You are watching: Net ionic equation for nh3 and hcl
Wow I simply realized ns forgot every my g chem....unless i"m confuse what a "net ionic equation" is, It"s got to be: --> NH4(+) + CL(-) Ammonia is the base, HCL is the acid. NH3 accepts one H native HCL. It becomes positive, the Cl is negative
This is sort of a wierd one. I will certainly assume the this is in aqueuous solution: complete Equation(s): (1) NH3 + H2O + HCl -> NH4+ + OH- + H+ + Cl- (2) NH4+ + OH- + H+ + Cl- -> NH4+ + H2O + Cl- "Add" Together and cancel terms on both sides: NH3 + HCl -> NH4+ + Cl- The answer depends upon the wording the the question. If both of these are assumed to be in aqueous systems at the beginning, equation (2) is the full ionic equation, for this reason the network ionic equation would just be: H+ + OH- -> H2O If the NH3 is a gas, the net ionic is simply H+(aq) + NH3(g) -> NH4+(aq)
NH3 + H+ ---> Cl- is a spectator ion in aqueous solution. Remember, however, the NH3 is the conjugate base of a weak acid, so the is an equilibrium relationship. if you space asked "what is the net ionic equation the the protonation the NH3 by Hcl" then you deserve to write it together a one-way reaction.
NH3 + H+ ---> Cl- is a spectator ion in aqueous solution. Remember, however, the NH3 is the conjugate basic of a weak acid, so it is an equilibrium relationship. if you room asked "what is the network ionic equation the the protonation that NH3 by Hcl" climate you have the right to write it together a one-way reaction.
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