Self Test 5G.3A

Moderators: Chem_Mod, Chem_Admin

GFolk_1D
Posts: 101
Joined: Fri Aug 09, 2019 12:15 am

Self Test 5G.3A

Postby GFolk_1D » Mon Jan 06, 2020 2:30 pm

Write the equilibrium constant fir the reaction 2 AgNO3 (aq) + 2NaOH (aq)-----> Ag2O (s) + 2NaNO3 (aq) + H2O (l)

I'm a bit confused as to how to take the net ionic equation into account. Thanks!

Angus Wu_4G
Posts: 102
Joined: Fri Aug 02, 2019 12:15 am

Re: Self Test 5G.3A

Postby Angus Wu_4G » Mon Jan 06, 2020 3:23 pm

For the net ionic equation, you should separate the ions in all compounds and cancel out ions that appear in both the reactants and products side. For this particular problem, both Na+ and NO3- will be cancelled out, leaving the equation as just 2Ag + 2OH- yields Ag20 + H2O. Then write your equilibrium constant for this reaction.

Sam McNeill 1E
Posts: 110
Joined: Sat Aug 24, 2019 12:17 am

Re: Self Test 5G.3A

Postby Sam McNeill 1E » Mon Jan 06, 2020 3:34 pm

For this problem, also remember that the activity of solids and liquids is 1, so you would not consider them when calculating.

Alison Hamant 2B
Posts: 2
Joined: Wed Nov 14, 2018 12:19 am

Re: Self Test 5G.3A

Postby Alison Hamant 2B » Mon Jan 06, 2020 6:45 pm

Do you normally use the net iconic equation when calculating the equilibrium constant?

anjali41
Posts: 109
Joined: Fri Aug 09, 2019 12:15 am

Re: Self Test 5G.3A

Postby anjali41 » Mon Jan 06, 2020 8:14 pm

Dr. Lavelle hasn't mentioned anything yet about using the ionic equations, so I think it might be a strategy specific to this problem/problems like it.


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 1 guest