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L2 Chemical Reactivity
Equilibrium, rate of reaction, acids and bases
26
Chemistry
Not Applicable
09/22/2012

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Term
Effect of increased pressure on equilibrium (gas system)
Definition
Pressure increase is counteracted by decreasing number of gas particles in equilibrium. Thus, equilibrium shifts to the side with smallest number of moles of gas.
Term
Effect of increased temperature on equilibrium
Definition
Equilibrium favours the endothermic reaction
Term
In equilibrium reactions, enthalpy change refers to...
Definition
Forward reaction
Term
Addition of unreactive gases/catalyst does what to position of equilibrium?
Definition
Has no effect
Term
If equilibrium constant is large, what does that say about position of equilibrium?
Definition
It means there is a large concentration of products compared to reactants so equilibrium favours the forward direction
Term
Equilibrium constant
Definition
products (to the power of n)
-----------------------------
reactants (to the power of n)
Term
Increase concentration of products does what to equilibrium?
Definition
Favours reverse direction
Term
Increase concentration of reactants does what to equilibrium?
Definition
Favours forward reaction
Term
An acid is.....
A base is......
Definition
Acid: PROTON DONOR
Base: PROTON ACCEPTER
Term
Acid-base reaction
Definition
A reaction where a proton is donated and accepted
Term
Strong acids dissociate partially/fully?
Definition
FULLY
Term
Weak acids dissociate partially/fully?
Definition
PARTIALLY
Term
What are alkalis?
Definition
Soluble bases that form OH- ions in solution
Term
Acid + Metal oxide =
Definition
metal compound + water
Term
Acid + Metal hydroxide =
Definition
metal compound + water
Term
Acids and bases can/cannot conduct electricity?
Definition
CAN - they contain ions that are free to move
Term
Acid + metal =
Definition
metal compound + hydrogen gas
Term
Acid + carbonate =
Definition
metal compound + water + carbon dioxide gas
Term
Bases turn litmus..
Definition
BLUE
Term
Acids turn litmus...
Definition
RED
Term
Hydrogen ions attach to water molecules to form
Definition
H3O+ ions
Term
Strong acid:
Definition
- conduct better b/c more ions in a given volume
- lower pH b/c greater concentration of H3O+ ions
- react faster and more vigorously than weak acids
Term
Strong base:
Definition
- Has a greater tendency to accept protons than weak bases
Term
Low pH =
Definition
high concentration of H3O+ ions
Term
calculating pH of strong base
Definition
pH = -log [H3O+ concentration]
only a strong base because it fully dissociates
Term
Kw
Definition
[concentration of H3O+ ions] x [concentrations OH- ions] = 1 x10-14
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