For 1) write out the oxidation and reduction half reactions:
Fe2+ ---> Fe3+ +e-
Cr2O72- + 14 H+ +6e- ---> 2Cr3+ +7H2O
since you need conservation of mass with the electrons, you multiply the oxidation half-rxn by 6, so you have 6 electrons on either side of the equation. the correct answer is A.
For 2) remember that molarity1*volume1 = molarity2 * volume2 if the moles are kept constant. therefore 1.600L * .05M = 2L * X (where x is new molarity). X = .04.
Since pH = -log [H+] and since you can assume that HNO3 will dissociate completely, you know that -log (.04) = 1.40 is the pH.
For 3) BaCrO4 is in a ration of one mole cation to one mole anion. what you need to do is find out how many moles of each are in the original solutions (M*V=n). They tell you that you have a limiting and excess equation, and that Ba2+ is in excess, so all you have to do is set up a box:
Ba2+ + CrO42- ----> BaCrO4
initial x y 0 (i didn't do the calculations, but x=
change -y -y y moles of Ba2+ originally, and y =
final x-y 0 y moles of CrO42- originally)
solve for the final conc. of Ba2+ by dividing x-y by the total volume.