The Student Room Group
Uni students - Complete our survey >>
Uni students - Complete our survey >>
Uni students - Complete our survey >>

Balancing redox in basic solution help!!!!

Hi guys, I have just balanced a redox reaction in a basic solution, everything adds ups, apart from the charges at the end...
I’ve got -4 on one side and -2 on the other. Is it normal for the charges to not balance sometimes? And if so, what is it this called?
Reply 1
Avatar for Interea
Interea
19
As far as I'm aware your charges should balance in a redox equation (unless I'm misunderstanding you). Could you possibly post what you've got?
Original post by Rasaa22
Hi guys, I have just balanced a redox reaction in a basic solution, everything adds ups, apart from the charges at the end...
I’ve got -4 on one side and -2 on the other. Is it normal for the charges to not balance sometimes? And if so, what is it this called?
Reply 2
Avatar for Rasaa22
Rasaa22
OP
12
Yes, question: HCN > CO3^2- + NH3. In a basic solution. (CO3^2- as in Carbon and 3 oxygen with -2 ion charge)

Ended up:
4OH- + HCN > CO3^2- + NH3 + H2O
The atoms balance but not the charge
Original post by Interea
As far as I'm aware your charges should balance in a redox equation (unless I'm misunderstanding you). Could you possibly post what you've got?
Reply 3
Avatar for Interea
Interea
19
I think in this case you can just add electrons to balance the charges, as it is not a full redox equation (i.e. combining 2 half equations). See what anyone else says though, I've got a headache so I'm not exactly with it right now...
Original post by Rasaa22
Yes, question: HCN > CO3^2- + NH3. In a basic solution. (CO3^2- as in Carbon and 3 oxygen with -2 ion charge)

Ended up:
4OH- + HCN > CO3^2- + NH3 + H2O
The atoms balance but not the charge
Reply 4
Avatar for Rasaa22
Rasaa22
OP
12
THANK YOU SO MUCH! That’s exactly what I thought, adding electrons at the end to balance the charge. But I wondered if there was any rules, and what does it mean by ‘not a full redox equation’
Sorry to hear it, hope you feel better soon!! Xxxx
Original post by Interea
I think in this case you can just add electrons to balance the charges, as it is not a full redox equation (i.e. combining 2 half equations). See what anyone else says though, I've got a headache so I'm not exactly with it right now...
Reply 5
Avatar for Interea
Interea
19
Sometimes they refer to equations with electrons and only either oxidation or reduction as half equations, and then when you combine a reduction and oxidation equation (balancing to cancel out electrons) you get a full redox equation.
Original post by Rasaa22
THANK YOU SO MUCH! That’s exactly what I thought, adding electrons at the end to balance the charge. But I wondered if there was any rules, and what does it mean by ‘not a full redox equation’
Sorry to hear it, hope you feel better soon!! Xxxx

Quick Reply

Related discussions

Latest

Trending

Trending

Articles for you