Determine the concentrations of Pb2+ and I− in a saturated solution of PbI2 (Ksp for PbI2 is 1.4 × 10−8.)
(a) 0.0015 M and 0.0030 M
(b) 0.0015 M and 0.0015 M
(c) 0.0015 M and 0.00075 M
(d) 0.0019 M and 0.0019 M
(e) 0.0019 M and 0.0038 M
Interpretation:
The concentrations values for the given ions should be determined using the given solubility product value.
Concept Introduction:
Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If K value is less than one then the respective reaction will move to the left side and if K value is higher (or) greater than one then respective reaction will move to the right side of reaction.
Solubility product: It is used to express the concentration of dissolved ions whose stoichiometric coefficients are raised to power of it. It expresses the equilibrium between solids and its respective ions in the solution.
Answer to Problem 15.2KSP
The concentration values for
Explanation of Solution
Reason for correct option:
The general chemical equation that represents the given conditions is as follows,
Given,
The solubility product for
Considering the given reaction we set up (ICE) equilibrium table as follows,
The concentration for
Therefore, the value for x was determined and the concentration of
Hence, the correct option is option (a).
Reason for in-correct options:
Consider all options other than the correct one.
These options show us that they do not contain the correct value which is obtained from the calculation using solubility product formula and the ice table for the given chemical reaction.
Hence, the incorrect options are option (b), (c) (d)and (e).
The correct option that contains the concentration values for the given reaction was determined by using solubility product formula.
Want to see more full solutions like this?
Chapter 15 Solutions
Chemistry: Atoms First
- Draw a nanoscale (particulate) level diagram for an equilibrium mixture ofarrow_forwardA sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answerarrow_forwardWrite the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)arrow_forward
- Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g)C2H6CO(g)+H2(g)At 180C, the equilibrium constant for the decomposition is 0.45. If 20.0 mL (d=0.785g/mL) of isopropyl alcohol is placed in a 5.00-L vessel and heated to 180C, what percent- age remains undissociated at equilibrium?arrow_forwardAt a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forwardThe density of trifluoroacetic acid vapor was determined at 118.1 C and 468.5 torr, and found to be 2.784 g/L. Calculate KC for the association of the acid.arrow_forward
- Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at 25C are 10.0 g of NH4HS, ammonia with a partial pressure of 0.692 atm, and H2S with a partial pressure of 0.0532 atm. When equilibrium is established, it is found that the partial pressure of ammonia has increased by 12.4%. Calculate K for the decomposition of NH4HS at 25C.arrow_forwardSolid CaCO3 ; is placed in a closed container and heated to 800 °C. What is the equilibrium concentration of Co2 in the following equilibrium, for which K=2.5103 ? CaCO3(s)CaO(s)+Co2(g)arrow_forwardAt 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)arrow_forward
- Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.arrow_forwardFor the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?arrow_forwardPhosgene, COCl2, used in the manufacture of polyurethane plastics, is prepared from CO and Cl2. CO(g)+Cl2(g)COCl2(g) An equilibrium mixture at 395C contains 0.012 mol CO and 0.025 mol Cl2 per liter, as well as COCl2 If Kc at 395C is 1.23 103, what is the concentration of COCl2?arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning