Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 13, Problem 74APP
For each of the following slightly soluble ionic compounds, write the equilibrium equation for dissociation and the solubility product expression:
a.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
6.1 The solubility of aluminum hydroxide (Al(OH)3) is approximately 1.8 x 10-9
Mat a specific temperature. Calculate the solubility product constant (Ksp) for
aluminum hydroxide at this temperature.
Qa.
none of these
O b. 2.8 x 10^-34
O c. 3.0 x 10^-34
O d. 2.3 x 10^-26
O e. 3.2 x 10^-18
O f. 1.3 x 10^-17
O g. 1.0 x 10^-35
Clear my choice
6.2 A plot of In K vis 1/T gives a slope of -3186 K and an intercept of -18.3.
Calculate the value of delta H in kJ/mol. (Give 3 digits of the calculator answer)
none of these
a.
Ob. 383 kJ/mol
Oc. -38.4 kJ/mol
Od. 192 kJ/mol
-2.20 kJ/mol
Oe.
Of. -152 kJ/mol
g. 26.5 kJ/mol
Clear my choice
MacBook Air
a) Describe any example of systems involving two (or more) simultaneous chemical equilibria.
b) Write the ionic equation for the dissolution and the solubility product for each of the following
slightly soluble compounds:
BaSO
1.
11.
III.
IV.
Ag SO
Al(OH),
Pb(OH)CI
Write the equilibrium constant expression, Kc, for the following reactions. Indicate also if the equilibrium is homogeneous or heterogeneous. (ONLY 7 AND 8) COMPLETE SOLUTION
Chapter 13 Solutions
Basic Chemistry
Ch. 13.1 - Prob. 1PPCh. 13.1 - Prob. 2PPCh. 13.1 - In the following reaction, what happens to the...Ch. 13.1 - Prob. 4PPCh. 13.1 - Prob. 5PPCh. 13.1 - Prob. 6PPCh. 13.2 - What is meant by the term reversible reaction?Ch. 13.2 - Prob. 8PPCh. 13.2 - Which of the following are at equilibrium? a. The...Ch. 13.2 - Which of the following are not at equilibrium? a....
Ch. 13.2 - 13.11 The following diagrams show the chemical...Ch. 13.2 - Prob. 12PPCh. 13.3 - Write the equilibrium expression for each of the...Ch. 13.3 - Prob. 14PPCh. 13.3 - Prob. 15PPCh. 13.3 - Prob. 16PPCh. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - Prob. 21PPCh. 13.3 - Identify each of the following as a homogeneous or...Ch. 13.3 - Prob. 23PPCh. 13.3 - Prob. 24PPCh. 13.3 - Prob. 25PPCh. 13.3 - What is the numerical value of Kc for the...Ch. 13.4 - Prob. 27PPCh. 13.4 - Prob. 28PPCh. 13.4 - Indicate whether each of the following equilibrium...Ch. 13.4 - Indicale whether each of the following equilibrium...Ch. 13.4 - Prob. 31PPCh. 13.4 - The numerical value of the equilibrium constant,...Ch. 13.4 - Prob. 33PPCh. 13.4 - The numerical value of the equilibrium constant,...Ch. 13.5 - In the lower atmosphere, oxygen is converted to...Ch. 13.5 - Prob. 36PPCh. 13.5 - Hydrogen chloride can be made by reacting hydrogen...Ch. 13.5 - When heated, carbon monoxide reacts with water to...Ch. 13.5 - Use the following equation for the equilibrium of...Ch. 13.5 - Use the following equation for the equilibrium of...Ch. 13.5 - Prob. 41PPCh. 13.5 - Prob. 42PPCh. 13.6 - For each of the following slightly soluble ionic...Ch. 13.6 - For each of the following slightly soluble ionic...Ch. 13.6 - Prob. 45PPCh. 13.6 - Prob. 46PPCh. 13.6 - A saturated solution of silver carbonate, Ag2CO3 ,...Ch. 13.6 - Prob. 48PPCh. 13.6 - Calculate the molar solubility, S , of CuI if it...Ch. 13.6 - Calculate the molar solubility, S , of SnS if it...Ch. 13.6 - The CO2 level in the atmosphere has increased over...Ch. 13.6 - Prob. 52PPCh. 13 - Write the equilibrium expression for each of the...Ch. 13 - Write the equilibrium expression for each of the...Ch. 13 - Prob. 55UTCCh. 13 - Would the equilibrium constant, Ke , for the...Ch. 13 - Prob. 57UTCCh. 13 - Prob. 58UTCCh. 13 - Prob. 59APPCh. 13 - Prob. 60APPCh. 13 - For each of the following reactions, indicate if...Ch. 13 - For each of the following reactions, indicate if...Ch. 13 - Consider the reaction: (13.3) 2NH3(g)N2(g)+3H2(g)...Ch. 13 - Prob. 64APPCh. 13 - Prob. 65APPCh. 13 - Prob. 66APPCh. 13 - Prob. 67APPCh. 13 - According to Le Châtelier's principle, does the...Ch. 13 - Prob. 69APPCh. 13 - Prob. 70APPCh. 13 - The numerical value of the equilibrium constant,...Ch. 13 - The numerical value of the equilibrium constant,...Ch. 13 - For each of the following slightly soluble ionic...Ch. 13 - For each of the following slightly soluble ionic...Ch. 13 - Prob. 75APPCh. 13 - Prob. 76APPCh. 13 - Prob. 77APPCh. 13 - Prob. 78APPCh. 13 - What is the molar solubility, S , of CdS if it has...Ch. 13 - Prob. 80APPCh. 13 - Prob. 81CPCh. 13 - Prob. 82CPCh. 13 - Prob. 83CPCh. 13 - Indicate how each of the following will affect the...Ch. 13 - Prob. 85CPCh. 13 - Prob. 86CPCh. 13 - Prob. 87CPCh. 13 - Prob. 88CP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 9.26 Lead (II) iodide can be produced upon cooling lead (II) and iodide ions from a solution. 21¯(aq) + Pb²+ (aq) = PbI₂ (s) + Heat In which direction will the equilibrium shift (right or left) if the following changes occur to the reaction at equilibrium? a. add iodide (I) b. heat the reaction c. remove lead (II) iodide d. cool the reactionarrow_forward(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) O 0.0958 M O 0.383 M O 0.767 M O 0.192 Marrow_forward15. 16. In a saturated solution of lead (II) chloride, the concentration of chloride ion is 6.2 x 104 mol/L. The Ksp of lead(II) chloride would be which of the following? 17. a. 1.9 x 107 b. 6.0 x 10-¹1 c. 1.2 x 10-10 The following diagram represents a kinetic energy distribution at two temperatures. d. 2.3 x 10-¹7 e. none of the above Number of Molecules with a Particular Kinetic Energy a. T₁ > T₂ b. T₂ > T₁ C. T₁ T₂ Kinetic Energy In comparing the two temperatures, it is obvious that I ₂ d. T₁ = T₂ e. cannot be determined A full syringe contains this equilibrium: 2 NO₂(g) = N₂O4(g) colourless gas brown gas Based on Le Chatelier's principle, what would be observed when the syringe is used to compress this gas mixture? a. the mixture gets darker b. the mixture gets darker then lighter c. the mixture get lighter then darker d. the mixture gets lighter e. none of the abovearrow_forward
- 14.55 Heating solid sodium bicarbonate in a closed vessel establishes the following equilibrium: (15.5) 2NaHCO3(s) = N22CO3(s) + H20(g) + CO2(8) What would happen to the equilibrium position if (a) CO2 gas were added to the system, (b) Na2CO3 were removed from the system, (c) NaHCO3 were removed from the system. The temperature remains constant in each case.arrow_forward9.10) Which of the following processes are at equilibrium? a. opposing rates of reaction are equal b. concentrations of reactants and products are equal c. the concentration of reactants and products do not changearrow_forward6.56 Use each expression for the equilibrium constant to write a chemical equation. 88.D [AB,]² [A,][B,]² [A,B,] illupe 1ot a6. K= w a. K = e erl) wollot [A]°[B]³ %3Barrow_forward
- 14.10 Write the balanced chemical equation for the dissociation of each of the following carboxylic acids in water: CH3 O || a. CH3-CH-C-OH b. butanoic acidarrow_forward8.) Consider the following equilibrated system: 2NO2(g)=2NO(g) + O2(g). If the Kc value is 0.918, find the equilibrium concentration of the O2 gas if the NO2 concentration is 0.520 M and the [NO] is 0.300 M at equilibrium. (2.76 M)arrow_forward8) What is the pH of a solution containing 0.280 M weak base, B', with a K, of 3.9 X 107? (10.51) в (ад) + H-0 (1) ВН (аq) + ОН (ад)arrow_forward
- At high temperatures nitrogen (N2) and oxygen (O2) will react to form NO.N2(g) + O2(g) ⇆ 2 NO(g) (4.1)The value for the equilibrium constant for reaction 4.1 is KC = 2.7 x 10^-17 at some temperature T.A system initially has [N2] = 0.0800 M and [O2] = 0.0500 M. There is no NO initially present inthe system. Find the value for [NO] that will be present at equilibrium.arrow_forward7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s) Sr2 (aq) 2F (aq) 2arrow_forwardA 1 liter vessel established equilibrium with the following reaction, 2 SO2+O2=2SO3, has 0.11 mole SO2,0.05 mole O2 and 0.12 mole SO3. Another 1 liter vessel is used and contains initially 96 g of SO2,how much O2 (in grams) must be added, if at equilibrium, one half of SO2 will be converted to SO3?A. 6.04B. 9.34C. 13.34D. 9.60arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY