Question

1) The concentration of H₂C₂O₄ in a solution is determined by titrating it with a 0.1053 M permanganate solution. The balanced net ionic equation for the reaction is:

• 2MnO₄^-(aq) + 5H₂C₂O₄(aq) + 6H₃O⁺(aq) -- > 2Mn²⁺(aq) + 10CO₂(g) + 14H₂O(l)

In one experiment, 24.77 mL of the 0.1053 M permanganate solution is required to react completely with 20.00 mL of theH₂C₂O₄ solution. Calculate the concentration of the H₂C₂O₄ solution.

Answer in _______ M

2) A dichromate solution is standardized by titrating it with a 0.1322 M Fe²⁺ solution. The balanced net ionic equation for the reaction is:

• Cr₂O₇^2-(aq) + 6Fe²⁺(aq)+14H₃O⁺(aq) --> 2Cr³⁺(aq) + 6Fe³⁺(aq)+21H₂O(l)

If 22.78 mL of the 0.1322 M Fe²⁺ solution is required to react completely with 40.00 mL of the dichromate solution, calculate the concentration of the dichromate solution.

Answer in _______ M

3) Suppose a solution of the reducing agent Cu⁺ is titrated with a solution of the oxidizing agent permanganate. The balanced net ionic equation for the reaction is:

• MnO₄^-(aq) + 5Cu⁺(aq)+8H₃O⁺(aq) --> Mn²⁺(aq) + 5Cu²⁺(aq)+12H₂O(l)

What volume (in mL) of a 0.1515 M MnO₄^- solution would be required to consume the Cu⁺ in a 30.00 mL sample of a solution containing 0.4734 M Cu⁺?

Answer in ______ mL

Answer 1