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36 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Acid |
A proton donor |
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Base |
A proton acceptor |
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Monobasic acid |
An acid which can donate 1 proton per molecule |
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Dibasic acid |
An acid which can donate 2 protons per molecule |
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Tribasic acid |
An acid which can donate 3 protons per molecule |
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Strong Acid |
An acid which completely dissociates |
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Weak acid |
An acid which partially dissociates |
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Acid + Carbonate = |
Salt + H2O + CO2 |
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Acid + Base = |
Salt + H2O |
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Acid + Metal = |
Salt + H2 |
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Conjugate Acid - Base pair |
Two species which can transform into eachother by the loss or gain of a proton |
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Convert from [H+] to pH |
-Log([H+]) |
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Convert from pH to [H+] |
10^-pH |
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What is Ka, and what species is it used for? |
The acid dissociation constant, used for weak acids |
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The equation for constant of weak acids |
Ka = ([H+] [A-] / [HA]) |
Use [HA] |
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What does a large Ka indicate? (2) |
A large extent of dissociation, a stronger weak acid |
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What does a small Ka indicate? (2) |
A small extent of dissociation, a weaker weak acid |
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What does a small Ka indicate? (2) |
A small extent of dissociation, a weaker weak acid |
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Convert from Ka to pKa |
-Log(Ka) |
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Convert from pKa to Ka |
10^-pKa |
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What does a small pKa indicate? |
A stronger weak acid |
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What does a large pKa indicate? |
A weaker weak acid |
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What is Kw? |
Ionic product of water |
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What value is Kw at 25°C? |
1x10^-14 |
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Expression for dissociation of a strong base? |
Kw = [H+] [OH-] |
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Buffer definition, and consists of? (2) |
A solution which resists changes in pH, consisting of a weak acid and it's conjugate base |
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State marks for: How a solution of glycolic acid and glycolate ions can act as a buffer |
1) Equilibrium 2) Glycolic acid reacts with added alkali 3) Equilibrium shifts right 4) Glycolate ions react with added acid 5) Equilibrium shifts left |
(5) |
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State marks for: How a solution of glycolic acid and glycolate ions can act as a buffer |
1) Equilibrium 2) Glycolic acid reacts with added alkali 3) Equilibrium shifts right 4) Glycolate ions react with added acid 5) Equilibrium shifts left |
(5) |
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Define pH |
-Log([H+(aq)]) |
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Equation constants for buffers |
Ka = ([H+] [A-])/[HA] |
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What kind of bonding molecules will make ions in an ionic equation? |
Acidic ionic and Aqueous ionic |
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What type of bonding molecules will not form ions in an ionic equation? |
Solid ionic and covalent |
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Ionic equation of: Mg(NO3)2(aq) + Na2CO3(aq) > 2NaNO3(aq) + MgCO3(s) |
Mg^2+ + CO3^2- > MgCO3 |
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Cation |
An ion with net positive charge |
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Anion |
An ion with net negative charge |
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NH3, is an acid, base...? |
Weak base |
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