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18 Cards in this Set
- Front
- Back
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ΔG°=?
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-RTlnK(eq)
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a <-> b
Keq = ? |
[b]/[a]
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At 25°C, ΔG° = ?
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-1.4 logKeq (kcal/mol)
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HA + H2O <-> A- + H3O+
Which is the acid? |
HA, A- is CB
H2O is the base, H3O+ is CA |
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HA + H2O <-> A- + H3O+
Ka = ? |
[A-][H3O+]/[HA]
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pKa = ?
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-logKa
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A smaller pKa indicates what about the compound?
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Stronger acid, better ability to protonate something
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A larger pKa indicates what about the compound?
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Weaker acid, stronger conjugate base
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What kind of relationship do conjugate base and acid have?
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Inverse relationship
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Conjugate base of CH4?
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-CH3
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Conjugate base of HF
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F-
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Order the acids by strength:
CH4, NH3, H2O, HF Explain the trend |
HF 3.18 > H2O 15.74 > NH3 38 > CH4 48
The increase in electronegative across a row means the CB will be able to stabilize itself (weaker), so the acid will be strong |
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Order the acids by strength:
H2O, H2S Explain the trend |
H2S 7.00 > H2O 15.74
The larger the molecule, the more stable the CB (weaker base), stronger acid |
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Order the acids by strength:
HF, HCl Explain the trend |
HCl -7 > HF 15.74
The larger the molecule, the more stable the CB (weaker base), stronger acid |
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Order the acids by strength:
H3C-CH3, H2C=CH2, HCCH Explain the trend |
HCCH 25, H2C=CH2 44, H3C-CH3 50
sp > sp2 > sp3 Less p character, more s character = electrons closer to nucleus = more stable CB |
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H2O + HA (pKa = x) <-> H3O+ (pKa = -1.74) + A-
logKeq = ? ΔG° = ? |
-1.74 - x
pKa acid on right - pKa acid on left ΔG° = -1.4 * (-1.74-x) |
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A- + H2O (pKa = 15.74) <-> HA (pKa = y) + OH-
logKeq=? ΔG° = ? |
y - 15.74
ΔG° = -1.4 * (y-15.74) |
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R-CC-H pKa = 25
Which base will you use to deprotonate it? |
A base where the CA has a pKa > 25
pKa of CA - 25 > 0 ΔG° = -1.4* (+ve) = -ve = favourable, proceed towards the right |
