A student performs a redox titration between 10.0 mL of hypochlorous acid, HClO(aq), and chromium (III) nitrate, Cr(NO₃)₃(aq). The half-reaction are given below. 7 H₂O + 2 Cr³ ⟶ Cr₂O₇²(aq) + 14 H(aq) + 6 e-
2 HClO(aq) + 2 H(aq) + 2 e- ⟶Cl₂(g) + H₂O
Give the overall oxidation-reduction reaction.
What is the oxidation number of chromium in Cr₂O₇²- ?
Give one indication that this is an oxidation-reduction reaction. Explain your reasoning.
As the reaction proceeds the solution becomes more acidic and the pH of the solution decreases. Explain why.
The titration uses chromium (III) nitrate, yet nitrate does not appear in the half-reaction. Explain the role of nitrate in the reaction
The 10.0 mL of hypochlorous acid requires 26.5 mL of 0.120 M chromium (III) nitrate to reach equivalence.
Determine the initial molarity of acid
Determine the final molarity of Cr₂O₇²- once the reaction has gone to completion. (assume the volumes are addictive)
Chlorine gas is only slightly soluble in water.
What intermolecular force must be present between the chlorine gas and water?
The chlorine gas is collected in a gas collection vessel. The pressure of the chlorine gas alone is Hg at 25.0 Celsius
Determine the volume of chlorine gas collected, in L.