PRINCIPLES+REACTIONS
8th Edition
ISBN: 9781337759632
Author: Masterton
Publisher: CENGAGE L
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Question
Chapter 15, Problem 68QAP
Interpretation Introduction
Interpretation:
The correct statement needs to be identified.
Concept introduction:
Solubility product constant
Expert Solution & Answer
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Students have asked these similar questions
(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 0.00336 g of Ag2C2O4 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ag2C2O4.Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?solubility = mol/L
(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature?
Ksp
=
(b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-
product constant for Y₂(CO3)3.
Ksp
=
(c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04?
solubility
mol/L
The thermodynamic solubility product of AGCN is 6.0x10-17.
(a) What is [Ag+] in a 0.033 M KNO3 solution?
4.0
7.7e-9
X mol·L-1
(b) What is [Ag+] in a 0.033 M KCN solution?
4.0 1.8e-15
X mol·L-1
Chapter 15 Solutions
PRINCIPLES+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
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Similar questions
- Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the accompanying anion. What mass of CaO should be added to 1.0 L of this aqueous solution to precipitate all the Mg2+ and Ca2+ as CaCO3 and MgCO3? What is the total mass of the two solids formed?arrow_forwardDescribe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forward
- The thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1arrow_forwardConsider the insoluble compound nickel(II) hydroxide , Ni(OH)2 . The nickel ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN), , K=1.0×10³" . Be sure to specify states such as (aq) or (s). + + K =arrow_forwardBecause barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?arrow_forward
- Lead (II) chloride, PbCl2, has Ksp = 1.6 x 10–5. (a) Determine the solubility of PbCl2 expressed in mol/L; (b) How many grams of PbCl2 will dissolve in 250 mL of water? (c) Predict whether PbCl2 precipitate will be formed when 2.0 mL of 0.10 M Pb(NO3)2 is added to 3.0 mL of 0.10 M NaCl.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_forwardCalculate the silver ion concentration, [Ag'], of a solution prepared by dissolving 1.00 g of AgNO3 and 10.0 g of KCN in sufficient water to make 1.00 L of solution. (Hint: Because k is very large, assume the reaction goes to completion then calculate the [Ag). RAg" (aq) + 2CN (aq) = Ag(CN)2(aq) kr = 1.0 x 1021 42 1g AgNO3 Helpful hint : You will need: AgNO3 = 169.989 1 mol AgNO3 169.98 g AgNO3 mol 5.89 x 103 mol Ag KCN = 65.12 3 mol 19KCN 1 mol KCN 65.12 g KCN 0.154 mol CN-arrow_forward
- A 3.20 L solution of 1.25 x 10³ M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 x 10¹¹ M NaCl. (a) Calculate Qc for the dissolution of PbCl₂. (b) No precipitate has formed. Is the solution supersaturated, saturated, or unsaturatedarrow_forwardChemistry The first container contains 20 ml 0.02 M AgNO3 solution at 25 ° C and the second container contains 40mL 0.04 M CaCl2 solution. (A) Determine the solubility product of AgNO3 in solution of 1st pot. (B) Analyze whether AgCI precipitation will occur when the solution of the 2nd container is completely mixed with the solution of the 1st container. The solubility of AgNO3 at 25 ° C = 2.2 × 10-3gL-1 and the solubility of AgCI is 1.8 × 10-10, the mass of Ag = 107.87arrow_forwardCalcium carbonate is sparingly soluble in water. CaCO:(s) = Ca²"(aq) + CO;²(aq) Kp= 3.4 x 109 (a) Calculate the solubility of CaCO; in sea water containing 0.01 mol L-ª of Ca²* ions. (b) Given the additional information below and using the Henderson Hasselbalch equation, what is the major form of carbonate in sea water and why? pH sea water = 8.1 H2CO: pKai = 6.35 HCO; pK2 = 10.33 Write down the relevant equilibria and explain why the actual solubility of calcium carbonate (4.6 x 10-7 mol L-') is higher than the value you determined in part (a)?arrow_forward
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