(aq)]
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How to Calculate pKa
-log10Ka
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How to Calculate Ka
10^-pKa
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Strong Acid Calculation
[H+(aq)] = [HA(aq)]
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Weak Acid Calculation
Ka = [H+(aq)][A-(aq)] / [HA(aq)] or [H+(aq)]^2 / [HA(aq)]
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Ionic Product of Water (Kw)
[H+(aq)][OH-(aq)] At 25 degrees,1x10^-14 mol^2 dm^-6
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Strong Alkali
[OH-(aq)] = [NaOH(aq)]
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Strong Alkali Calculation
[H+(aq)] = Kw/[OH-(aq)]
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Buffer
Is a mixture that minimises pH changes on addition of small amounts of acid or base
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Equivalence
Is the point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution
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End Point
Is the point in the titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator
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Standard Enthalpy Change of Neutralisation
Is the energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of water under standard conditions
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Other cards in this set
Card 2
Front
Is the change in concentration of a reactant or product per unit time at the start of the reaction when time = 0
Back
Initial Rate of Reaction
Card 3
Front
The power to which its concentration is raised in the rate equation
Back
Card 4
Front
Is the sum of all the individual orders
Back
Card 5
Front
Is the constant that links the rate of reaction with the concentrations of the reactants raised to the powers of their orders in the rate equation
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