Which solution would effectively reduce 0.012 mol of bromine to bromide ions?

To determine which solution can effectively reduce 0.012 mol of bromine (Br2) to bromide ions (Br^-), it's important to look at the reducing agents and their equivalents.

Bromine is being reduced to bromide ions, and in this context, we should consider the stoichiometry of the redox reaction. The reduction of bromine (as Br2) to bromide involves a transfer of electrons. One mole of Br2 requires two moles of electrons to be completely reduced to two moles of bromide ions.

To find out how many moles of the reducing agent are required, we first calculate the number of moles of bromine needing reduction:

• For 0.012 mol of Br2, the moles of electrons required are 0.012 mol Br2 * 2 moles of electrons/1 mol Br2 = 0.024 mol of electrons.

Now, let's look at option D, which is 50 cm³ of 0.24 mol dm−3 H2SO3(aq):

1. The concentration of H2SO3 can be converted to moles:

• Volume = 50 cm³ = 0.050 dm³