Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 15, Problem 71QAP
Consider the equilibrium curve for AgCl shown below.
Which of the following statements about a solution at point A on the curve are true?
(a) The solution is saturated and at equilibrium.
(b) Addition of NaCl increases the concentration of Cl- in solution.
(c) Addition of NaCl increases the concentration of in solution.
(d) Addition of Ag+ results in the precipitation of AgCl.
(e) Addition of solid NaNO3 to the solution without change in volume does not change [Ag+] or [Cl-].
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
You have a test tube in which the following equilibrium is established.
Fe* (aq) + SCN (aq) = FESCN* (ag)
Describe how concentrations of Fe*, SCN and FeSCN* will change if a crystal KSCN
is added to the mixture above? What would stay constant?
How would the addition of a few drops of a NaOH solution affect the equilibrium in system (B)?
HC2H3O2(ag)=H+(ag) + C2H3O2- (ag)
O No effect will be observed.
The hydroxide would neutralize the H+ ions present and shift the equilibrium to the left.
O The hydroxide would neutralize the H+ ions present and shift the equilibrium to the right.
Write the ionic equation for the dissolution and the solubility product expression for each of the following slightly soluble ionic compounds:(a) AgI, silver iodide, a solid with antiseptic properties(b) CaCO3, calcium carbonate, the active ingredient in many over-the-counter chewable antacids(c) Mg(OH)2, magnesium hydroxide, the active ingredient in Milk of Magnesia(d) Mg(NH4)PO4, magnesium ammonium phosphate, an essentially insoluble substance used in tests for magnesium(e) Ca5(PO4)3OH, the mineral apatite, a source of phosphate for fertilizers
Chapter 15 Solutions
Chemistry: Principles and Reactions
Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Calculate K for the reactions in Question 1.Ch. 15 - Calculate K for the reactions in Question 2.Ch. 15 - Calculate K for the reactions in Question 3.Ch. 15 - Calculate K for the reactions in Question 4.Ch. 15 - Calculate [H+] and pH in a solution in which...Ch. 15 - Calculate [OH-] and pH in a solution in which the...
Ch. 15 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 15 - Prob. 12QAPCh. 15 - A buffer solution is prepared by adding 15.00 g of...Ch. 15 - A buffer solution is prepared by adding 5.50 g of...Ch. 15 - A solution with a pH of 9.22 is prepared by adding...Ch. 15 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Copper(l) chloride, CuCl, is the starting material...Ch. 15 - Prob. 22QAPCh. 15 - Prob. 23QAPCh. 15 - Ksp for CaSO4 at 100C is estimated to be1.6105. At...Ch. 15 - Prob. 25QAPCh. 15 - At 25C, 10.24 mg of Cr(OH)2 are dissolved in...Ch. 15 - Calcium nitrate is added to a sodium sulfate...Ch. 15 - Cadmium(ll) chloride is added to a solution of...Ch. 15 - Water from a well is found to contain 3.0 mg of...Ch. 15 - Silver(I) sulfate (Ksp=1.2105) is used in the...Ch. 15 - A solution is prepared by mixing 13.00 mL of...Ch. 15 - A solution is prepared by mixing 45.00 mL of 0.022...Ch. 15 - A solution is 0.047 M in both NaF and Na2CO3....Ch. 15 - Solid lead nitrate is added to a solution that is...Ch. 15 - A solution is made up by adding 0.632 g of barium...Ch. 15 - A solution is made up by adding 0.839 g of...Ch. 15 - Prob. 37QAPCh. 15 - To a beaker with 500 mL of water are added 95 mg...Ch. 15 - Write net ionic equations for the reaction of H+...Ch. 15 - Prob. 40QAPCh. 15 - Prob. 41QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 43QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 45QAPCh. 15 - Write an overall net ionic equation and calculate...Ch. 15 - Consider the reaction...Ch. 15 - Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2...Ch. 15 - Aluminum hydroxide reacts with an excess of...Ch. 15 - Prob. 50QAPCh. 15 - Calculate the molar solubility of gold(I) chloride...Ch. 15 - Calculate the molar solubility of PbCl2 in 0.2 M...Ch. 15 - For the reaction...Ch. 15 - For the reaction Zn(OH)2(s)+2OH(aq)Zn(OH)42(aq)...Ch. 15 - What are the concentrations of Cu2+, NH3, and...Ch. 15 - Prob. 56QAPCh. 15 - Calcium ions in blood trigger clotting. To prevent...Ch. 15 - Prob. 58QAPCh. 15 - A town adds 2.0 ppm of F- ion to fluoridate its...Ch. 15 - Consider the following hypothetical dissociation:...Ch. 15 - Prob. 61QAPCh. 15 - Consider a 2.0-L aqueous solution of 4.17 M NH3,...Ch. 15 - Marble is almost pure CaCO3. Acid rain has a...Ch. 15 - Prob. 64QAPCh. 15 - Prob. 65QAPCh. 15 - The box below represents one liter of a saturated...Ch. 15 - Consider a saturated solution of BaCO3 at 7.5C....Ch. 15 - Prob. 68QAPCh. 15 - Consider the insoluble salts JQ, K2R, L2S3, MT2,...Ch. 15 - Prob. 70QAPCh. 15 - Consider the equilibrium curve for AgCl shown...Ch. 15 - Dissolving CaCO3 is an endothermic reaction. The...Ch. 15 - Challenge Problems Insoluble hydroxides such as...Ch. 15 - What is the solubility of CaF2 in a buffer...Ch. 15 - What is [Br-] just as AgCl begins to precipitate...Ch. 15 - Prob. 76QAPCh. 15 - Prob. 77QAPCh. 15 - Prob. 78QAP
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
- A small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved salt may or may not be attained. Explain.arrow_forwardAlthough silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.arrow_forwardDiscuss how the concentration of Ca2+ ions, that are in equilibrium with calcitechanges upon changing the following parameters.(a) temperature(b) pressure(c) ph(d)Partial pressure of O2(e)Partial pressure of CO2arrow_forward
- 4. The value of the solubility product, K for calcium hydroxide, Ca(OH), is 5.5 x 10, at25"C. (a) Write the K expression for calcium hydroxide. (b) What is the mass of Ca(OH), in 500 ml of a saturated solution at 25°C? (c) What is the pH of the solution in (b)? (d) If 1.0 mole of OH Is added to the solution in (b), what will be the resulting Ca concentration? Assume that the volume of the solution does not change.arrow_forward(4) A solution is made of a mixture of 0.500 M Calcium chloride and 0.0100 M iron (II) nitrate. The two metals are to be separated by precipitation by increasing the pH. (a) At what pH will the first metal begin to precipitate? (b) At what pH will 99.9% of the first metal be precipitated? (c) At what pH will the second metal begin to precipitate? (d) Can the metals be separated successfully?arrow_forwardWhat is the effect on the amount of solid Mg(OH)2 that dissolves and the concentrations of Mg2+ and OH− when each of the following are added to a mixture of solid Mg(OH)2 and water at equilibrium? (a) MgCl2 Applying Le Châtelier's principle, we can predict that the amount of solid Mg(OH)2 that dissolves will ---Select---increase, decrease, remain unchanged, the [Mg2+ ] will ---Select---increase, decrease, remain unchanged, and the [OH− ] will ---Select--- increase, decrease, remain unchanged. (b) KOH Applying Le Châtelier's principle, we can predict that the amount of solid Mg(OH)2 that dissolves will ---Select---increase, decrease, remain unchanged , the [Mg2+ ] will ---Select--- increase, decrease, remain unchanged , and the [OH− ] will ---Select--- increase, decrease, remain unchanged . (c) HClO4 Applying Le Châtelier's principle, we can predict that the amount of solid Mg(OH)2 that dissolves will ---Select--- increase, decrease, remain unchanged , the [Mg2+ ] will…arrow_forward
- (a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?arrow_forwardWhat is the effect on the amount of solid Mg(OH)2 that dissolves and the concentrations of Mg2+ and OH– when each of the following are added to a mixture of solid Mg(OH)2 in water at equilibrium?(a) MgCl2(b) KOH(c) an acid(d) NaNO3(e) Mg(OH)2arrow_forwardExplain why we can simplify the calculations for K when the value of K is very small (less 4.1 than -10*). 4.2 HCN will react very slightly with water with a K = 6.2 x 10-10. HCN(aq) + H,O() H,O* (aq) and CN" (aq) A chemist starts with a 0.50 M HCN solution. What is the equilibrium concentration of H;O*?. Then use the concentration of H3O* to calculate the pH of the solution with the equation pH = -log[H3O*] (you can do this!!!). Put your final answers in the box. If you need more space to show your work, you can use the backside of this page. [H;O'] at equilibrium pH = -log(H,O] pH = % of HCN that reactedarrow_forward
- Complete the following solubility constant expression for Fe(OH)2.arrow_forwardThe solubility product of MgF, is 10-8.2 (A) What is the solubility of Mg²* at equilibrium with MgF2? (B) If MgF2 is dissolved in a solution of 0.011-molar F¯, how much will dissolve at equilibrium?arrow_forwardCalculate the equilibrium molar concentrations of trichloroacetic acid in an aqueous solution that contains 284.9 mg of trichloroacetic acid,Cl3CCOOH (163.4 g/mol), in 15 mL (the acid is 73.0% ionized in water). Indicate unitsarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY