# Ionic equation for H2SO4 and NaOH

Watch
Announcements
Thread starter 12 years ago
#1
The reaction goes like this:

H2SO4 + 2NaOH ---> Na2SO4 + 2H2O

so is the ionic equation

H+ + OH- ---> H2O
or
2H+ + 2OH- --> 2H2O
1
12 years ago
#2
first one
0
12 years ago
#3
I'm pretty sure it's the last one. In the reaction, it's '2NaOH'.
0
12 years ago
#4
The initial equation isn't balanced...
0
Thread starter 12 years ago
#5
my mistake... i edited the question. so is it the first one or the second one.
0
12 years ago
#6
they are both fine really, but by convention the top one

x + y = z is the same as 2x+2y = 2z
0
12 years ago
#7
Could someone refresh my memory and tell me how you deduce ionic equations again? (My chemistry has become a little rusty)
0
12 years ago
#8
(Original post by LurkerintheDark)
Could someone refresh my memory and tell me how you deduce ionic equations again? (My chemistry has become a little rusty)
1) Write out the normal equation: NaOH(aq) + HCl(aq) ---> H2O(l) + NaCl(aq)
2) Split up all the ions: Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) ----> H2O(l) + Na+(aq) + Cl-(aq)
3) Cancel the ions on both sides: OH-(aq) + H+(aq) ---> H2O(l)
0
12 years ago
#9
(Original post by EierVonSatan)
1) Write out the normal equation: NaOH(aq) + HCl(aq) ---> H2O(l) + NaCl(aq)
2) Split up all the ions: Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) ----> H2O(l) + Na+(aq) + Cl-(aq)
3) Cancel the ions on both sides: OH-(aq) + H+(aq) ---> H2O(l)
Ahh, cheers, mate. I thought it was something like that; the ions which are cancelled are known as 'spectator ions', aren't they?

By the way, why doesn't water water split into seperate ions? And is it true that in a regular equation, the precipitate on the R.H.S. isn't split into ions during cancellation, and remains a compound? Thanks.
0
12 years ago
#10
(Original post by LurkerintheDark)
Ahh, cheers, mate. I thought it was something like that; the ions which are canceled are known as 'spectator ions', aren't they?
yep

By the way, why doesn't water water split into separate ions? And is it true that in a regular equation, the precipitate on the R.H.S. isn't split into ions during cancellation, and remains a compound? Thanks.
Water is covalent not ionic. If you get a precipitate then it doesn't dissolve in the solvent so it stays a solid...so yes
0
12 years ago
#11
(Original post by EierVonSatan)
yep

Water is covalent not ionic. If you get a precipitate then it doesn't dissolve in the solvent so it stays a solid...so yes
Aa--haaaa; thanks for the enlightenment, man. So, in a equation with hydrogen molecules, you wouldn't be able to seperate them into seperate ions because it is a covalent molecule? Of course...
0
Thread starter 12 years ago
#12
correct, if you're talking about H2 molecules. but if its about hydrogen ions (eg HCl dissolved in aq solution) then its something different altogether.
0
2 years ago
#13
basically can someone just explain the whole question to me. I am so confused
0
2 years ago
#14
(Original post by ashley193)
basically can someone just explain the whole question to me. I am so confused
On Halloween you have dug up a 10 year old thread!
The thread has more the one question in the end.

Can I suggest you start a new thread with just the question you have today? 😁
0
1 year ago
#15
Water isn't split into ions because water is a liquid and the others are in the aqueous state, so the state that is common in all elements are splitted into ions but the one that is different stays the same.
0
X

new posts
Back
to top
Latest
My Feed

### Oops, nobody has postedin the last few hours.

Why not re-start the conversation?

see more

### See more of what you like onThe Student Room

You can personalise what you see on TSR. Tell us a little about yourself to get started.

### Poll

Join the discussion

#### Have you experienced financial difficulties as a student due to Covid-19?

Yes, I have really struggled financially (22)
14.01%
I have experienced some financial difficulties (42)
26.75%
I haven't experienced any financial difficulties and things have stayed the same (65)
41.4%
I have had better financial opportunities as a result of the pandemic (23)
14.65%
I've had another experience (let us know in the thread!) (5)
3.18%