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Lecture

CHEM 1114 Lecture Notes - Amphoterism, Sodium Chloride, Nonmetal

by

Department
Chemistry
Course Code
CHEM 1114
Professor
K.Sveinson

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Hydrolysis of Salts
Hydrolysis: splitting apart means of water
-salts form when a positive metal ion from the base combines with a negative non-metal ion from the
acid
(NaCl is formed between NaOH and HCl)
-salt solutions can be acidic, basic or neutral
(ions from the salt may react with water to produce H3O , OH- or neither)
Cations that do hydrolyze
Anions that do not hydrolyze
NH4
+
*Fe3+
*Al3+
*Cr3+
gives off acidic solution
CIO 4
-
I-
Br-
Cl-
NO3
-
SO4
2-
(has no effect on the nature of solutions)
The conjugates of all strong acids
* = ions that exist as hexahydrates in solutions
Fe3+ = Fe(H2O)6 3+ ; Al3+ = Al(H2O)6 3+
Predicting the Nature of a Solution
-No hydrolysis and salt solution is neutral (pH=7)
Ex. Na +H2O no reaction <the solution is neutral since no H3O+ or OH- is produced
Salts of strong bases and weak acids
-hydrolysis of the anion, producing OH- aka anionic hydrolysis
-salt solution is basic (pH > 7)
Ex. NH4Cl
NH4 +H2O  NH3 + H3O
Cl- + H2O no reaction
The solution is ACIDIC , H3O is produced
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