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anonymous
 4 years ago
HELP! Can you someone tell me what the net ionic equations for these are..its been driving me crazy!
a) AgNO3 + KCl
b) Ni(NO3)2 + Na2S
c) CaCl2 + Na2CO3
anonymous
 4 years ago
HELP! Can you someone tell me what the net ionic equations for these are..its been driving me crazy! a) AgNO3 + KCl b) Ni(NO3)2 + Na2S c) CaCl2 + Na2CO3

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AravindG
 4 years ago
Best ResponseYou've already chosen the best response.3Na2S (aq) + Ni (NO3)2 (aq) > 2 NaNO3 + NiS

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Yes i got that but i am looking for the "net ionic equation"

Xishem
 4 years ago
Best ResponseYou've already chosen the best response.1First, let's split up the first reaction into its component ions...\[Ag(aq)^++NO_3^(aq)+K^+(aq)+Cl^(aq)\]Then, find out what the products will be. In this case, it's a precipitation reaction...\[AgNO_3(aq)+KCl(aq) \rightarrow AgCl(s) + KNO_3(aq)\]Now, this is the overall equation. The net ionic equation involves breaking each compound into its component ions, and dropping all ions that appear in aqueous solution on both the reactants and products side. Doing this to the above equation...\[Ag^+(aq)+Cl^(aq) \rightarrow AgCl(s)\]This is the net ionic equation for a.

AravindG
 4 years ago
Best ResponseYou've already chosen the best response.3oh srry i will help u in c

AravindG
 4 years ago
Best ResponseYou've already chosen the best response.32) Write out the total ionic equation and cancel anything that is common on both sides Ca+2(aq) + 2Cl(aq) + 2Na+(aq) + CO32(aq) > CaCO3(s) + 2Na+(aq) + 2Cl(aq) so the net ionic equation becomes: Ca+2(aq) + CO32(aq) > CaCO3(s) this is net eqn for c

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Xishem why did you get rid of the K and NO3

Xishem
 4 years ago
Best ResponseYou've already chosen the best response.1The net ionic equation is the total equation with all spectator ion removed. Spectator ions are ions which are present in aqueous solution on both sides of the equation. In other words, they didn't participate in the reaction (spectators). I'll show it for part a...\[Ag^+(aq)+NO_3^(aq)+K^+(aq)+Cl^(aq) \rightarrow\]\[Ag^+(s)+Cl^(s)+K^+(aq)+NO_3^(aq)\]The potassium ion and the nitrate ion exist in aqueous solution on both sides of the equation, therefore they are spectator ions and are to be removed to give...\[Ag^+(aq)+Cl^(aq) \rightarrow AgCl(s) \]Which is the net ionic equation. Make sense?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0OHHHHH yessss okay that makes a lot more sense now...thanks guys! i will try b) ill post what I got

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0would it be Ni2(aq) + S2 (aq) > NiS(s)

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0:D!!!! THANKS Xishem and AravindG! I wish i could give more than 1 medals hah
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