For this experiment you want to prepare a 0.10 m solution of sodium hydroxide. how many grams of sodium hydroxide must be added to give you 500.0 ml of that solution? question 1 options:

c×v
n (NaOH) =
1000

0.1 × 500
n (NaOH) =
1000
n (NaOH) = 0.05 moles

Mass= Mr(NaOH) × moles
Mass= (23+16+1) × 0.05
Mass=2.15 g (2.15 grams)

The answer is not c

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.