Question
How would I balance the following redox equation?
I know the Charge on the Br is 5, but i am comfused on where to go from there.
H20 + Br^- + Al^3+ -> Al + BrO3^- + H^+
Thank you so much in advance
I know the Charge on the Br is 5, but i am comfused on where to go from there.
H20 + Br^- + Al^3+ -> Al + BrO3^- + H^+
Thank you so much in advance
Answers
DrBob222
Br is -1 on the left; +5 on the right. Loss of 6e.
Al is +3 on the left; 0 on the right. Gain of 3e.
Multiply the Br half by 1.
Multiply the Al half by 2.
Then balance the H^+ and H2O
Post your work if you get stuck.