Laboratory Experiments For Chemistry: The Central Science, Si Edition
14th Edition
ISBN: 9781292221335
Author: Theodore E. Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 17, Problem 58E
calculate the solubility of LaF3 in grams per liter in
a. pure water,
b. 0.010 M KF solution.
c. 0.050 M LaCI3 solution.
Expert Solution & Answer
Learn your wayIncludes step-by-step video
schedule15:45
Students have asked these similar questions
Calculate the solubility (g/L) of Pbl2 in 1.0 M Pb(NO3)2 solution.
а.
1.4 x 10-8
b.
1.2 x 10-4
C. 0.055
d.
5.9 x 10-5
е.
0.027
For the determination of Ca in blood serum, 5 mL of a serum sample is taken and Ca2 + is precipitated as CaC2O4. The precipitate is filtered and dissolved and dissolved with 0.001 M KMnO4 by heating. Calculate the concentration according to 4.94 mL KMnO4 preference.
A. 0.00135
B. 0.00247
C. 0.1135
D. 0.00563
24. The solubility of a salt A2B3 is 1.0 × 10-3 M. Calculate its solubility product.
A. 1.08 x 10-13
B.
1.08 x 10-15
C. 1.08 x 10-10
D. 1.08 x 10-17
25. Calculate the molar solubility of magnesium fluoride (MgF2) in a solution of 0.250 M in NaF. For magnesium
fluoride, Ksp = 5.16 X 10-11.
A. 2.35 x 10-4 M
B. 2.06 x 10-10 M
C. 2.87 x 10-5 M
D. 8.26 x 10-10 M
Chapter 17 Solutions
Laboratory Experiments For Chemistry: The Central Science, Si Edition
Ch. 17.1 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 17.1 - Practice Exercise 2 Calculate the pH of a solution...Ch. 17.1 - Calculate the concentration of the lactate ion in...Ch. 17.1 - Practice Exercise 2 Calculate the format ion...Ch. 17.2 - Practice Exercise 1 If the pH of a buffer solution...Ch. 17.2 - Prob. 17.3.2PECh. 17.2 - Prob. 17.4.1PECh. 17.2 - Prob. 17.4.2PECh. 17.2 - Calculate the number of grams of ammonium chloride...Ch. 17.2 - Prob. 17.5.2PE
Ch. 17.2 - Prob. 17.6.1PECh. 17.2 - Determine The pH of the original buffer described...Ch. 17.3 - An acid-base titration is performed: 250.0 mL of...Ch. 17.3 - Prob. 17.7.2PECh. 17.3 - Prob. 17.8.1PECh. 17.3 - Calculate the pH in the solution formed by adding...Ch. 17.3 - Prob. 17.9.1PECh. 17.3 - Prob. 17.9.2PECh. 17.4 - Which of these expressions correctly expresses the...Ch. 17.4 - Prob. 17.10.2PECh. 17.4 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 17.4 - Prob. 17.11.2PECh. 17.4 - Prob. 17.12.1PECh. 17.4 - Prob. 17.12.2PECh. 17.5 - Consider a saturated solution of the salt MA3, in...Ch. 17.5 - Prob. 17.13.2PECh. 17.5 - Prob. 17.14.1PECh. 17.5 - Prob. 17.14.2PECh. 17.5 - Prob. 17.15.1PECh. 17.5 - Prob. 17.15.2PECh. 17.6 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 17.6 - Does a precipitate form when 0.050 L of 2.0 × 10-2...Ch. 17.6 - Under what conditions does an ionic compound...Ch. 17.6 - Prob. 17.17.2PECh. 17 - Prob. 1DECh. 17 - The following boxes represent aqueos solutions...Ch. 17 - Prob. 2ECh. 17 - Prob. 3ECh. 17 - Prob. 4ECh. 17 - Prob. 5ECh. 17 - Prob. 6ECh. 17 - Prob. 7ECh. 17 - Prob. 8ECh. 17 - 17.9 The following graphs represent the behavior...Ch. 17 - Prob. 10ECh. 17 - 17.11 The graph below shows the solubility of a...Ch. 17 - 17.12 Three cations, Ni+2, Cu+2, and Ag+, are...Ch. 17 - Prob. 13ECh. 17 - Prob. 14ECh. 17 - Prob. 15ECh. 17 - Use information from Appendix D to calculate the...Ch. 17 - Prob. 17ECh. 17 - a. calculate the percent ionization of 0.125 M...Ch. 17 - Prob. 19ECh. 17 - 17.20 Which of the following solutions is a...Ch. 17 - Prob. 21ECh. 17 - Calculate the pH of a buffer that is 0.105n M in...Ch. 17 - Prob. 23ECh. 17 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 17 - You are asked to prepare a pH = 3.00 buffer...Ch. 17 - You are asked to prepare an pH = 4.00 buffer...Ch. 17 - Prob. 27ECh. 17 - Prob. 28ECh. 17 - Prob. 29ECh. 17 - Prob. 30ECh. 17 - Prob. 31ECh. 17 - Prob. 32ECh. 17 - The accompanying graph shows the titration curves...Ch. 17 - Prob. 34ECh. 17 - 17.35 The samples of nitric and acetic acids shows...Ch. 17 - 17.36 Determine whether each of the following...Ch. 17 - Prob. 37ECh. 17 - Prob. 38ECh. 17 - Prob. 39ECh. 17 - Assume that 30.0 mL of a M solution of a week base...Ch. 17 - Prob. 41ECh. 17 - Prob. 42ECh. 17 - Prob. 43ECh. 17 - Prob. 44ECh. 17 - Prob. 45ECh. 17 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 17 - Prob. 47ECh. 17 - Prob. 48ECh. 17 - 17.49 for each statement, incate whether it is...Ch. 17 - The solubility of two slighty soluble salts of...Ch. 17 - Prob. 51ECh. 17 - 17.52
a. true or false: solubility and...Ch. 17 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 17 - Prob. 54ECh. 17 - Prob. 55ECh. 17 - Prob. 56ECh. 17 - using calculate the molar solubility of AgBr in a....Ch. 17 - calculate the solubility of LaF3 in grams per...Ch. 17 - Prob. 59ECh. 17 - Consider a beaker containing a saturated solution...Ch. 17 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 17 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 17 - 17.63 Which of the following salts will be...Ch. 17 - For each of the following slightly soluble salts,...Ch. 17 - Prob. 65ECh. 17 - Prob. 66ECh. 17 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 17 - Prob. 68ECh. 17 - Prob. 69ECh. 17 - Prob. 70ECh. 17 - Calculate the minimum pH needed to precipitate Mn...Ch. 17 - Prob. 72ECh. 17 - Prob. 73ECh. 17 - Prob. 74ECh. 17 - Prob. 75ECh. 17 - Prob. 76ECh. 17 - A solution containing several metal ions is...Ch. 17 - An unknown solid is entirely soluble in water. On...Ch. 17 - Prob. 79ECh. 17 - Prob. 80ECh. 17 - 17.81
Precipitation of the group 4 cautions of...Ch. 17 - Prob. 82ECh. 17 - Prob. 83AECh. 17 - Prob. 84AECh. 17 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 17 - Prob. 86AECh. 17 - Equal quantities of 0.010 M solution of an acid HA...Ch. 17 - Prob. 88AECh. 17 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 17 - A sample of 0.2140 g of an unknown monophonic acid...Ch. 17 - A sample of 0.1687 g of an unknown monoprotic acid...Ch. 17 - Prob. 92AECh. 17 - Prob. 93AECh. 17 - What is the pH of a solution made by mixing 0.30...Ch. 17 - Suppose you want to do a physiological experiment...Ch. 17 - Prob. 96AECh. 17 - Prob. 97AECh. 17 - For each pair of compounds, use Kap values to...Ch. 17 - Prob. 99AECh. 17 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 17 - Salts containing the phosphate ion are added to...Ch. 17 - Prob. 102AECh. 17 - 17.103 The solubility –product constant for barium...Ch. 17 - Prob. 104AECh. 17 - Prob. 105AECh. 17 - A buffer of what pH is needed to give a Mg2+...Ch. 17 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 17 - Prob. 108AECh. 17 - Prob. 109AECh. 17 - Prob. 110IECh. 17 - Prob. 111IECh. 17 - Prob. 112IECh. 17 - Prob. 113IECh. 17 - Prob. 114IECh. 17 - Prob. 115IECh. 17 - Prob. 116IECh. 17 - A concentration of 10-100 parts per billion (by...Ch. 17 - Prob. 118IECh. 17 - Prob. 119IECh. 17 - In nonaqueous solvents, it is possible to react HF...
Additional Science Textbook Solutions
Find more solutions based on key concepts
Starting with 10 bacterial cells per milliliter in a sufficient amount of complete culture medium with a 1-hour...
Microbiology with Diseases by Body System (5th Edition)
WHAT IF? Most prairies experience regular fires, typically every few years. If these disturbances were relative...
Campbell Biology in Focus (2nd Edition)
Out of the given objects found at an ancient campsite which can be used to determine the age of the site is to ...
Living By Chemistry: First Edition Textbook
a. How can aspirin be synthesized from benzene? b. Ibuprofen is the active ingredient in pain relievers such as...
Organic Chemistry (8th Edition)
Why can algae and cyanobacteria be considered indicators of productivity as well as of pollution?
Laboratory Experiments in Microbiology (12th Edition) (What's New in Microbiology)
90. Classify each chemical reaction as a synthesis, decomposition, single-displacement, or double-displacement ...
Introductory Chemistry (6th Edition)
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
- Calculate the solubility (in grams per liter) of magnesium hydroxide in the following. (a) pure water (b) 0.041 M Ba(OH)2 (c) 0.0050 M MgCl2arrow_forwardA volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?arrow_forwardIn a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?arrow_forward
- Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) KClO4:[K+]=0.01M,[ClO4]=0.01M (b) K2PtCl6:[K+]=0.01M,[PtCl62]=0.01M (c) PBI2:[Pb2+]=0.003M,[I]=1.3103M (d) Ag2S:[Ag+]=11010M,[S2]=11013Marrow_forward9. Calculate the molar solubility of BaSO4 (Ksp = 1.1 x 1010) in a. water. b. a solution containing 1.0M SO,2- ionsarrow_forwardCalculate the solubility (in grams per liter) of silver chloride in the following.a. pure water b. 0.025 M BaCl2 c. 0.17 M AgNO3arrow_forward
- 1. The molar solubility of copper(II) sulfide in a 0.201 M ammonium sulfide solution is M. 2. The molar solubility of copper(II) sulfide in a 0.154 M copper(II) acetate solution is M. 3. The maximum amount of calcium carbonate that will dissolve in a 0.200 M sodium carbonate solution is M.arrow_forwarda. Give the chemical equation for the dissociation of P6C1,. 4. b. What is the molar solubility of PbCl,? c. What are the equilibrium concentration of the ions?arrow_forwardThe solubility of a certain salt A2D in a 0.05M solution of A(NO3) is 0.006 M. 1. Calculate the solubility of A2D in a 0.0O1M solution of Na2D. 2. If 50.00 mL of 0.010M A(NO3) is mixed with 25 mL of 0.050M Na2D, calculate the mass of the precipitate, if there are any (Molar mass of A2D = 231.2 g/mol).arrow_forward
- A. Calculate the molar solubility of CaF2 in a 0.1450 M cesium fluoride, CsF solution. Solubility M B. Let's say we have a beaker where a saturated solution of calcium fluoride is in equilibrium with solid calcium fluoride. In which of these cases will the molar solubility be lowest after equilibrium is reestablished? After letting some of the solvent evaporate. Upon the addition of more water. None of these things will do it. After the addition of 0.170 moles of Ca2+ ion. Not enough information given. After the addition of 0.170 moles of F ion. O After the addition of solid NaNO3. The Ksp of calcium fluoride is 3.50x 10-11.arrow_forwardSolid Nal is slowly added to a solution that is 0.010 M in Cu* and 0.010 M Ag*. a. Which compound will begin to precipitate first? b. Calculate the Ag* concentration when Cul first begins to precipitate. c. What percent of Ag* remains in solution at this point?arrow_forward5. A D CHEMISTRY 1110L LAB REPORT: PERIODIC PROPERTIES OF METALS Part One 1. Color of test solutions: 1 M Na₂CO3 1 M LICI 0.1 M MgCl₂ 0.1 M BaCl₂ Part Two 71FX Part Three 4. Flame colors and solubilities of the six unknown solutions Unknown A B C D E 0.1 M SrCl₂ 2. Does the color of the sodium flame depend upon the anion used? Why? F HWIS-1 MgClz CaCl₂ SrCl₂ BaCl, 3. Do you observe a trend in solubilities for the Group IIA sulfates? Group IIA carbonates? Does solubility increase or decrease as you go down a group? Color of Flame Identity of the Six Unknown Solutions B H₂SO4 Name Partner Desk # H₂SO4 1M NaCl 1M KBr 0.1 M CaCl, F Na₂CO3 Na₂CO3 32arrow_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 Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY