A sample solution contains Sn²⁺ ions and is titrated with a 0.0500 M solution of Ce⁴⁺, consuming 35.44 mL of the Ce⁴⁺ solution. The products of the redox reaction are Sn⁴⁺ and Ce³⁺. What mass of Sn²⁺ was present in the original solution?

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is: Sn²⁺ + Ce⁴⁺ → Sn⁴⁺ + Ce³⁺ From the balanced equation, we can see that: 1 mole of Ce⁴⁺ reacts with 1 mole of Sn²⁺. Therefore, moles of Sn²⁺ in original solution: = moles of Ce⁴⁺ used for titration = concentration of Ce⁴⁺ x volume of Ce⁴⁺ used = 0.0500 mol/L x 0.03544 L = 0.001772 mol Mass of Sn²⁺ in original solution: = moles of Sn²⁺ x molar mass of Sn²⁺ = 0.001772 mol x (118.76 g/mol + 32.06 g/mol) (molar mass of Sn²⁺) = 0.210 g Therefore, the answer is B.

A Sample Solution Contains Sn2+ Ions and Is Titrated with a 0.0500

A Sample Solution Contains Sn²⁺ Ions and Is Titrated with a 0.0500