In a lab experiment for the dissolution of borax: na2[b4o5(oh)4] x 8 h2o(s) \rightleftharpoons 2 na+(aq) + b4o5(oh)) + 8 h2? o(l)5.00 ml of borax solution was prepared at 19.2 ^{\circ} ? c (292.35 k). it was diluted in a flask and titrated with 3.14 ml of 0.4760 m hcl. ksp? = 0.013355797 or 1.34 x 10-2? for this trial\deltag^{\circ}? = -rtln(k) for this trial was determined to be 10.48999 kj1.) what does the value of \delta g^{\circ} tell you about ksp? at this temperature? 2.) under standard conditions does the solvation reaction favor products or reactants? 3.) since \delta g^{\circ} is positive, why does some of the borax still dissolve at room temperature? (hint: what is the difference between \delta g and \delta g^{\circ}? )4.) does your value for \delta h^{\circ}? suggest that the solvation of borax is endothermic or exothermic? explain why is this result consistent with the observation that more borax dissolved at higher temperatures.