Question : Write the equilibrium equations showing any hydrolysis (if any) that is happening in the solution for each of the solutions,. Discussion:Correlate the observed pH with the hydrolysis equilibria.
Procedure:Part 1. Using a pH meter, measure the pH of the following 5 salt solutions (use the solutions that are labeled "Experiment 3"): 1 M NaC2H3O2 , 1 M NaCl, 1 M NH4Cl, 1 M NH4C2H3O2, 1 M Na2CO3 .Part 2. Go to the reagent shelves and find the containers of solid ammonium chloride, ammonium acetate, and ammonium carbonate. Open the containers and cautiously smell. Rank the three solids in terms of the strength of the ammonia odor. Part 3. Using a pH meter, measure the pH of 0.1 M NaH2PO4 (sodium dihydrogen phosphate) and 0.1 M Na2HPO4 (sodium monohydrogen phosphate).Part 4. Weigh out about 2 grams of solid aluminum sulfate (since this is an approximate mass, use the centigram balance, do not use the analytical balance) in a 50 mL beaker. Add about 10 mL of water and mix thoroughly with a stirring rod. Measure the pH of the solution.Into another 50 mL beaker, weigh out about 2 grams of solid sodium bicarbonate. Add about 10 mL of water and mix thoroughly. Measure the pH of the solution.Now mix these two solutions together in a larger beaker. Note any observations.
Data:
Part 1
1M of:
NaCH3CO2 ph=8.79
NaCl ph = 6.89
NH4Cl ph=5.06
NH4CH3CO2 ph = 6.90
Na2CO3 ph=11.82
Part 2
NH4Cl(s) - smell weak
NH4CH3CO2 (s)- smell medium
(NH4)2CO3(s)- smell strong
Part 3
0.1 M NaH2PO4 ph=8.56
0.1 M Na2HPO4 ph=4.65
Part 4
2g of Al2(SO4) (s) + 10 ml H2O (50 ml beaker)
ph = 7.96
2g NaHCO3(s) + 10 ml H2O (50 ml beaker)
ph = 3.07
This is only one question to write equilibrium equations showing any hydrolisys.
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