Balancing Redox Reaction Basic Balancing Basic Balancing in
Balancing Redox ½ Reaction (Basic)
Balancing Basic • Balancing in basic solution is just like acidic with one additional step • When balancing in acidic you will have H+ at the end +, you want OH • In basic you don’t want H -
To change to basic • To change to basic, simply add an equivalent number of OH- to each side and simplify
Example • Balancing the following by using the ½ reaction method in a basic solution • As. O 4 -3 + Zn H 3 As + Zn +2 • Acidic: • 11 H+ + As. O 4 -3 + 4 Zn H 3 As + 4 H 2 O + 4 Zn+2 • Basic: • 11 H+ + As. O 4 -3 + 4 Zn H 3 As + 4 H 2 O + 4 Zn+2 • +11 OH+ 11 OH • 11 H 2 O + As. O 4 -3 + 4 Zn H 3 As + 4 H 2 O + 4 Zn+2+ 11 OH • 7 H 2 O + As. O 4 -3 + 4 Zn H 3 As + 4 Zn+2+ 11 OH-
Another Example • • • Ag + NO 3 - Ag + + N+2 Acidic: 3 Ag +6 H+ + NO 3 - 3 Ag + + N+2+ 3 H 2 O Basic: 3 Ag +6 H+ + NO 3 - 3 Ag + + N+2+ 3 H 2 O + 6 OH- • 3 Ag +6 H 2 O + NO 3 - 3 Ag + + N+2+ 3 H 2 O + 6 OH • 3 Ag +3 H 2 O + NO 3 - 3 Ag + + N+2 + 6 OH-
One More • Mn(NO 3)2 + Na. Bi. O 3 + HNO 3 Na. Mn. O 4 + Bi(NO 3)3 + H 2 O + Na. NO 3 • Acidic: • 2 Mn+2 + 14 H+ + 5 Bi. O 3 - 2 Mn. O 4 - + 5 Bi +3 + 7 H 2 O • Basic: • 2 Mn+2 + 14 H+ + 5 Bi. O 3 - 2 Mn. O 4 - + 5 Bi +3 + 7 H 2 O + 14 OH • 2 Mn+2 + 14 H 2 O + 5 Bi. O 3 - 2 Mn. O 4 - + 5 Bi +3 + 7 H 2 O+ 14 OH • 2 Mn+2 + 7 H 2 O + 5 Bi. O 3 - 2 Mn. O 4 - + 5 Bi +3 + 14 OH-
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