Writing net ionic equations (having problems)

  • Thread starter Thread starter mousechild
  • Start date Start date
  • Tags Tags
    Ionic Net Writing
AI Thread Summary
The discussion revolves around writing net ionic equations for three balanced chemical reactions. The user expresses confusion about balancing the equations and the proper representation of ions, particularly with Ba(OH)2. Key points include the importance of not separating solids, liquids, or gases in net ionic equations and identifying spectator ions to simplify the equations. The user successfully derives the net ionic equations for the first two reactions and seeks confirmation on their accuracy. Overall, the conversation highlights the challenges of understanding net ionic equations and the clarification provided by fellow forum members.
mousechild
Messages
2
Reaction score
0
We have been given three balanced equations to write as net ionic equations. Our teacher forgot to teach us this bit and has now left the college. I'm really stuck, any help would be so kindly appreciated TY x



The equations are:

1. Pb(NO3)2 (aq) + 2KCl (aq) = PbCl2(s) + KNO3 (aq)

2. 2HCL(aq) + Ba(OH)2(aq) = BaCl2(aq) + 2H2O(l)

3. NaCl(aq) + AgNO3(aq) = NaNO3(aq) +AgCl(s)




With the first equation I don't think it is balanced, so I tried to firstly balance it by writing:

Pb(NO3)2(aq) + 2KCL(aq) = PbCl2(s) + 2KNO3(aq)

Then I attempted to write it ionically:

[Pb]2+ + 2[NO3]- + [K]+ + [Cl]- = [Pb]+2 + 2[Cl]- + 2[K]+ + 2[NO3]-


for the second one I got as far as writing: 2[H]+ + 2[Cl}- but I am very unsure of how to write Ba(OH)2. Is there 2 lots of Ba and 2 lots of OH? I don't understand why the OH is in brackets. :(

I haven't started trying to figure out the third question yet, I've spent hours trying to work out how you do the first two and I'm getting in a bit of a panic.


If you have been so kind as to take the time to read my problem (I know it's long and I sound like a complete idiot!) then thanks so much, and if you could help me then even more thanks. xx


 
Physics news on Phys.org
Generally, whenever you see a solid, liquid, or gas in a chemical equation, that compound does not separate into ions in the net ionic equation. So in your first one, don't separate PbCl2. Then you cross out the spectator ions, or the ions that appear on both sides of the equation, and what you have left makes the net ionic equation.

For Ba(OH)2 in 2, think about the charges of the ions: Ba2+ and OH-. You need two OH- ions to balance the charge of Ba2+.
Subscripts after parentheses apply only to what is inside the parentheses.
 
Thanks so much Bohrok, it's starting to make sense (I think!)...for the first one I have got:

Pb2+ + 2Cl- = PbCl2

and for the second:

2H+ + 2OH- = 2H2O

and for the third:

Cl- + Ag+ = AgCl am I correct? x
 
Thread 'Confusion regarding a chemical kinetics problem'
TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
Back
Top