1. In the determination of the quilibrium constant for the hydrolysis of 5.00mL of SbCl3, 24mL of water was addedand 0.0015 mol SbOCl precipitated.
a) Should [SbOCl] now be included in the calcuation?
b) How many moles of SbCl3 remain in thesolution? What is the concentration of SbCl3?
c) How many moles of H+ and Cl-were produced by the reaction? Calculate the concentration ofH+ and Cl-. (Remember that theSbCl3 is in 6M HCl.)
d) Calculate the equilibrium constant using the sevalues.