Consider a saturated solution of AgBr in 0.010 M NH3.AgBr (s) 5 Ag* + BrAg* + NH3 (aq) 5 Ag(NH3)*Ag(NH3)* + NH3 (aq) 5 Ag(NH3)2* KrKsp = 5.0 x10-13Kf = 2.04 x10³8.13 x103NH3+ H2O 5 NH4* + OH-Kb = 1.75 x105(aq)H2O S H* + OH¯Kw = 1.00 x10-14a. How many unknown concentrations must be solved? How many equations are required?b. Write a charge balance equation for the system.c. Write a mass balance equation for the system.

Consider a saturated solution of AgBr in 0.010 M NH3. AgBr (s) Ag* + NH3 (aq) 5 Ag(NH3)* S Ag* + Br Ksp = 5.0 x10-13 Kf = 2.04 x10³ Ag(NH3)* + NH3 (aq) 5 Ag(NH3)2* K¢ = 8.13 x10³ %3D %3D NH3 (aq) + H2O 5 NH4* + OH- Kb = 1.75 x10$ %3D H2O S H* + OH¯ Kw = 1.00 x10-14 %3D a. How many unknown concentrations must be solved? How many equations are require: b. Write a charge balance equation for the system. Write a mass balance equation for the system.

Consider a saturated solution of AgBr in 0.010 M NH3. AgBr (s) Ag* + NH3 (aq) 5 Ag(NH3)* S Ag* + Br Ksp = 5.0 x10-13 Kf = 2.04 x10³ Ag(NH3)* + NH3 (aq) 5 Ag(NH3)2* K¢ = 8.13 x10³ %3D %3D NH3 (aq) + H2O 5 NH4* + OH- Kb = 1.75 x10$ %3D H2O S H* + OH¯ Kw = 1.00 x10-14 %3D a. How many unknown concentrations must be solved? How many equations are require: b. Write a charge balance equation for the system. Write a mass balance equation for the system.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 3E

See similar textbooks

Similar questions

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
Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12×10−12. What is the solubility (in mol/L) of silver chromate in 1.20 M potassium chromate aqueous solution? What is the solubility (in mol/L) of silver chromate in 1.20 M1.20 M silver nitrate aqueous solution? What is the solubility (in mol/L) of silver chromate in pure water?
Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a) [Ag][PO4] (b) [Ag+][PO43 - ] (c) [Ag+]3[PO43 - ](d) [Ag+[[PO43 - ]3 (e) [Ag+]3[PO43 - ]3
Calculate the solubility (in g/L) of CaSO4(s) in 0.400 M Na2SO4(aq) at 25°C 0.400 M Na2SO4(aq) at 25°C. The Ksp of CaSO4 is 4.93×10−5.
In nature, silver iodide (AgI) is obtained in the form of the mineral iodargyrite. This compound has a bright yellow color and has a melting point of 552 oC. However, in the laboratory this compound can be prepared by heating a solution of silver nitrate (AgNO3) and an alkaline iodide such as potassium iodide (KI).a. What are the effects of the salts KI and AgNO3 on the solubility of AgI in water? Please describe your answer. b. Describe the effect of the salt KNO3 on the solubility of AgI in water. Explain why it’s different from the effects noted in question 9a?
Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103
The molar solubility of Fe(OH)2 at 25 °C is 1.6×10−5. What is Ksp for Fe(OH)2? 1.0×10−9 1.6×10−2 1.6×10−14 4.1×10−15
Calculate the solubility at 25 C of AgCl in pure water and in a 0.0070 M AgNO3 solution. Ksp= 1.77 x 10^-10 AgCl
The solubility of Ag(I) in aqueous solutions containing dif-ferent concentrations of Cl is based on the following equilibria:Ag⁺(aq)+Cl⁻(aq)⇌AgCl(s) Kₛₚ=1.8X10⁻¹⁰ Ag⁺(aq)+2Cl⁻(aq)⇌AgCl₂⁻(s) K(f)=1.8X10⁻⁵ When solid AgCl is shaken with a solution containing Cl⁻, Ag(I)is present as both Ag⁺ and AgCl₂⁻. The solubility of AgCl is thesum of the concentrations of Ag and AgCl₂.(a) Show that [Ag⁺] in solution is given by[Ag⁺]=1.8X10⁻¹⁰/[Cl⁻]and that [AgCl₂⁻] in solution is given by [AgCl₂⁻](3.2X10⁻⁵)([Cl⁻] (b) Find the [Cl⁻] at which [Ag⁺][AgCl₂⁻].(c) Explain the shape of a plot of AgCl solubility vs. [Cl⁻].(d) Find the solubility of AgCl at the [Cl⁻] of part (b), which is the minimum solubility of AgCl in the presence of Cl
Metal sulfides are prepared by bubbling hydrogen sulfide gas, H2S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H2S, which occurs when [H2S]=0.100 M, the equilibrium shown is established. H2S(aq)+2H2O(l)↽−−⇀S2−(aq)+2H3O+(aq)?eq=1.1×10−20 An aqueous solution containing 0.0570 M Pb2+ and 0.0570 M Ag+ is saturated with H2S. Above what concentration of S2− will PbS precipitate? The ?sp of PbS is 8.9×10−29. [S2−]= M Above what concentration of S2− will Ag2S precipitate? The ?sp of Ag2S is 3.3×10−50. [S2−]= M If the pH of the solution is adjusted to 2.83, which species will precipitate from the saturated H2S solution? both PbS and Ag2S neither species PbS Ag2S
Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2 CrO4 is 1.12× 10^(-12). What is the solubility (in mol/L) of silver chromate in 1.40 M potassium chromate aqueous solution? solubility: What is the solubility (in mol/L) of silver chromate in 1.40 M silver nitrate aqueous solution? solubility: What is the solubility (in mol/L) of silver chromate in pure water? solubility:
The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.