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Primarygun

A correct chemical equation

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Ammonia dissolves in water and react with water to form ammonium ions and hydroxide ions.

NH3(aq)+ H2O(l)+ HCl(aq)----> H2O(l)+ NH4Cl(aq)

Or NH4OH(aq)+HCl(aq)---->NH4Cl(aq)+H2O(l)

 

Moreover, can anyone write down the ionic equation of hydrogen chloride gas dissolve in sodium hydroxide?

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I think this is what you are looking for...

The net ionic equation is

NH4+ + OH- + H+ + Cl- = NH4Cl + H2O

 

The half equations are

NH4OH = NH4+ + OH-

HCl = H+ + Cl-

 

~Scott

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NoNo. I know of the concept.

I want to check how do we present it.

hydrogen chloride gas is one of the reactants. However, before the chemical equation, itself ionizes first. In this equation, it is (g) not named (aq).

Therefore, I think the correct equation may differ from that one.

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Sorry i didn't read your post closely enough. I'm not quite sure... but if it ionizes before the equation it shouldm't make a difference if the ions are in solution or not. I think the end products will be the same.

 

~Scott

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I wonder whether the ionic equation is different.

Such as now, chlorine atom is now considered taking part in the reaction as it finally becomes ions.

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I was just thinking that if the HCL is gas, and the NH4OH is aqueous, then wouldn't the HCL have to become aqueous in order to react with the NH4OH? I think the ionic equation would be the same either way unless theres some rule im not remembering.

 

~Scott

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How about the ionic equation between solid sodium carbonate and hydrochloric acid?

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Ah now that one is easy...

HCl(aq) + NaCO3(s) = HCO3(aq) + NaCl(aq)

HCl = H+ + Cl-

NaCO3= Na+ + CO3-

 

2HCO3(aq) quickly decomposes into H2O(l) and CO2(g)

 

So it is more like HCl + NaCO3 = H2O + CO2 + NaCl (<= I know its not balanced)

 

~Scott

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"Ammonia dissolves in water and react with water to form ammonium ions and hydroxide ions.

NH3(aq)+ H2O(l)+ HCl(aq)----> H2O(l)+ NH4Cl(aq)

Or NH4OH(aq)+HCl(aq)---->NH4Cl(aq)+H2O(l)

 

Moreover, can anyone write down the ionic equation of hydrogen chloride gas dissolve in sodium hydroxide?"

 

ammonia in water is NH3(aq) not NH4OH. hydrogen chloride gas doesn't really dissolve in sodium hydroxide. it just reacts with the sodium hydroxide, forming a soluble salt.

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NH3(aq) is a weak base in equilibrium.

NH3(aq) + H2O(l) <=> NH4+ + OH-

So wouldnt it be fair to say that the reactants are still NH4+ and OH-, even if its not in the form of NH4OH? just curious.

NH3(aq) +HCL(g) + H2O = NH4CL + H2O

 

Primarygun- The ionic equation for the reaction between NaOH and HCL is

Na+ + OH- + H+ + Cl- = H2O + NaCl

Half equations

NaOH = Na+ + OH-

HCl = H+ + Cl-

 

~Scott

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"NH3(aq) is a weak base in equilibrium.

NH3(aq) + H2O(l) <=> NH4+ + OH-"

to the former, yes. to the latter, no, not really. it's been recently found that ammonia in solution is NH3(aq), not NH4OH(aq)

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Na+ + OH- + H+ + Cl- = H2O + NaCl

Half equations

NaOH = Na+ + OH-

HCl = H+ + Cl-

Are you sure? The original reactant is a gas.

NH3(aq)+ H2O(l)+ HCl(aq)----> H2O(l)+ NH4Cl(aq)

Or NH4OH(aq)+HCl(aq)---->NH4Cl(aq)+H2O(l)

Thanks budullewraagh.

We usually eliminate the H2O(l) of both sides, right?

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Primarygun- The ionic equation for the reaction between NaOH and HCL is

Na+ + OH- + H+ + Cl- = H2O + NaCl

Half equations

NaOH = Na+ + OH-

HCl = H+ + Cl-

 

~Scott

 

 

That is not correct. The only way that is correct is if the NaCl precipitates out of solution. The ionic equation for NaOH reacting with HCl is

Na+ + OH- + H+ + Cl- -> H2O + Na+ + Cl-

 

The Net Ionic Equation is

H+ + OH- -> H2O

 

For the reaction with aqueous NaOH and HCl gas, the reaction is the same as hydrochloric acid and sodium hydroxide. This is because in order for the HCl to react with the ionic NaOH, it has to dissolve in water first. If the NaOH was anhydrous, then you could get a reaction between it and the HCl gas.

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