A solution contains both iron(II) and iron(III) ions. A 50.00 mL sample of the solution is titrated with 34.80 mL of 0.02800 M KMnO4, which oxidizes all the Fe2+ to Fe3+. The permanganate ion is reduced to manganese(II) ion. Another 50.00 mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The resulting solution is again titrated with 0.02800 M KMnO4; this time 47.80 mL is required. What are the concentrations of Fe2+ and Fe3+ in the (original) solution?

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explanation:

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

the correct answer would be b) volume versus temperature, because they are also directly proportional.