Concept explainers
(a)
Interpretation:
The possibility of precipitate formation should be explained, when mixing of
Concept Introduction:
Solubility product constant:
The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.
The equilibrium constant of more soluble ionic compound is given by
Ion product:
The multiplication of concentrations power of number of ion each ions in the formula to give the ion product.
Precipitation occurs that solution is supersaturated if
Precipitation will not occurs that solution is saturated and in equilibrium if
Precipitation will not occurs that solution is unsaturated if
(b)
Interpretation:
The possibility of precipitate formation should be explained, when mixing of
Concept Introduction:
Solubility product constant:
The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.
The equilibrium constant of more soluble ionic compound is given by
Ion product:
The multiplication of concentrations power of number of ion each ions in the formula to give the ion product.
Precipitation occurs that solution is supersaturated if
Precipitation will not occurs that solution is saturated and in equilibrium if
Precipitation will not occurs that solution is unsaturated if
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
General Chemistry: Atoms First
- Lead(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_forwardLead sulfate PbSO4, was used as a white paint pigment. When a solution is prepared that is 5.0 103 M in lead ion, Pb2+, and 1.0 104 M in sulfate ion, SO42, would you expect some of the lead sulfate to precipitate?arrow_forwardWill a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?arrow_forward
- You have 95 mL of a solution that has a lead(II) concentration of 0.0012 M. Will PbCl2 precipitate when 1.20 g of solid NaCl is added?arrow_forwardTo a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be • no precipitate? • a precipitate of BaCO3 only? • a precipitate of CaCO3 only? • a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.arrow_forwardA solution is prepared by mixing 45.00 mL of 0.022 M AgNO3 with 13.00 mL of 0.0014 M Na2CO3. Assume that volumes are additive. (a) Will precipitation occur? (b) Calculate [Ag+], [CO32-], [Na+], and [NO3-] after equilibrium is established.arrow_forward
- 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_forwardA solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?arrow_forwardCalculate the solubility (in grams per liter) of magnesium hydroxide in the following. (a) pure water (b) 0.041 M Ba(OH)2 (c) 0.0050 M MgCl2arrow_forward
- How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?arrow_forwardWhat must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4, from a solution that is 0.0034 M Sr2+?arrow_forwardA 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?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning