The net ionic hydrolysis equation for aqueous ammonium ethanoate is NH4CH3COO(aq)⇄NH4+(aq)+CH3COO-(aq) NH4OH(aq)+CH3COOH(aq)⇄NH4CH3COO(aq)+H2O(l) H2O(l)⇄H+(aq)+OH-(aq) NH4CH3COO(aq)+H2O(l)⇄NH4OH(aq)+CH3COOH(aq)
The net ionic hydrolysis equation for aqueous ammonium ethanoate is
| NH4CH3COO(aq)⇄NH4+(aq)+CH3COO-(aq) | |
| NH4OH(aq)+CH3COOH(aq)⇄NH4CH3COO(aq)+H2O(l) | |
| H2O(l)⇄H+(aq)+OH-(aq) | |
| NH4CH3COO(aq)+H2O(l)⇄NH4OH(aq)+CH3COOH(aq) |
Homework Answers
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The net ionic hydrolysis equation for aqueous ammonium ethanoate
is
NH4CH3COO(aq)⇄NH4+(aq)+CH3COO-(aq)
NH4OH(aq)+CH3COOH(aq)⇄NH4CH3COO(aq)+H2O(l)
H2O(l)⇄H+(aq)+OH-(aq)
NH4CH3COO(aq)+H2O(l)⇄NH4OH(aq)+CH3COOH(aq)
1 Part A: The net ionic hydrolysis equation for aqueous ammonium chloride is: a.H2O(l)⇄H+(aq)+OH-(aq) b.NH4+(aq)+H2O(l)⇄NH4OH(aq)+H+(aq) c....
1 Part A: The net ionic hydrolysis equation for aqueous ammonium chloride is: a.H2O(l)⇄H+(aq)+OH-(aq) b.NH4+(aq)+H2O(l)⇄NH4OH(aq)+H+(aq) c. NH4OH(aq)+HCl(aq)⇄NH4Cl(aq)+H2O(l) d. NH4Cl(aq)⇄NH4+(aq)+Cl-(aq) Part B: Adding acid to the buffer, NH3-NH4+, will produce this (net ionic) reaction: a. H+(aq)+OH-(aq)⇄H2O(l) b. H+(aq)+NH4+(aq)⇄NH3(aq)+H2(g) c. H+(aq)+NH4+(aq)⇄NH52+(aq) d. H+(aq)+NH3(aq)⇄NH4+(aq)
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Which net ionic equation best represents the reaction that occurs when an aqueous solution of lithium nitrate is mixed with an aqueous solution of ammonium chloride? 0 Lit(aq) + C1-(aq) →→LiCl(s) O NH4Cl(aq) + LINO3(aq) -LiCl(s) + NH4NO3(aq) O NH4+(aq) + NO3- (aq) → NH4NO3(aq) O No net reaction occurs. O Lit(aq) + NH4Cl(aq) —-LiCl(s) + NH4+ (aq) The following reaction occurs in basic solution: _H2O(aq) + _ MnO4 (aq) +_ CIO (aq) → _MnO2(s) + _C104 (aq) +_ OH(aq)...
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