Determine the molar solubility for Srs(PO.): (Ksp = 1.0 × 10-3"). 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. Sr:(PO.):(s) 3 Sr (aq) 2 PO. (aq) Initial (M) Change (M) Equilibrium (M) RESET 3.0 x 10 -1.0 x 10 2.0 x 10 20 x 10* 3.0 x 10 01 1.0 x 10* -31 1.0 x 10+x 1.0 x 10-x -2x +2x 3.0x 10+ 3x 3.0 x 10-3x 20x 10 2x 20x 10-2x

Determine the molar solubility for Srs(PO.): (Ksp = 1.0 × 10-3"). 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. Sr:(PO.):(s) 3 Sr (aq) 2 PO. (aq) Initial (M) Change (M) Equilibrium (M) RESET 3.0 x 10 -1.0 x 10 2.0 x 10 20 x 10* 3.0 x 10 01 1.0 x 10* -31 1.0 x 10+x 1.0 x 10-x -2x +2x 3.0x 10+ 3x 3.0 x 10-3x 20x 10 2x 20x 10-2x

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.69QE

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To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?
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Determine the molar solubility for Sr,(PO,), (Ksp = 1.0 x 1031). 4/2 1 NEXT > Based on the given values, set up ICE table in order to determine the unknown. Sr,(PO,),(s) 3 Sr* (aq) 2 PO, (aq) + 4 Initial (M) Change (M) Equilibrium (M) 5 RESET 1.0 x 1031 -1.0 x 1031 2.0 x 1031 -2.0х 1031 3.0 x 1031 -3.0 x 1031 - +x +2x +3x -X -2x -3x 1.0 x 1031 + x 1.0 x 1031 - x 2.0 x 1031 + 2x 2.0 x 1031 - 2x 3.0 x 1031 + 3x 3.0 x 1031 - 3x
Determine the molar solubility for Ag:CrO. (Ksp = 1.2 × 10-12). 3 NEXT 2 Based on the given values, set up ICE table in order to determine the unknown. Ag:CrO.(s) 2 Ag (aq) Cr:O.2 (aq) Initial (M) Change (M) Equilibrium (M) O RESET 1.2 x 10 -1.2 x 10 2.4 x 10 -2.4 x 10 2 ++ 0. 1.2 x 10+ 2x 1.2 x 10-2x 24 x 10+x 2.4 x 10- -2x 1.2 x 10-x +2x 1.2 x 10+ I 24 x 10+ 2x 24x 10-2x
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Determine the molar solubility for Cr(OH)s (Ksp = 6.3 × 10-31). 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. Cr(OH):(s) Cr*(aq) З ОН (аq) + Initial (M) Change (M) Equilibrium (M) 2 RESET 6.3 x 1081 -6.3 x 1081 1.89 x 10-90 -1.89 × 100 +x -X +3x -3x 6.3 x 10-31 + x 6.3 x 1031 - x 6.3 x 10-3 + 3x 6.3 x 10- - 3x 1.89 x 100 + x 1.89 x 10- x 1.89 x 10-0 + 3x 1.89 x 100 - 3x
35). Will a precipitate of magnesium fluoride form when 400. mL of 1.5 x 10-3 M MgCl2 are added to 600. mL of 2.5 x 10-3M NaF? (Ksp of MgF2 = 6.9 x 10-9) Calculate Q and explain your answer. (b) Calculate the new concentration of Mg2+ ion. (c) Calculate the new concentration of F– ion. (d) Show the Q expression. (e) Calculate Q. (f) Will a precipitate of magnesium fluoride form?
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