Consider a saturated solution of calcium oxalate, CaC204, in which the following equilibrium canoccur:CaC204(s) = Ca2* (aq) + C204²- (aq)Ksp = 1.3 x 10-8C20,2 (aq) + H2O (1) = HC204 (aq) + OH (aq)HC204 (aq) + H20 (I) = H2C204 (aq) + OH- (aq)If the pH is fixed at 2.30 (then charge balance becomes invalid), find the concentration ofCa2+ in the solution. Assume y =1 for all species.Къ1 1.8 х 10-10K62 = 1.8 x 10-130.090 MO 1.3 x 10-8 M| 99.1 ppmO 1.14 x 10-3 MO 1.8 x 10-6 M

Solubility product: It is defined as the product of its dissolved ion concentrations raised to the…

Consider a saturated solution of calcium oxalate, CaC2O4, in which the following equilibrium can occur: CaC2O4(s) = Ca²* (aq) + C20,²- (aq) Ksp = 1.3 x 10-8 C20,2- (aq) + H20 (1) = HC204 (aq) + OH- (aq) HC204 (aq) + H20 (1) 2 H2C204 (aq) + OH- (aq) If the pH is fixed at 2.30 (then charge balance becomes invalid), find the concentration of Ca2+ in the solution. Assume y =1 for all species. Къ 1.8 х 10-10 Kb2 = 1.8 x 10-13 | 0.090 M O 1.3 x 10-8 M | 99.1 ppm O1.14 x 10-3 M 1.8 x 10-6 M

Consider a saturated solution of calcium oxalate, CaC2O4, in which the following equilibrium can occur: CaC2O4(s) = Ca²* (aq) + C20,²- (aq) Ksp = 1.3 x 10-8 C20,2- (aq) + H20 (1) = HC204 (aq) + OH- (aq) HC204 (aq) + H20 (1) 2 H2C204 (aq) + OH- (aq) If the pH is fixed at 2.30 (then charge balance becomes invalid), find the concentration of Ca2+ in the solution. Assume y =1 for all species. Къ 1.8 х 10-10 Kb2 = 1.8 x 10-13 | 0.090 M O 1.3 x 10-8 M | 99.1 ppm O1.14 x 10-3 M 1.8 x 10-6 M

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Consider a saturated solution of calcium oxalate, CaC204, in which the following equilibrium can
occur:
CaC204(s) = Ca2* (aq) + C204²- (aq)
Ksp = 1.3 x 10-8
C20,2 (aq) + H2O (1) = HC204 (aq) + OH (aq)
HC204 (aq) + H20 (I) = H2C204 (aq) + OH- (aq)
If the pH is fixed at 2.30 (then charge balance becomes invalid), find the concentration of
Ca2+ in the solution. Assume y =1 for all species.
Къ1 1.8 х 10-10
K62 = 1.8 x 10-13
0.090 M
O 1.3 x 10-8 M
| 99.1 ppm
O 1.14 x 10-3 M
O 1.8 x 10-6 M

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