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# Writing net ionic equations and predict precipitate.

Registered User Posts: 4,706 Senior Member
edited October 2006
4. Write the net ionic equations for the reation, if any, that occurs when aqueous solutions of the following are mixed.

f. silver nitrate and ammonium carbonate
How do I do this?

g. strontium nitrate and potassium iodide
Sr2+ (aq) + I- (aq) ---> SrI2 (s)
Is this right?

3. Find the precipitates, if any.

e. Hg2(NO3)3 (aq) + CuSO4 (aq)
>

f. Ni(NO3)2 (aq) + CaCl2 (aq)
>
No precipitate. Is this right?

g. K2CO3 (aq) + MgI2 (aq)
>
Precipitate formed: KI
Is this right?

h. Na2CrO4 (aq) + AlBr3 (aq)
>

I am really bad at predicting products and finding the precipitates. Can someone look over these and help me out? I have a quiz on Tuesday on this. AHHHH...
Post edited by lil_killer129 on

## Replies to: Writing net ionic equations and predict precipitate.

• Registered User Posts: 1,842 Senior Member
Ok for E F G and H I may be totally wrong... but
in E. shouldn't HGso4 be a precip? I remember So4 is sol in a lot of things but I don't think it is in HG.
In f. i think ur right
G. Woah Woah Woah. You really need to know I BR and CL are sol in almost everything. Also group 1 metals are also sol in almost anything. however MgCo3 is not sol.
For h. i think its none (not sure)
I got a 5 on the ap chem.. i remember solubility still pretty well.
• Registered User Posts: 4,706 Senior Member
Thanks Gyros321. Can anyone else offer me any help? I really want to ace this quiz on Tuesday.
• Registered User Posts: 84 Junior Member
hum .. I dont know how I can help you but since we are learning the same thing right now i could give you some advice. When you are predicting if the reaction is a preciptation, you have to know the solubility rule. If an element is insoluble then yuou will have a preciptation reaction cuz it will turn solid. And remembers IONS have to be involved in order to preciptate. Therefore its important to look for the ions first, if no ions, then you can tell that its not gonna be a preciptation. Two nonmetals .. no precipation. (thats all I can remember so far.. )
• Registered User Posts: 807 Member
lol, we're doing the same thing 2
• Registered User Posts: 99 Junior Member
f. silver nitrate and ammonium carbonate

Ag2+ + CO3 2- => AgCO3

g. strontium nitrate and potassium iodide
Sr2+ (aq) + I- (aq) ---> SrI2 (s)
Is this right?

I think it's:

I- => I2 (g)

h. Na2CrO4 (aq) + AlBr3 (aq)
>

precipitate is Al2CrO43

btw...I got a 5 on the AP, so hopefully i have some credibility :)
• Registered User Posts: 2,500 Senior Member
u really have to know ur solubilities. i just learned this stuff yesterday but it is very straightforward. and know ur charges of each ions. remember, always switch the positive and negative ions of each compound and then rewrite the new compounds. then remember see which is soluble and if they both are, then there is no reactant.
• Registered User Posts: 327 Junior Member
nitrate is always soluble
acetate is always soluble
all chlorides/bromides/iodides are soluble except with silver,mercury lead
sulfate is always soluble except with strontium,barium,mercury,lead

hydroxides/sulfides are always insoluble except with group 1a metal cations, ammonium, and strontium barium calcium
phosphate/carbonate are always insoluble except with group 1a metal cations and ammonium
This discussion has been closed.