Consider the reaction$$\mathrm{Fe}^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftharpoons \mathrm{FeSCN}^{2+}(a q)$$.How will the equilibrium position shift if a. water is added, doubling the volume? b. \(\mathrm{AgNO}_{3}(a q)\) is added? (AgSCN is insoluble.) c. \(\mathrm{NaOH}(a q)\) is added? \(\left[\mathrm{Fe}(\mathrm{OH})_{3} \text { is insoluble. }\right]\) d. \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) is added? c. \(\mathrm{NaOH}(a q)\) is added?is insoluble.] d. \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) is added?

a. When water is added, doubling the volume, the concentration of all ions decreases, and the equilibrium shifts to the right, favoring the formation of \(\mathrm{FeSCN}^{2+}(a q)\). b. When \(\mathrm{AgNO}_{3}(a q)\) is added, the concentration of \(\mathrm{SCN}^-\) ions decreases due to the formation of insoluble \(\mathrm{AgSCN}\), and the equilibrium shifts to the left, favoring the formation of more \(\mathrm{SCN}^-\) ions. c. When \(\mathrm{NaOH}(a q)\) is added, the concentration of \(\mathrm{Fe}^{3+}\) ions decreases due to the formation of insoluble \(\mathrm{Fe}(\mathrm{OH})_{3}\), and the equilibrium shifts to the left, favoring the formation of more \(\mathrm{Fe}^{3+}\) ions. d. When \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) is added, the concentration of \(\mathrm{Fe}^{3+}\) ions increases, and the equilibrium shifts to the right, favoring the formation of more \(\mathrm{FeSCN}^{2+}(a q)\).