The dissolution of ZnCO3 is described by the chemical equation:ZnCO3(s)Zn2+(aq)+CO, (aq)The Ksp expression describing the dissolution of ZnCO3 and its value are:Ksp¸= [Zn²+][CO²¯] = 1.20 ;1.20 × 10-101st attemptWhat is the solubility of ZnCO3 at 25°C in a buffer solution with a pH of 9.350?

Step 1: Formula Determination Step 2: Calculation of [H3O+]pH = 9.350We know that,pH =…

Answered: The dissolution of ZnCO3 is described…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 70QAP: . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method...

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A 0.64 g sample of the white crystalline dimer (4) is dissolved in 25.0 mL of benzene at 20 C. Use the equilibrium constant to calculate the concentrations of monomer (2) and dimer (4) in this solution.
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.
A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 102 atm at 25C. Calculate the Ksp value for the salt, assuming ideal behavior.
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
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?
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
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
Use the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products). (a) TlCl. (b) BaF2. (c) Ag2CrO4. (d) CaC2O4H2O (e) the mineral anglesite, PbSO4
Write the expression of the reaction quotient for the ionization of HOCN in water.
When 1.55 g of solid thallium(I) bromide is added to 1.00 L of water, the salt dissolves to a small extent. TlBr(s)Tl+(aq)+Br(aq) The thallium(I) and bromide ions in equilibrium with TlBr each have a concentration of 1.9 103 M. What is the value of Ksp for TlBr?
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) KHC4H4O6. (b) PbI2. (c) Ag4[Fe(CN)6], a salt containing the Fe(CN)4- ion. (d) Hg2I2

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