Chapter 16, Problem 33CI

Interpretation Introduction

(a)

Interpretation:

  ${\text{MnO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right){\text{ + C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\to {\text{Mn}}^{\text{2+}}\left(\text{aq}\right){\text{ + CO}}_{\text{2}}\left(\text{g}\right)$

To write the balanced oxidation half-reaction

Concept Introduction:

Here are the steps to balance redox reaction in an acidic medium:

1. Determine the oxidation numbers of the elements to figure out the oxidation and reduction half of the equation.
2. To balance every half reaction in acidic medium, use H₂O to balance O, use H+ to balance H, and finally use electrons to balance the net charge.

Interpretation Introduction

(b)

Interpretation:

  ${\text{MnO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right){\text{ + C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\to {\text{Mn}}^{\text{2+}}\left(\text{aq}\right){\text{ + CO}}_{\text{2}}\left(\text{g}\right)$

To write the balanced reduction half-reaction

Concept Introduction:

Here are the steps to balance redox reaction sin an acidic medium:

1. Determine the oxidation numbers of the elements to figure out the oxidation and reduction half of the equation.
2. To balance every half reaction in acidic medium, use H₂O to balance O, use H+ to balance H, and finally use electrons to balance the net charge.

Interpretation Introduction

(c)

Interpretation:

${\text{MnO}}_{\text{4}}{}^{\text{-}}\left(\text{aq}\right){\text{ + C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}\to {\text{Mn}}^{\text{2+}}\left(\text{aq}\right){\text{ + CO}}_{\text{2}}\left(\text{g}\right)$

To write the balanced ionic equation for the reaction

Concept Introduction:

Here are the steps to balance redox reaction sin an acidic medium:

1. Determine the oxidation numbers of the elements to figure out the oxidation and reduction half of the equation.
2. To balance every half reaction in acidic medium, use H₂O to balance O, use H+ to balance H, and finally use electrons to balance the net charge.

Interpretation Introduction

(d)

Interpretation:

If 24.6 ml of a KMnO₄ solution is needed to titrate a solution containing 0.758 g of Na₂C₂O₄, the molarity of the KMnO₄ solution should be determined.

Concept Introduction:

$\text{Moles = }\frac{\text{mass}}{\text{molar mass}}$

  $\text{Molarity = }\frac{\text{moles of solute}}{\text{Liter of solution}}$