Concept explainers
(a)
Interpretation:
It should be shown that
Concept introduction:
Solubility product constant,
(b)
Interpretation:
The buffer component that should be increased in concentration and the minimum value to ensure the beginning of precipitation of MnS should be determined.
Concept introduction:
The pH of a buffer system can be determined by Henderson-Hasselbalch equation as follows:
Here,
Want to see the full answer?
Check out a sample textbook solutionChapter 18 Solutions
Mastering Chemistry With Pearson Etext -- Standalone Access Card -- For General Chemistry: Principles And Modern Applications (11th Edition)
- Consider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions. Predict the effect on each equilibrium if a saturated solution of sodium iodide were added. Explain your prediction in each case. AgI(s) ⇌ Ag+(aq) + I−(aq) PbI2(s) ⇌ Pb2+(aq) + 2 I−(aq)arrow_forwardA solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.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
- A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?arrow_forwardHow 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_forwardAssuming 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 11.45arrow_forward
- 6. CaF2 (s) ⇌ Ca2+ (aq) + 2 F- (aq) Dissolution of the slightly soluble salt Calcium Fluoride is shown by the equation above. Which of the following changes will increase [Ca2+] in a saturated solution of Calcium Fluoride, and why? (assume that after each change some Calcium Fluoride (s) remains in contact with the solution) a)Allowing some of the water to evaporate from the solution, because more Calcium Fluoride (s) will precipitate. b) Adding 1.0 M HNO3 (aq), because some F- (aq) ions will become protonated. c) Adding 0.1 M NaNO3 (aq), because additional liquid will dilute the solution. d) Adding NaF (s), because the reaction will proceed toward reactants.arrow_forwardcalculate the molar solubility of AgBr in 3.1×10−2 M AgNO3 solution. Ksp = 5.0x10-13 for AgBrarrow_forwardUse values of Ksp for AgI and Kf for Ag(CN)2- to determine the molar solubility of AgI in a 0.100 M NaCN solution.arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning