Part A Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base? Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base?
HCl(aq) + NH3(aq) ↔ NH4Cl(aq)
H3O+(aq) + NH3(aq) ↔ NH4+(aq) + H2O(l)
HCl(aq) + NaOH(aq) ↔ H2O(l) + NaCl(aq)
H3O+(aq) + OH-(aq) ↔ 2 H2O(l)
HCl(aq) + NH3(aq) ↔ NH4Cl(aq)
This is not the net ionic equation because in net ionic equation
NH4Cl(aq) should be present as NH4+(aq) and Cl-(aq)
H3O+(aq) + NH3(aq) ↔ NH4+(aq) + H2O(l)
This is a net ionic equation for the neutralization reaction of a strong acid with a weak base
H3O+ is an strong acid and NH3 is weak base
HCl(aq) + NaOH(aq) ↔ H2O(l) + NaCl(aq)
This is a reaction between strong acid and strong base
H3O+(aq) + OH-(aq) ↔ 2 H2O(l)
This is a net reaction between strong acid and strong base
Answer:
H3O+(aq) + NH3(aq) ↔ NH4+(aq) + H2O(l)
Part A Which is a net ionic equation for the neutralization reaction of a strong acid...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
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