Term
| Effect of increased pressure on equilibrium (gas system) |
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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. |
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| Effect of increased temperature on equilibrium |
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Definition
| Equilibrium favours the endothermic reaction |
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Term
| In equilibrium reactions, enthalpy change refers to... |
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Definition
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Term
| Addition of unreactive gases/catalyst does what to position of equilibrium? |
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Definition
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| If equilibrium constant is large, what does that say about position of equilibrium? |
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Definition
| It means there is a large concentration of products compared to reactants so equilibrium favours the forward direction |
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Term
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Definition
products (to the power of n)
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reactants (to the power of n) |
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Term
| Increase concentration of products does what to equilibrium? |
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Definition
| Favours reverse direction |
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Term
| Increase concentration of reactants does what to equilibrium? |
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Definition
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Term
An acid is.....
A base is...... |
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Definition
Acid: PROTON DONOR
Base: PROTON ACCEPTER |
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Term
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Definition
| A reaction where a proton is donated and accepted |
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Term
| Strong acids dissociate partially/fully? |
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Definition
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Term
| Weak acids dissociate partially/fully? |
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Definition
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Term
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Definition
| Soluble bases that form OH- ions in solution |
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Definition
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Definition
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Term
| Acids and bases can/cannot conduct electricity? |
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Definition
| CAN - they contain ions that are free to move |
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Term
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Definition
| metal compound + hydrogen gas |
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Term
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Definition
| metal compound + water + carbon dioxide gas |
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Definition
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Term
| Hydrogen ions attach to water molecules to form |
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Definition
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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 |
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Term
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Definition
| - Has a greater tendency to accept protons than weak bases |
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Term
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Definition
| high concentration of H3O+ ions |
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Term
| calculating pH of strong base |
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Definition
pH = -log [H3O+ concentration]
only a strong base because it fully dissociates |
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Term
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Definition
| [concentration of H3O+ ions] x [concentrations OH- ions] = 1 x10-14 |
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