Back
to top
Ionic equation for H2SO4 and NaOH
Watch
Announcements
Page 1 of 1
Go to first unread
Skip to page:
The reaction goes like this:
H2SO4 + 2NaOH ---> Na2SO4 + 2H2O
so is the ionic equation
H+ + OH- ---> H2O
or
2H+ + 2OH- --> 2H2O
H2SO4 + 2NaOH ---> Na2SO4 + 2H2O
so is the ionic equation
H+ + OH- ---> H2O
or
2H+ + 2OH- --> 2H2O
1
reply
my mistake... i edited the question. so is it the first one or the second one.
0
reply
Report
#6
they are both fine really, but by convention the top one
x + y = z is the same as 2x+2y = 2z
x + y = z is the same as 2x+2y = 2z
0
reply
Report
#7
Could someone refresh my memory and tell me how you deduce ionic equations again? (My chemistry has become a little rusty)
0
reply
Report
#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)
Could someone refresh my memory and tell me how you deduce ionic equations again? (My chemistry has become a little rusty)
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
reply
Report
#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)
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)
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
reply
Report
#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?
Ahh, cheers, mate. I thought it was something like that; the ions which are canceled are known as 'spectator ions', aren't they?
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.
0
reply
Report
#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
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
0
reply
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
reply
Report
#14
(Original post by ashley193)
basically can someone just explain the whole question to me. I am so confused
basically can someone just explain the whole question to me. I am so confused
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
reply
Report
#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
reply
X
Page 1 of 1
Go to first unread
Skip to page:
Quick Reply
Today on TSR
-
Ofqual consultationTeachers to use 'mini-exams' and other work to decide grades
- Is it too late to do well in my A-levels?
- What Harry Potter house are you in?
- 2021 wellbeing blog launch
- Student tips on lockdown mental health