It was found that an equilibrium solution contained 3.00 x 10-4 M Fe3+ (3.00 times10 to the minus 4th power MFe 3+), 3.00 x 10-4 M SCN (3.00 times 10 to theminus 4th power M SCN minus) and 5.00 x 105 M FESCN2+ (5.00 times 10 to theminus 5th power M Fe SCN 2+ ). What is K, for this solution?C0.00005009.00 x 10* (9.00 times 10 to the minus 9th power)0.00234) 0.000300O 556O 0.00180O750.身

Equilibrium constant Kc is the ratio of multiplication of concentration of product to…

Answered: It was found that an equilibrium…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 95QRT

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Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) AgCl(s) in 0.025 M NaCl. (b) CaF2(s) in 0.00133 M KF. (c) Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4. (d) Zn(OH)2(s) in a solution buffered at a pH of 11.45
Calculate the equilibrium concentrations of NH3, Cu2+, Cu(NH3)2+, Cu(NH3)22+, Cu(NH3)32+, and Cu(NH3)42+ in a solution prepared by mixing 500.0 mL of 3.00 M NH3 with 500.0 mL of 2.00 103 M Cu(NO3)2. The stepwise equilibria are Cu2+(aq)+NH3(aq)CuNH32+(aq)K1=1.86104CuNH32+(aq)+NH3(aq)Cu(NH3)22+(aq)K2=3.88103Cu(NH3)22+(aq)+NH3(aq)Cu(NH3)32+(aq)K3=1.00103Cu(NH3)22+(aq)+NH3(aq)Cu(NH3)42+(aq)K4=1.55102
A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?
A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the resulting solution. [Ksp for AgIO3(s) = 3.17 108.]
Suppose that solid AgCl and AgI are placed in 1.0 L water in separate beakers. Some, but not all, of each solid compound dissolves. In which beaker is the silver ion concentration, [Ag+], larger? Does the volume of water in which each compound dissolves affect the equilibrium concentration?
In the presence of CN, Fe3+ forms the complex ion Fe(CN)63. The equilibrium concentrations of Fe3+ and Fe(CN)63 are 8.5 1040 M and 1.5 103 M, respectively, in a 0.11-M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63. Fe3+(aq)+6CN(aq)Fe(CN)63(aq)Koverall=?
Consider the equilibrium curve for AgCl shown below. Which of the following statements about a solution at point A on the curve are true? (a) The solution is saturated and at equilibrium. (b) Addition of NaCl increases the concentration of Cl- in solution. (c) Addition of NaCl increases the concentration of in solution. (d) Addition of Ag+ results in the precipitation of AgCl. (e) Addition of solid NaNO3 to the solution without change in volume does not change [Ag+] or [Cl-].
A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.

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