Net ionic equation question?
How do I write a balanced net ionic equation to illustrate the reaction when hydrochloric acid is added to a bleach solution to produce chlorine ? I think you start with this? HCl + NaClO ---> HClO + NaCl
What is the net ionic equation for HCl+NH3--->???
HCl + NH3 -------> Cl- + NH4+
What is the net ionic equation for NaCl+agNO3--->NaNO3+AgCl?
The net ionic equation simply represents the reaction’s constituent ions minus the “spectator ions,” or the ions that do not synthesize a different compound. This reaction is a precipitation reaction, in which the reagents form solid silver chloride in a sodium nitrate solution.This is the long way: write out the complete ionic equation.Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → Na+(aq) + NO3-(aq) + AgCl(s)Notice the AgCl does not get broken down into its constituent ions. This is because a solid, by definition, won’t ionize unless in the presence of a solvent. Chloride anion compounds are generally soluble in water, but Ag+, the given cation, actually won’t dissolve, as it is an exception. Now we just remove the duplicate ions on both sides and we’re done:Cl-(aq) + Ag+(aq) → AgCl(s)It’ll be faster as you practice. If the reaction is clearly a precipitation (double replacement) reaction, simply find the constituent ions of the precipitate in the reagents and write your equation with said ions. Cheers!
Net ionic equations please help?
complete the net ionice equactions for the successive reactions that take place when a AgNO3 solution is treated, in turn, with HCl, excess NH3, KBr, Na2S2O3, and KI 1) Ag+ + CI+ ------> ________________________________________ 2) AgCI(s) + 2NH3 -------> ________________________________________... 3) Ag(NH3)2+ + Br- ---------->_____________________________... 4) AgBr(s) + 2S2O3^-2------->________________________... 5) Ag(S2O3)2^-3 + I- ---------------->_______________________...
NET IONIC Equation for Carbonate and HCl??? HELP ME PLEASE.?
Hi Okay.!! To start any equation, write the skeletal equation (this means that I simply directly translate the word problem into an equation) and also balance it: CO3- + 2HCl ---> H2CO3 + 2Cl- Note how since carbonate ions have a negative 2- charge, I have to put 2 H+'s to balance the charge. In doing so, I also then have to balance out HCl and Cl- Now we can split up all the ions that we can and write an ionic equation (the net comes afterward). Notice how I didn't split the carbonic acid. It is a weak acid and so I will assume that only a few dissociate. For purposes of a net ionic equation, I will then leave it undissociated. CO3- + 2H+ 2Cl- ---> H2CO3 + 2Cl- Now look how we have 2Cl- on both sides of the equation? They aren't doing anything and so we call them spectator ions. Cancel them out because they're not important in the reaction. Once you do that, then you have the net ionic equation. It's called net because we only want to know the useful part of the reaction. CO3- + 2H+ ---> H2CO3 This is your balanced net ionic equation. In reality though, carbonic acid does dissociate and so this reaction should not be represented by a forward arrow but in fact an equilibrium arrow like this: CO3- + 2H+ ⇌ H2CO3 Anyways, don't worry too much about that for now :) I hope this helped and feel free to ask questions if this was confusing! UPDATE: Haha, no problem Okay! So KHP has the chemical formula KHC8H5O4. Now we can write our molecular equation. Take note that this is a double displacement reaction meaning that the cations of each reactant have switched to yield the products. NaOH(aq) + KHC8H5O4(aq) ---> NaKC8H5O4(aq) + H2O(l) Now to split up all of the ions to make the ionic equation: Na+(aq) + OH-(aq) + K+(aq) + HC8H5O4-(aq) ---> Na+(aq) + K+(aq) + C8H5O42-(aq) + H+(aq)+OH-(aq) Now we cancel out the spectator ions Na+, K+, and OH- from both sides. Here is our net ionic equation: HC8H5O4-(aq) ---> C8H5O42-(aq) + H+(aq) I'm always here for more help :D
What is the molecular, ionic, and net ionic equation of [math]NaCl+Pb(NO_3)_2[/math]?
2NaCl + Pb(NO3)2 --> PbCl2 + 2NaCl2Na+(aq) + 2Cl-(aq) + Pb2+(aq) +2 NO3(aq) --> Pb2+Cl-2(s) + 2Na+(aq) + 2NO3-(aq)Pb2+(aq) + 2Cl-(aq) --> PbCl2(s)
What is the net ionic equation for a solution of silver carbonate, HCl, HNO3, NH3, KI and Na2S?
We need to do this piece by piece. started out with silver carbonate and HCl: Ag2CO3(s) + 2 HCl(aq) --> 2 AgCl(s) + H2O(l) + CO2(g) I had to add NH3: AgCl(s) + 2 NH3(aq) <=> [Ag(NH3)]^2+(aq) + Cl^-(aq) (solution clear) I added HNO3: [Ag(NH3)]^2+(aq) + Cl^-(aq) + 2 H^+(aq) + 2 NO3^-(aq) <=> AgCl(s) + 2 NH4^+(aq) + 2 NO3^-(aq) (made it cloudy). added excess NH3: AgCl(s) + 2 NH3(aq) <=> [Ag(NH3)]^2+(aq) + Cl^-(aq) (made it clear again) then added KI: [Ag(NH3)]^2+(aq) + I^- <=> AgI(s) + 2 NH3(aq) then added Na2S: 2 AgI(s) + Na2S(aq) <=> Ag2S(s) + 2 Na^+(aq) + 2 I^-(aq) Ag2S is less soluble than AgI. I have no idea what you mean by 'alkaline color'. The two terms do not go together. Were you speaking of using a pH paper or litmus paper? These reactions are not written as 'net ionic' equations. You need to go into the reactions above and turn the reactions above into an overall net ionic equation. Just get a piece of paper and put the puzzle together. You can do it.
What are the molecular, complete ionic & net ionic equations of HCl+KHCO3?
When acids acts on a carbonate or hydrogen carbonate, the acid decomposes them into a salt, carbon dioxide gas and water. Molecular: HCl(aq) + KHCO3(aq) -------> KCl(aq) + H2O(l) + CO2(g) Complete ionic: H^+(aq) + Cl^-(aq) + K^+(aq) + HCO3^-(aq) -------> K^+(aq) + Cl^-(aq) + H2O(l) + CO2(g) Net ionic:(obtained by eliminating spectator ions) H^+(aq) + HCO3^-(aq) -------> H2O(l) + CO2(g)