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Author Topic: help with 4 net ionic equations  (Read 7658 times)

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g0ldmember

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help with 4 net ionic equations
« on: March 10, 2005, 01:38:55 AM »

Hey I am doing an assignment but there are a couple questions I couldn't get.  Could somone answer this question for me.
Write a balanced net ionic equation for the following reactants in aqueous solution:

Iron (II) + KI
Iron(III) + KI
Copper (II) + NH3
Silver (I) and NaOH
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Donaldson Tan

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Re:help with 4 net ionic equations
« Reply #1 on: March 10, 2005, 02:50:12 AM »

you should demonstrate that you have at least attempted the problems.

iron(iii) oxides iodide ions
i am not sure if iron(II) iodide is water-soluble
ammonia forms a complex with copper(II)
the last equation is obviously a precipitation reaction
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g0ldmember

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Re:help with 4 net ionic equations
« Reply #2 on: March 10, 2005, 08:11:13 AM »

I did try them... along with the 20 other questions I had those are just the ones i had trouble with b/c i dont understand net ionic equations very  well
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Re:help with 4 net ionic equations
« Reply #3 on: March 10, 2005, 11:24:22 AM »

i do one example for you, on the complexing of copper(ii) ions with ammonia

eg. we add excess ammonia to aq. copper(ii) nitrate solution.

Cu(NO3)2 (aq) + 4NH3 (aq) -> Cu(NH3)42+ (aq) + 2NO3- (aq)

upon observation, you realise that there is nitrate ions on both side of the equation. essentially, the aq nitrate ion remains as nitrate ion, therefore it can be removed from both sides of the equation. hence, the net ionic reaction is:

Cu2+ (aq) + 4NH3 (aq) -> Cu(NH3)42+ (aq)
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"Say you're in a [chemical] plant and there's a snake on the floor. What are you going to do? Call a consultant? Get a meeting together to talk about which color is the snake? Employees should do one thing: walk over there and you step on the friggin� snake." - Jean-Pierre Garnier, CEO of Glaxosmithkline, June 2006
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