Think about this reaction and its equilibrium constant: Ag3PO4(s) = 3 Ag*(aq) + PO43-(aq) K=2.95× 10~15 Suppose 19.6 g of Ag3PO4 is added to 4.8 L of water, creating a saturated solution with some undissolved solid resting on the bottom of the beaker. Calculate the equilibrium concentration of Ag*(aq) in units of millimol/liter, mM. Enter your answer to the third decimal place.

Think about this reaction and its equilibrium constant: Ag3PO4(s) = 3 Ag(aq) + PO43-(aq) K=2.95× 10~15 Suppose 19.6 g of Ag3PO4 is added to 4.8 L of water, creating a saturated solution with some undissolved solid resting on the bottom of the beaker. Calculate the equilibrium concentration of Ag(aq) in units of millimol/liter, mM. Enter your answer to the third decimal place.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 117IP: In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization:...

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In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
Write the expression of the reaction quotient for the ionization of HOCN in water.
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Use the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.