Net ionic compounds

Clueless333

1. Calcium + Water yields calcuim hydroxide + hydrogen
Need balanced and net ionic equation, I got
Ca + 3/2H20 =Ca(OH)2 +H
I can't figure out how to balance it further and I don't know how to get the net equation cause calcuim hydroxide is soluble which means it wouldn't be in the net equation right?

2. Silver(I)nitrate + potassium iodide yields silver(I)iodide + potassium nitrate
I got
AgNO2- + KI = AgI + KNO2-
Ag+ + I- = AgI
Potassium nitrate is soluble so it's not in the net equation but silver iodide is not soluble so it is. Is it balanced ok? Am I right? Heeelllpp!

bomba923

[tex] \text{Ca}}\left( {{\text{OH}}} \right)_2 [/tex] is soluble in water.
Therefore, you will observe hydrolysis, as:
[tex] {\text{H}}_{\text{2}} {\text{O}} \rightleftharpoons {\text{H}}^ + \left( {aq} \right) + {\text{OH}}^ - \left( {aq} \right) [/tex]

*Or you balance it as:
[tex] 2{\text{H}}_{\text{2}} {\text{O}} \rightleftharpoons {\text{H}}_{\text{3}} {\text{O}}^{\text{ + }} \left( {aq} \right) + {\text{OH}}^ - \left( {aq} \right) [/tex]

*Actually, silver(I) nitrate is--> [tex] \text{AgNO} _ 3 [/tex]

You are right, [tex] \text{KNO} _ 3 [/tex] and [tex] \text{AgNO} _ 3 [/tex] and [tex] {\text{KI}} [/tex] are all obviously soluble. Looking at your chemicals, you will observe [tex] {\text{AgI}} [/tex] precipitate. Therefore, the net ionic reaction equation will omit the potassium cations and the nitrate anions:

[tex] {\text{Ag}}^ + \left( {aq} \right) + {\text{I}}^ - \left( {aq} \right) \rightleftharpoons {\text{AgI}}\left( s \right) [/tex]

Remember those common solubility rules. They can help greatly

kinoauyn

ok, I understand how to work out soluble and nonsoluble compounds but I do not know how to write Net Ionic Equations. So if I had:

BaCl2(aq) + 2AgNO3(aq) -->Ba(NO3)2(aq)+2AgCl(s)

Would the Net Ionic equation be:
a) 2Ag+(aq) + 2Cl-(aq) -->2Ag+Cl-(s)

or
b) Ag+(aq) + Cl-(aq) --> Ag+Cl-(s)

or
c) 2Ag+(aq) + Cl2-(aq) --> 2Ag+Cl-(s)

My current guess would be (c)