You need to make an aqueous solution of 0.216 m manganese(ii) sulfate for an experiment in lab, using a 125 ml volumetric flask. how much solid manganese(ii) sulfate should you add?

125 mL= 0.125 L
0.216 M==0.126 mol/L

0.126 mol/L*0.125L=0.0158 mol MnSO4 are needed
Molar mass (MnSO4)= 54.9+32.1+4*16.0= 151 g/mol

 151 g/mol*0.0158 mol=2.39 g solid  MnSO4

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.

It is a ok  i know i have a brain functioning well.