Concept explainers
Interpretation:
The amount of calcium oxalate that dissolves in
Concept introduction:
Solubility product is the product of concentrations of ions raised to the power of their
Answer to Problem 67E
The amount of calcium oxalate that will dissolve in
Explanation of Solution
The equilibrium equation for calcium oxalate is shown below.
The solubility product constant for calcium oxalate is calculated by the formula shown below.
Where,
•
•
The given value of
The equilibrium equation for sodium oxalate is shown below.
In the above reaction, the concentration of
Substitute the values of
The concentration of
According to the equilibrium equation for calcium oxalate shown above, the concentration of
The molar mass of
The volume of the solution is
The conversion of
So, the conversion of
The volume of the solution is
The number of moles of solute is calculated as shown below.
The molarity of the solution is calculated as shown below.
Substitute equation (2) in equation (3) as shown below.
Substitute the values of molarity, molar mass and volume of solution in above equation as shown below.
Therefore, the mass of the solute is calculated as shown below.
The amount of calcium oxalate required is
Want to see more full solutions like this?
Chapter 18 Solutions
Introductory Chemistry: An Active Learning Approach
- How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.arrow_forwardWrite the ionic equation for the dissolution and the Ksp expression for each of the following slightly soluble ionic compounds: (a) LaF3. (b) CaCO3. (c) Ag2SO4. (d) Pb(OH)2arrow_forwardSolid sodium fluoride is slowly added to an aqueous solution that contains 0.0100-M Pb2+ and 0.0100-M Ca2+. (a) Determine which precipitates first, calcium fluoride or lead(II) fluoride. (b) Calculate the percentage of Ca2+ or Pb2+ that has precipitated just prior to the precipitation of the compound that precipitates second.arrow_forward
- When 5 M ammonia is added to a solution containing Cu(OH)2(s), the precipitate will eventually dissolve in solution. Why? If 5 M HNO3 is then added, the Cu(OH)2 precipitate re-forms. Why? In general, what effect does the ability of a cation to form a complex ion have on the solubility of salts containing that cation?arrow_forwardLead(II) chromate, PbCrO4, was used as a yellow paint pigment (chrome yellow). When a solution is prepared that is 5.0 104 M in lead ion, Pb2, and 5.0 105 M in chromate ion, CrO42, would you expect some of the lead(II) chromate to precipitate?arrow_forwardA solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?arrow_forward
- Calculate the volume of 1.50 M CH3CO2H required to dissolve a precipitate composed of 350 mg each of CaCO3, SrCO3, and BaCO3.arrow_forwardList some salts whose solubility increases as the pH becomes more acidic. What is true about the anions in these salts? List some salts whose solubility remains unaffected by the solution pH. What is true about the anions in these salts?arrow_forwardWrite the Ksp expression for each of these slightly soluble salts: CuBr HgI2 SrSO4arrow_forward
- Calcium nitrate is added to a sodium sulfate solution that is 0.0150 M. (a) At what concentration of Ca2+ does a precipitate first start to form? (b) Enough Ca(NO3)2 is added to make [ Ca2+ ]=0.0075 M. What percentage of the original sulfate ion has precipitated?arrow_forwardThe Ksp for lead iodide (PbI2) is 1.4 108. Calculate the solubility of lead iodide in each of the following. a. water b. 0.10 M Pb(NO3)2 c. 0.010 M NaIarrow_forwardA 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning