10 Questions
What is the oxidation product of the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
Molecular iodine (I2)
What is the reducing agent in the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
Iodide ion (I-)
What is the oxidation number of manganese in the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
+4
What is the oxidation number of iodine in the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
-1
What is the purpose of adding two H2O molecules to the right-hand side of the reduction half-reaction?
To balance the O atoms
What is the purpose of adding four H+ ions to the left-hand side of the reduction half-reaction?
To balance the H atoms
What is the purpose of adding three electrons to the left-hand side of the reduction half-reaction?
To balance the charges
What is the overall reaction obtained by adding the oxidation and reduction half-reactions?
4 MnO4- + I- → MnO2 + I2
What is the oxidation half-reaction in the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
2I- → I2 + 2e-
What is the reduction half-reaction in the oxidation of iodide ion (I-) by permanganate ion (MnO4-) in basic solution?
MnO4- + 4 H+ + 3e- → MnO2 + 2 H2O
Calculate the equilibrium concentration of hydrogen ions and nitrous acid, and check the validity of the approximation. Also, determine the pH of the solution using weak acid and base equilibria concepts.
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