The Hydrolysis Reactions - Write net-ionic equations for the reaction of each salt with water below. If there is no reaction, write N.R.
1. NH4C2H3O2
2. NH4Cl
3. NaCl
4. Na2CO3
5. NaC2H3O2
6. NaHSO4
7. FeCl3
8. NaH2PO4
9. NaHCO3
To determine the net-ionic equations for the hydrolysis reactions, we need to identify the ions present in each salt and determine how they react with water.
1. NH4C2H3O2:
NH4C2H3O2 → NH4+ + C2H3O2-
Both ions, NH4+ and C2H3O2-, are spectator ions and do not react with water. Therefore, there is no hydrolysis reaction. N.R.
2. NH4Cl:
NH4Cl → NH4+ + Cl-
The NH4+ ion reacts with water to form NH3 and H3O+.
NH4+ + H2O → NH3 + H3O+
The Cl- ion does not react with water. Therefore, the net-ionic equation is:
NH4+ + H2O → NH3 + H3O+ + Cl-
3. NaCl:
NaCl → Na+ + Cl-
Both Na+ and Cl- ions do not react with water. Therefore, there is no hydrolysis reaction. N.R.
4. Na2CO3:
Na2CO3 → 2Na+ + CO3^2-
Both Na+ and CO3^2- ions do not react with water. Therefore, there is no hydrolysis reaction. N.R.
5. NaC2H3O2:
NaC2H3O2 → Na+ + C2H3O2-
The C2H3O2- ion reacts with water to form acetic acid (CH3COOH) and hydroxide ions (OH-).
C2H3O2- + H2O → CH3COOH + OH-
The Na+ ion does not react with water. Therefore, the net-ionic equation is:
C2H3O2- + H2O → CH3COOH + OH- + Na+
6. NaHSO4:
NaHSO4 → Na+ + HSO4-
The HSO4- ion reacts with water to form hydronium ions (H3O+) and sulfate ions (SO4^2-).
HSO4- + H2O → H3O+ + SO4^2-
The Na+ ion does not react with water. Therefore, the net-ionic equation is:
HSO4- + H2O → H3O+ + SO4^2- + Na+
7. FeCl3:
FeCl3 → Fe^3+ + 3Cl-
Both Fe^3+ and Cl- ions do not react with water. Therefore, there is no hydrolysis reaction. N.R.
8. NaH2PO4:
NaH2PO4 → Na+ + H2PO4-
The H2PO4- ion reacts with water to form dihydrogen phosphate (H2PO4-) and hydronium ions (H3O+).
H2PO4- + H2O ↔ HPO4^2- + H3O+
The Na+ ion does not react with water. Therefore, the net-ionic equation is:
H2PO4- + H2O ↔ HPO4^2- + H3O+ + Na+
9. NaHCO3:
NaHCO3 → Na+ + HCO3-
The HCO3- ion reacts with water to form carbonic acid (H2CO3) and hydroxide ions (OH-).
HCO3- + H2O ↔ H2CO3 + OH-
The Na+ ion does not react with water. Therefore, the net-ionic equation is:
HCO3- + H2O ↔ H2CO3 + OH- + Na+
Note: The double arrow (↔) represents a reversible reaction, indicating that the reaction can proceed in both forward and backward directions.
1. NH4C2H3O2: Well, this one is a bit of a "smelly" situation! When NH4C2H3O2 dissolves in water, it breaks down into NH4+ and C2H3O2-. So the net-ionic equation is NH4+(aq) + C2H3O2-(aq) -> N.R. (no reaction).
2. NH4Cl: Ah, the classic NH4Cl! When NH4Cl dissolves in water, it dissociates into NH4+ and Cl-. So the net-ionic equation is NH4+(aq) + Cl-(aq) -> N.R. (no reaction).
3. NaCl: Ah, the good old table salt! When NaCl dissolves in water, it dissociates into Na+ and Cl-. So the net-ionic equation is Na+(aq) + Cl-(aq) -> N.R. (no reaction).
4. Na2CO3: Time to carbonate! When Na2CO3 dissolves in water, it dissociates into 2 Na+ and CO3(2-). So the net-ionic equation is 2 Na+(aq) + CO3(2-)(aq) -> N.R. (no reaction).
5. NaC2H3O2: Ah, the salty vinegar! When NaC2H3O2 dissolves in water, it dissociates into Na+ and C2H3O2-. So the net-ionic equation is Na+(aq) + C2H3O2-(aq) -> N.R. (no reaction).
6. NaHSO4: Sulfuric acid alert! When NaHSO4 dissolves in water, it dissociates into Na+ and HSO4-. So the net-ionic equation is Na+(aq) + HSO4-(aq) -> N.R. (no reaction).
7. FeCl3: Iron chloride, coming through! When FeCl3 dissolves in water, it dissociates into Fe(3+) and 3 Cl-. So the net-ionic equation is Fe(3+)(aq) + 3 Cl-(aq) -> N.R. (no reaction).
8. NaH2PO4: Phosphoric acid time! When NaH2PO4 dissolves in water, it dissociates into Na+ and H2PO4-. So the net-ionic equation is Na+(aq) + H2PO4-(aq) -> N.R. (no reaction).
9. NaHCO3: Time to fizz it up! When NaHCO3 dissolves in water, it dissociates into Na+ and HCO3-. So the net-ionic equation is Na+(aq) + HCO3-(aq) -> N.R. (no reaction).
Well, there you have it! Hydrolysis reactions can be quite a "dissociative" affair!
1. NH4C2H3O2:
NH4C2H3O2 + H2O -> NH4OH + C2H3O2-
Net ionic equation: NH4+ + H2O -> NH4OH + H+
2. NH4Cl:
NH4Cl + H2O -> NH4+ + Cl-
Net ionic equation: No reaction (N.R.)
3. NaCl:
NaCl + H2O -> Na+ + Cl-
Net ionic equation: No reaction (N.R.)
4. Na2CO3:
Na2CO3 + H2O -> 2Na+ + CO3^2-
Net ionic equation: CO3^2- + H2O -> HCO3- + OH-
5. NaC2H3O2:
NaC2H3O2 + H2O -> Na+ + C2H3O2-
Net ionic equation: No reaction (N.R.)
6. NaHSO4:
NaHSO4 + H2O -> Na+ + HSO4-
Net ionic equation: HSO4- + H2O -> H3O+ + SO4^2-
7. FeCl3:
FeCl3 + H2O -> Fe(OH)3 + 3Cl-
Net ionic equation: Fe^3+ + 3H2O -> Fe(OH)3 + 3H+
8. NaH2PO4:
NaH2PO4 + H2O -> Na+ + H2PO4-
Net ionic equation: H2PO4- + H2O -> H3O+ + HPO4^2-
9. NaHCO3:
NaHCO3 + H2O -> Na+ + HCO3-
Net ionic equation: HCO3- + H2O -> H2CO3 + OH-
You need to learn to do these. The easy way, in the beginning, is to write the hydrolysis as if the salt (all of them) reacted completely with water, then apply rules to know what happens. For example, for NaC2H3O2,
NaC2H3O2 + HOH ==> NaOH + HC2H3O2. That is step 1.
Step 2. Look at the products. If the product is a weak acid or weak base, that cation/anion hydrolyzes. If not , it does not. Thus NaOH is a strong base; therefore Na^+ does NOT hydrolyze. HC2H3O2 is a weak acid; therefore, C2H3O2^- does. The net ionic equation for the hydrolysis of NaC2H3O2 is the following:
C2H3O2^- + HOH ==> HC2H3O2 + OH^-
The others follow the same set of rules. For the NH4^+, it is much easier to write BOTH as half reactions. For example, for NH4C2H3O2
NH4^+ + H2O ==> NH3 + H3O^+
NH3 is a weak base, therefore, the NH4^+ hydrolyzes.
You already know, from the first example I did, that C2H3O2^- hydrolyzes; therefore, BOTH NH4^+ and C2H3O2^- hydrolyze.