In: Chemistry
An aqueous solution contains 0.459 M hydrocyanic acid. How many mL of 0.244 M potassium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 9.300? mL note in case u need this
Acid/Base Ionization Constants at 25 oC |
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Acid |
Formula |
Ka1 |
Ka2 |
Ka3 |
Acid/Base Ionization Constants at 25 oC |
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Acid |
Formula |
Ka1 |
Ka2 |
Ka3 |
Acetic acid |
CH3COOH |
1.8×10-5 |
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Acetylsalicylic acid (aspirin) |
HC9H7O4 |
3.0×10-4 |
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Aluminum ion |
Al(H2O)43+ |
1.2×10-5 |
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Arsenic acid |
H3AsO4 |
2.5×10-4 |
5.6×10-8 |
3.0×10-13 |
Ascorbic acid |
H2C6H6O6 |
7.9×10-5 |
1.6×10-12 |
|
Benzoic acid |
C6H5COOH |
6.3×10-5 |
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Carbonic acid |
H2CO3 |
4.2×10-7 |
4.8×10-11 |
|
Ferric ion |
Fe(H2O)63+ |
4.0×10-3 |
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Formic acid |
HCOOH |
1.8×10-4 |
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Hydrocyanic acid |
HCN |
4.0×10-10 |
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Hydrofluoric acid |
HF |
7.2×10-4 |
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Hydrogen peroxide |
H2O2 |
2.4×10-12 |
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Hydrosulfuric acid |
H2S |
1.0×10-7 |
1.0×10-19 |
|
Hypochlorous acid |
HClO |
3.5×10-8 |
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Nitrous acid |
HNO2 |
4.5×10-4 |
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Oxalic acid |
H2C2O4 |
5.9×10-2 |
6.4×10-5 |
|
Phenol |
C6H5OH |
1.0×10-10 |
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Phosphoric acid |
H3PO4 |
7.5×10-3 |
6.2×10-8 |
3.6×10-13 |
Sulfuric acid |
H2SO4 |
very large |
1.2×10-2 |
|
Sulfurous acid |
H2SO3 |
1.7×10-2 |
6.4×10-8 |
|
Zinc ion |
Zn(H2O)42+ |
2.5×10-10 |
Base |
Formula |
Kb |
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---|---|---|---|---|
Ammonia |
NH3 |
1.8×10-5 |
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Aniline |
C6H5NH2 |
7.4×10-10 |
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Caffeine |
C8H10N4O2 |
4.1×10-4 |
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Codeine |
C18H21O3N |
8.9×10-7 |
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Diethylamine |
(C2H5)2NH |
6.9×10-4 |
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Dimethylamine |
(CH3)2NH |
5.9×10-4 |
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Ethylamine |
C2H5NH2 |
4.3×10-4 |
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Hydroxylamine |
NH2OH |
9.1×10-9 |
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Isoquinoline |
C9H7N |
2.5×10-9 |
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Methylamine |
CH3NH2 |
4.2×10-4 |
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Morphine |
C17H19O3N |
7.4×10-7 |
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Piperidine |
C5H11N |
1.3×10-3 |
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Pyridine |
C5H5N |
1.5×10-9 |
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Quinoline |
C9H7N |
6.3×10-10 |
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Triethanolamine |
C6H15O3N |
5.8×10-7 |
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Triethylamine |
(C2H5)3N |
5.2×10-4 |
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Trimethylamine |
(CH3)3N |
6.3×10-5 |
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Urea |
N2H4CO |
1.5×10-14 |
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