Writing equations

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Valeria Viera 1B
Posts: 60
Joined: Fri Apr 06, 2018 11:05 am

Writing equations

Postby Valeria Viera 1B » Sun Jan 20, 2019 6:24 pm

I took 14A a long time ago so I’m really rusty when it comes to writing equations
Can someone help me by explaining the steps to writing an equation where a weak base/acid reacts with water to make H3O or OH? Like how do you know where the H/proton is being transferred to? (For example in NH3 + H2O or Cl+ H2O )

Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

Re: Writing equations

Postby Mahir_Hasan2C » Sun Jan 20, 2019 6:26 pm

If we were to look at the example of whether NH3 is a base, it would be easier to rely on the Lewis structure. We see that NH3 has a lone pair, this can make a bond with one of the Hydrogens of water and create a hydroxide concentration. All in all, when in doubt make the lewis dot structure.

Andrew Bennecke
Posts: 62
Joined: Fri Sep 28, 2018 12:15 am

Re: Writing equations

Postby Andrew Bennecke » Mon Jan 21, 2019 1:27 pm

We would use the amphoteric compound, Ammonia/NH3, that acts as a weak base in this reaction In order to create Ammonium, NH4+, by mixing it with water. This would give us the equation NH3 (aq) + H2O (l) <-> NH4+ (aq) + OH- (aq).

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Joined: Fri Sep 28, 2018 12:18 am

Re: Writing equations

Postby 605168557 » Wed Feb 13, 2019 11:23 pm

Is there a general structure to follow when writing an equilibrium expression when only given the one reactant for example HClO2(aq)? I understand that the H3O+(aq) ion in addition to the acid's conjugate base(ClO2-(aq)) goes on the right side (product side) of the expression but is H2O(l) always included on the reactant side as well?

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