1. (Total 20 pts) Calculate a predominance diagram showing the solubility of Spertiniite - a rare Cu(II) hydroxide mineral, Cu(OH)2(s) - as a function of pH by plotting the logarithm of the concentration of each copper species against pH assuming the solution is in contact with Spertiniite. Consider only the following aqueous species: Cu²+; CuOH+; Cu(OH)2; Cu(OH)3. A. Write the reactions that form the aqueous species from Cu(OH)2(s) and the corresponding equilibrium relations. The equilibrium constants for the formation of the 4 aqueous species listed above are 108.68; K₂ = 100.98; K3 = 10–5; K4 = 10-18.2. (10 pt) B. Write the mass balance equation for the solution. (3 pt) C. Plot the total concentration of the dissolved species in a predominance diagram and indicate on the diagram the regions where the solution is oversaturated and undersaturated with Cu(II). Hint: The diagram can be drawn by hand. (7 pt) K₁ =

1. (Total 20 pts) Calculate a predominance diagram showing the solubility of Spertiniite - a rare Cu(II) hydroxide mineral, Cu(OH)2(s) - as a function of pH by plotting the logarithm of the concentration of each copper species against pH assuming the solution is in contact with Spertiniite. Consider only the following aqueous species: Cu²+; CuOH+; Cu(OH)2; Cu(OH)3. A. Write the reactions that form the aqueous species from Cu(OH)2(s) and the corresponding equilibrium relations. The equilibrium constants for the formation of the 4 aqueous species listed above are 108.68; K₂ = 100.98; K3 = 10–5; K4 = 10-18.2. (10 pt) B. Write the mass balance equation for the solution. (3 pt) C. Plot the total concentration of the dissolved species in a predominance diagram and indicate on the diagram the regions where the solution is oversaturated and undersaturated with Cu(II). Hint: The diagram can be drawn by hand. (7 pt) K₁ =

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 17E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...

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) 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
A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system called a heterogeneous equilibrium?
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
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 it is not appropriate to neglect the changes in the initial concentrations of the common ions. (a) TICl(s) in 0.025 M TlNO3. (b) BaF2(s) in 0.0313 M KF. (c) MgC2O4 in 2.250 L of a solution containing 8.156 g of Mg(NO3)2. (d) Ca(OH)2(s) in an unbuffered solution initially with a pH of 12.700
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
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?