What are the correct formulas and coefficients for the products of the following double-replacement reaction? rboh + h3po4 -->
a) rb(po4)3 + h2o
b) rbpo4 + 2h2o
c) rb3po4 + 3h2o
d) h3rb + po4oh

Bthats what im doing to and i figured it out it is b

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.