At this point, [Cl-] is governed by the Ksp reaction. We can make this a really easy calculation by simply assuming that we are starting from no dissolved Ag+ and Ci", but instead only solid AgCl. We can then calculate what the Ag* and Cl- concentrations are at 10 mL Ksp = 1.8 x 10-10 = [Ag*l[Cl¯] You have solved this kind of problem many times now. Do it again for [Cl"] for the 10 mL.

At this point, [Cl-] is governed by the Ksp reaction. We can make this a really easy calculation by simply assuming that we are starting from no dissolved Ag+ and Ci", but instead only solid AgCl. We can then calculate what the Ag* and Cl- concentrations are at 10 mL Ksp = 1.8 x 10-10 = [Ag*l[Cl¯] You have solved this kind of problem many times now. Do it again for [Cl"] for the 10 mL.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.BCP

See similar textbooks

Similar questions

Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of Al(OH)3(s) in very acidic solutions and in very basic solutions. b. Lets study the pH dependence of the solubility of Al(OH)3(s) in more detail. Show that the solubility of Al(OH)3, as a function of [H+], obeys the equation S=[H+]3Ksp/Kw3+KKw/[H+] where S = solubility = [Al3+] + [Al(OH)4] and K is the equilibrium constant for Al(OH)3(s)+OH(aq)Al(OH)4(aq) c. The value of K is 40.0 and Ksp for Al(OH)3 is 2 1032. Plot the solubility of Al(OH)3 in the pH range 412.
What concentration of SO is in equilibrium with Ag,SO, (s) and 4.90 x 10-3 M Ag+? The Ksp of Ag, SO, can be found in this table. M [so;] = ?
An experiment was carried out to determine the value of the equilibrium constant, Kc for the reaction. Total moles of Ag+ present= 3.6 x 10 -3 moles Total moles of NH3 present = 6.9 x 10-3 moles Measured concentration of Ag(NH3)2 + at equilibrium = 3.4 x 10-2 M Total solution volume = 100 mL a.)Calculate the equilibrium concentration of Ag+ (uncomplexed) b.)Calculate the equilibrium concentration of NH3 (uncomplexed) c.) Calculate the value of the equilibrium constant
Construct the expression for Ksp for solid A9CN in aqueous solution. AGCN(s) = Ag*(aq) + CN-(aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp RESET [AGCN] 2[A9CN] [A9CNJ? [Ag*] 2[Ag*] [Ag*P [Ag*] 2[Ag*] [Ag*P [CN] 2[CN] [CN-P [CN²] 2[CN ] [CN-1?
38. The organic compound 18-crown-6 (see preceding prob- lem) also binds strongly with the alkali metal ions in methanol. K* + 18-crown-6#[complex]* In methanol solution the equilibrium constant is 1.41 x 10. A similar reaction with Cst has an equilibrium con- stant of only 2.75 x 104. A solution is made (in methanol) containing 0.020 mol L each of K* and Cs*. It also contains 0.30 mol L' of 18-crown-6. Compute the equi- librium concentrations of both the uncomplexed K* and the uncomplexed Cs*.
Zn│Zn2+ (1.0 M)║Cu2+ (0.10 M)│Cu Ecell measurement .698 Reaction quotient, Ecell calculation
10a. Calculate the Ecell for the reaction Fe3+ Cr2 -----> Fe+2+ Crt3, when (Fe+3) = (Cr+2) = 1.50 x 10-³ M and (Fe+2) = Cr+3) = 2.5 x 10-4 M
0.1 gram of solid aluminum phosphate (Al(PO:) (s) is added to 500 L of pure water. Immediately the solid begins to dissolve according to the reactions below. Complete dissolution: Al(PO,) (s) → Al + PO, No K Solid present: Al(PO.) (s) + Al + PO, Ksp = 1012 %3D What is the concentration of dissolved phosphate (in M and mg/L) in the water once all reactions proceed to completion? Is the solid still present or has it completely dissolved? Why or why not? If the solid is present, calculate the solid concentration (in M and mg/L). Develop a plot showing the aqueous (dissolved) concentration of PO; (in M) on the Y-axis versus different AI(PO,)(5) additions (in M) on the X-axis. Include the critical point that separates whether the solid is completely dissolved or is still present and label your plot appropriately.
The Ksp of Cu3 (PO4), is 1.00 × 10-37. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of K3PO4 , how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
Construct the expression for Ksp for solid AgCN in aqueous solution. AgCN(s) Ag+ (aq) + CN- (aq) Based on your knowledge of how the solid will dissociate in aqueous solution, construct the expression for the solubility constant, Ksp. Each reaction participant must be represented by one tile. [AgCN] [Ag²+]² 2[AgCN] [CN-] Ksp [AgCN]² 2[CN-] = [Ag+] 1 [CN-12 2[Ag+] [CN²-] [Ag+]² 2[CN²-] [Ag²+] [CN²-1² RES 2[Ag²+]
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca? + (aq) and 0.0340 M Ag+(aq). What will be the concentration of Ca² + (aq) when Ag, SO, (s) begins to precipitate? Solubility-product constants, Ksp, can be found in the chempendix. |Ca**] = M What percentage of the Ca? + (aq) can be precipitated from the Ag*(aq) by selective precipitation? percentage: %
Cineplex Entertain.. E MLA Citation Make... XERCISE Writing Equilibrium Constant Expressions I [References) Fe(s) +5 CO(g) 2Fe(CO),(g) [Fe] [CO] [Fe(CO);] 1 K.= 1 Build the equilibrium constant expression for the reaction shown. Step 1. Drag the reactants and products to the numerator or denominator as appropriate. Click a species to remove it from the expression. Step 2. Drag the coefficients to the appropriate species. Click a coefficient to remove it from the expression. Recheck (3 of 8) 27th attempt Incorrect A correct equilibrium constant expression follows the form "products" over "reactants," where each species is raised to the power of its stoichiometric Solids and pure liquids are not included in the equilibrium expression. Show Hint