a) Theoretically, what would be the solubility product (Ksp) of an ionic compound having the general formula MX4 if 5.9x10-14 mol of this compound dissolves in 4.2 mL water at 25 °C? 6.0x10-58 8.1x10-71 2.4x10-62 1.4x10-52 7.5x10-73 b) Mg(OH)2 has Ksp = 1.2 x 10-11 At what minimum pH will a precipitate of Mg(OH)2 form in a solution of 0.23 M Mg(NO3)2? 9.16 5.14 4.84 10.28 8.86

a) Theoretically, what would be the solubility product (Ksp) of an ionic compound having the general formula MX4 if 5.9x10-14 mol of this compound dissolves in 4.2 mL water at 25 °C? 6.0x10-58 8.1x10-71 2.4x10-62 1.4x10-52 7.5x10-73 b) Mg(OH)2 has Ksp = 1.2 x 10-11 At what minimum pH will a precipitate of Mg(OH)2 form in a solution of 0.23 M Mg(NO3)2? 9.16 5.14 4.84 10.28 8.86

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 4P: Figure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If...

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