![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_largeCoverImage.gif)
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 16, Problem 106CP
Interpretation Introduction
Interpretation: The concentration of all the species in the given reaction is to be calculated.
Concept introduction: The solubility product is the mathematical product of a substance’s dissolved ion concentration raised to its power of its
Expert Solution & Answer
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Students have asked these similar questions
The equation below represents the equilibrium process of a saturated solution of Ca(OH)2
If the following changes are made to a saturated solution, what will be the effect on the [Ca2+] ?
Ca(OH)2 (s) <--> Ca2+(aq) + 2 OH- (aq) ΔH = -16.6 kJ
More solid Ca(OH)2 is added to the container.
Decrease Increase No Change
Ca(NO3)2 (s) is added. ( Ca(NO3)2 is very soluble)
Decrease Increase No Change
A strong acid is added to the solution
Decrease Increase No Change
A strong base is added to the solution
Decrease Increase No Change
The solution is raised to a higher temperature
Decrease Increase No Change
A 100.0 mL sample of a 0.100 M solution of boric acid (H3BO3) is combined with a 100.0 mL sample of a 0.100 M solution of borate ion (H2BO3–) and the following equilibrium system is established.
H3BO3(aq) + H2O(l) ⇌ H2BO3–(aq) + H3O+(aq)
What change will caused the equilibrium to shift towards the right? Select all that apply.
Addition of HCl
Increasing the pH
Addition of boric acid
Removal of borate ions
Le Châtelier’s Principle is described in terms of adding/removing reactants or products. While it is easy to add reactants/products, describe how we are able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for the reactions in B1, B2, and B3 below?
The following reaction will be studied:Mg(OH)2 (s) ⇌ Mg2+ (aq) + 2 OH¯ (aq)
We start with MgCl2 solution in wells B1, B2, B3, B4, and B5.We use phenolphthalein is an indicator that is colorless in acidic solutions and violet/pink in basic solutions. To well B1 of MgCl2, we add 5 drops of concentrated (0.5 M) NaOH to well B1 (it turns light pink) and then we add a few drops HCl and it becomes clear.
To well B2 of MgCl2, we only add dilute NaOH until it turns pink.
To Well B3 of MgCl2, we add 1-2 drops of dilute NaOH from a dropper bottle to well B3 to get a faint pink solution and then we add 3-5 drops EDTA and solution gets dark pink. EDTA is a…
Chapter 16 Solutions
Chemistry
Ch. 16 - To what reaction does the solubility product...Ch. 16 - Under what circumstances can you compare the...Ch. 16 - What is a common ion and how does its presence...Ch. 16 - List some salts whose solubility increases as the...Ch. 16 - What is the difference between the ion product, Q,...Ch. 16 - Mixtures of metal ions in aqueous solution can...Ch. 16 - Prob. 7RQCh. 16 - What is a complex ion? The stepwise formation...Ch. 16 - When 5 M ammonia is added to a solution containing...Ch. 16 - Figure 15-3 outlines the classic scheme for...
Ch. 16 - Which of the following will affect the total...Ch. 16 - Prob. 2ALQCh. 16 - You are browsing through the Handbook of...Ch. 16 - A friend tells you: The constant Ksp of a salt is...Ch. 16 - Explain the following phenomenon: You have a test...Ch. 16 - What happens to the Ksp value of a solid as the...Ch. 16 - Which is more likely to dissolve in an acidic...Ch. 16 - Two different compounds have about the same molar...Ch. 16 - Sodium chloride is listed in the solubility rules...Ch. 16 - For which of the following is the Ksp value of the...Ch. 16 - Ag2S(s) has a larger molar solubility than CuS...Ch. 16 - Solubility is an equilibrium position, whereas Ksp...Ch. 16 - Prob. 13QCh. 16 - Prob. 14QCh. 16 - The common ion effect for ionic solids (salts) is...Ch. 16 - Sulfide precipitates are generally grouped as...Ch. 16 - List some ways one can increase the solubility of...Ch. 16 - The solubility of PbCl2 increases with an increase...Ch. 16 - You have two salts, AgX and AgY, both with very...Ch. 16 - The stepwise formation constants for a complex ion...Ch. 16 - Silver chloride dissolves readily in 2 M NH3 but...Ch. 16 - If a solution contains either Pb2+(aq) or Ag+(aq),...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Prob. 25ECh. 16 - Use the following data to calculate the Ksp value...Ch. 16 - Approximately 0.14 g nickel(II) hydroxide,...Ch. 16 - The solubility of the ionic compound M2X3, having...Ch. 16 - The concentration of Pb2+ in a solution saturated...Ch. 16 - The concentration of Ag+ in a solution saturated...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Cream of tartar, a common ingredient in cooking,...Ch. 16 - Barium sulfate is a contrast agent for X-ray scans...Ch. 16 - Calculate the molar solubility of Cd(OH)2, Ksp =...Ch. 16 - The solubility rules outlined in Chapter 4 say...Ch. 16 - Calculate the molar solubility of Al(OH)3, Ksp = 2...Ch. 16 - Calculate the molar solubility of Co(OH)3, Ksp =...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - Calculate the solubility (in moles per liter) of...Ch. 16 - Calculate the solubility of Co(OH)2(s) (Ksp = 2.5 ...Ch. 16 - The Ksp for silver sulfate (Ag2SO4) is 1.2 105....Ch. 16 - The Ksp for lead iodide (PbI2) is 1.4 108....Ch. 16 - Calculate the solubility of solid Ca3(PO4)2 (Ksp =...Ch. 16 - Calculate the solubility of solid Pb3(P04)2 (Ksp =...Ch. 16 - Prob. 47ECh. 16 - The solubility of Pb(IO3)(s) in a 0.10-M KIO3...Ch. 16 - Which of the substances in Exercises 27 and 28...Ch. 16 - For which salt in each of the following groups...Ch. 16 - What mass of ZnS (Ksp = 2.5 1022) will dissolve...Ch. 16 - The concentration of Mg2+ in seawater is 0.052 M....Ch. 16 - Will a precipitate form when 100.0 mL of 4.0 104...Ch. 16 - A solution contains 1.0 105 M Ag+ and 2.0 106 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - If 10.0 mL of 2.0 103 M Cr(NO3)3 is added to 10.0...Ch. 16 - Calculate the final concentrations of K+(aq),...Ch. 16 - A solution is prepared by mixing 75.0 mL of 0.020...Ch. 16 - A 50.0-mL sample of 0.00200 M AgNO3 is added to...Ch. 16 - Prob. 60ECh. 16 - A solution contains 1.0 105 M Na3PO4. What is the...Ch. 16 - A solution is 1 104 M in NaF, Na2S, and Na3PO4....Ch. 16 - A solution contains 0.25 M Ni(NO3)2 and 0.25 M...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - In the presence of CN, Fe3+ forms the complex ion...Ch. 16 - In the presence of NH3, Cu2+ forms the complex ion...Ch. 16 - Prob. 69ECh. 16 - Prob. 70ECh. 16 - The overall formation constant for HgI42 is 1.0 ...Ch. 16 - A solution is prepared by adding 0.10 mole of...Ch. 16 - A solution is formed by mixing 50.0 mL of 10.0 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - a. Calculate the molar solubility of AgI in pure...Ch. 16 - Solutions of sodium thiosulfate are used to...Ch. 16 - Kf for the complex ion Ag(NH3)2+ is 1.7 107. Ksp...Ch. 16 - Prob. 78ECh. 16 - Prob. 79ECh. 16 - The solubility of copper(II) hydroxide in water...Ch. 16 - A solution contains 0.018 mole each of I, Br, and...Ch. 16 - Magnesium hydroxide, Mg(OH)2, is the active...Ch. 16 - Tooth enamel is composed of the mineral...Ch. 16 - The U.S. Public Health Service recommends the...Ch. 16 - What mass of Ca(NO3)2 must be added to 1.0 L of a...Ch. 16 - Calculate the mass of manganese hydroxide present...Ch. 16 - Prob. 87AECh. 16 - The active ingredient of Pepto-Bismol is the...Ch. 16 - Consider saturated solutions of die following...Ch. 16 - Silver cyanide (AgCN) is an insoluble sail with...Ch. 16 - Nanotechnology has become an important field, with...Ch. 16 - The equilibrium constant for the following...Ch. 16 - Calculate the concentration of Pb2+ in each of the...Ch. 16 - Will a precipitate of Cd(OH)2 form if 1.0 mL of...Ch. 16 - a. Using the Ksp value for Cu(OH)2 (1.6 1019) and...Ch. 16 - Describe how you could separate the ions in each...Ch. 16 - Nitrate salts are generally considered to be...Ch. 16 - In the chapter discussion of precipitate...Ch. 16 - Assuming that the solubility of Ca3(PO4)2(s) is...Ch. 16 - Order the following solids (ad) from least soluble...Ch. 16 - The Ksp for PbI2(s) 1.4 108. Calculate the...Ch. 16 - The solubility of Pb(IO3)2(s) in a 7.2 102-M KIO3...Ch. 16 - A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to...Ch. 16 - Prob. 105CPCh. 16 - Prob. 106CPCh. 16 - a. Calculate the molar solubility of AgBr in pure...Ch. 16 - Calculate the equilibrium concentrations of NH3,...Ch. 16 - Calculate the solubility of AgCN(s) (Ksp = 2.2 ...Ch. 16 - Calcium oxalate (CaC2O4) is relatively insoluble...Ch. 16 - The salt MX has a solubility of 3.17 108 mol/L in...Ch. 16 - Consider 1.0 L of an aqueous solution that...Ch. 16 - A solution saturated with a salt of the type M3X2...Ch. 16 - What mass of Ca(NO3O)2 must be added to 1.0 L of a...Ch. 16 - The Ksp for Q, a slightly soluble ionic compound...Ch. 16 - Aluminium ions react with the hydroxide ion to...
Knowledge Booster
Similar questions
- Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.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_forwardIn a lab experiment, a student manages to dissolve 0.0240 moles of a mysterious compound AB2 into 1 L of water. The mysterious compound dissociates using the following equation: AB2(S) ⇌ A(aq) + 2B(aq) What is the value of the Ksp for this compound? (Please provide your answer to 3 significant figures in scientific notation such as 1.23*10^-5)arrow_forward
- please,don't provied handwriting solution.arrow_forwardWrite the equilibrium constant expression for each of the following: (If a box is not needed, leave it blank.) Submit K K K K K a. CaCO3 (s) — CaO(s) + CO2(g) | b. BaBr₂ (s) ⇒ Ba²+(aq) + 2 Br¯(aq) c. 4H₂O(g) + 3 Fe(s) — 4H₂ (g) + Fe3 04 (8) d. HClO(aq)= H(aq)+CIO (aq) e. NH3(aq)+H,O(l)=NH_*(aq)+OH (aq) Show Tutor Stepsarrow_forwardFor the reaction below the value of KC = 3.5 x 10⁻⁵. If you start with 1.50 M NO and 0.75 M F₂, what is the concentration of NOF after the system has reached equilibrium? 2NO(g) + F₂(g) ⇌ 2NOF(g)arrow_forward
- Explain why we can simplify the calculations for K when the value of K is very small (less than ~104). 4.1 4.2 HCN will react very slightly with water with aK = 6.2 x 101º. 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 H30* to calculate the pH of the solution with the equation pH = -log[H;O*] (you can do this!!!). Put your final answers in the box. If you need more space to show your work, ou can use the backside of this page. %3D [H,O*] at equilibrium M. pH = -log[H;O*] pH = % of HCN that reactedarrow_forwardThe questions below refer to the following system: Co(H2O)6+4 CI=C0C1* + 6H,O (pink) (blue) When cobalt(II) chloride is added to pure water, the Co- ions hydrate. The hydrated form then reacts with the CF ions to set up the equilibrium shown here, Which statement below describes the change that the system will undergo if water is added? Select one: O a. More chloride 1ons will be produced. O b. The equilibrium will shift to the right. O c. There will be less of the hydrated cobalt ion at the new equilibrium position. D search F4 F5 F6 F8 F9 F10 F11 F12 PrtScr Ansert %23 %24 & 6. 8 E R T K B N Marrow_forwardA student determines that an aqueous solution that contains 9.32×10-2 M sodium cyanide and 0.163 M hydrocyanic acid, also has a H3O+ concentration of 8.05×10-10 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium:(1) as is usually done, without the inclusion of water in the expression for K: K =(2) for comparison, with the inclusion of water in the expression for K: K =arrow_forward
- 7. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant of ammonia, NH3, is 1.815x10-5 A student worker is asked to prepare a buffer solution with NH3 and ammonium salt. However, after the student did a thorough search, no ammonium salt is found. After the student reported the result to the professor, the professor told the student the buffer can be prepared with ammonia and a strong acid. Can you help this student out? The pH of the buffer to be prepared is 10.08. The molarity of the ammonia in the buffer is 0.4717 M. The molarity of the ammonia solution found in the laboratory is 1.201 M, the strong acid solution is 0.9948 M HNO3. The volume of the buffer solution to be prepared is 500.0 mL. Please answer the following questions. A. B. What is the molarity of the ammonium ion in the buffer? Please provider your answer below. Check answer How many mL of 0.9948 M HNO3 solution is needed? Please provider your answer below. 0² 0₂ $…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_forwardEthyl acetate (C H 3 COOC H 2 C H 3 ) is produced in theequilibrium system described by the following equation.C H 3 COOH + C H 3 C H 2 OH ⇌C H 3 COOC H 2 C H 3 + H 2 OWhy does the removal of water result in the productionof more ethyl acetate?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher: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
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133611097/9781133611097_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305580343/9781305580343_smallCoverImage.gif)
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