Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 17.6, Problem 17.6.2SR
Interpretation Introduction
Interpretation:
The required concentration of barium ion to start precipitation of barium solution has to be explained using the given data.
Concept introduction:
- The solubility product constant (
- Solubility product is the multiplication of concentration of dissolved ion, raised to the power of coefficients.
To calculate: The concentration of barium ion.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
A chemist is performing a titration in order to determine the amount of sodium hydroxide, NaOH(aq), in 125 mL of an aqueous
solution.
(a) If 28 mL of a 0.13 M HCl solution was used as a titrant to reach the equivalence point, what was the concentration of
sodium hydroxide in the initial solution?
M
(b) What was the initial pH of the sodium hydroxide solution?
6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic acid (CH3COOH) solution.
(A) write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.
(B) Write the complete ionic equation for the reaction that occurs when few drops of sodium hydroxide solution are added to the buffer.
Group of answer choices
a.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq)
(B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l)
b.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq)
(B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)
c.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq)
(B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l)
d.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq)
(B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)
Be sure to answer all parts.
What is the maximum mass (in grams) of each of the following soluble salts that can be added to 250
mL of 0.050 M BaCl, without causing a precipitate to form? (Assume that the addition of solid causes
no change in volume.)
(a) (NH),SO,
x 10
(Enter your answer in scientific notation.)
(b) Pb(NO3)2
(c) NaF
Chapter 17 Solutions
Chemistry: Atoms First
Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Prob. 17.1.1SRCh. 17.1 - Prob. 17.1.2SRCh. 17.2 - Starting with 1.00 L of a buffer that is 1.00 M in...Ch. 17.2 - Prob. 2PPACh. 17.2 - Prob. 2PPBCh. 17.2 - Prob. 17.3WECh. 17.2 - Prob. 3PPA
Ch. 17.2 - Prob. 3PPBCh. 17.2 - Prob. 17.2.1SRCh. 17.2 - Consider 1 L of a buffer that is 0.85 M in formic...Ch. 17.2 - Prob. 17.2.3SRCh. 17.2 - Prob. 17.2.4SRCh. 17.3 - Calculate the pH in the titration of 50.0 mL of...Ch. 17.3 - For the titration of 10.0 mL of 0.15 M acetic acid...Ch. 17.3 - Prob. 4PPBCh. 17.3 - Prob. 4PPCCh. 17.3 - Prob. 17.5WECh. 17.3 - Prob. 5PPACh. 17.3 - Prob. 5PPBCh. 17.3 - Which of the graphs [(i)(iv)] best represents the...Ch. 17.3 - Prob. 17.6WECh. 17.3 - Prob. 6PPACh. 17.3 - Prob. 6PPBCh. 17.3 - Calculate the pH at the equivalence point in the...Ch. 17.3 - Prob. 17.3.2SRCh. 17.3 - Prob. 17.3.3SRCh. 17.4 - Calculate the solubility of copper(II) hydroxide...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Prob. 17.8WECh. 17.4 - Prob. 8PPACh. 17.4 - Prob. 8PPBCh. 17.4 - Prob. 8PPCCh. 17.4 - Prob. 17.9WECh. 17.4 - Predict whether a precipitate will form from each...Ch. 17.4 - Prob. 9PPBCh. 17.4 - Prob. 17.4.1SRCh. 17.4 - Prob. 17.4.2SRCh. 17.4 - Prob. 17.4.3SRCh. 17.5 - Prob. 17.10WECh. 17.5 - Calculate the molar solubility of AgI in (a) pure...Ch. 17.5 - Arrange the following salts in order of increasing...Ch. 17.5 - Prob. 17.11WECh. 17.5 - Determine if the following compounds are more...Ch. 17.5 - Prob. 11PPBCh. 17.5 - Prob. 11PPCCh. 17.5 - Prob. 17.12WECh. 17.5 - Prob. 12PPACh. 17.5 - Prob. 12PPBCh. 17.5 - Beginning with a saturated solution of AgCl, which...Ch. 17.5 - Prob. 17.5.1SRCh. 17.6 - Prob. 17.13WECh. 17.6 - Prob. 13PPACh. 17.6 - Prob. 13PPBCh. 17.6 - Prob. 17.6.1SRCh. 17.6 - Prob. 17.6.2SRCh. 17 - Which of the acids in Table 16.5 (page 732) can be...Ch. 17 - Prob. 17.3KSPCh. 17 - How much sodium fluoride must be dissolved in 250...Ch. 17 - Use Le Chteliers principle to explain how the...Ch. 17 - Describe the effect on pH (increase, decrease, or...Ch. 17 - Prob. 17.3QPCh. 17 - Prob. 17.4QPCh. 17 - Determine the pH of (a) a 0.40 M CH3COOH solution,...Ch. 17 - Determine the pH of (a) a 0.20 M NH3 solution, and...Ch. 17 - Which pair of substances can be dissolved together...Ch. 17 - Prob. 17.2VCCh. 17 - Prob. 17.3VCCh. 17 - Prob. 17.4VCCh. 17 - Prob. 17.7QPCh. 17 - Prob. 17.8QPCh. 17 - Calculate the pH of the buffer system made up of...Ch. 17 - Calculate the pH of the following two buffer...Ch. 17 - Prob. 17.11QPCh. 17 - Prob. 17.12QPCh. 17 - Prob. 17.13QPCh. 17 - The pH of blood plasma is 7.40. Assuming the...Ch. 17 - Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl...Ch. 17 - Calculate the pH of 1.00 L of the buffer 1.00 M...Ch. 17 - Prob. 17.17QPCh. 17 - Prob. 17.18QPCh. 17 - Prob. 17.19QPCh. 17 - Prob. 17.20QPCh. 17 - The diagrams [(a)(d)] contain one or more of the...Ch. 17 - Prob. 17.22QPCh. 17 - Prob. 17.23QPCh. 17 - Prob. 17.24QPCh. 17 - Prob. 17.25QPCh. 17 - The amount of indicator used in an acid-base...Ch. 17 - Prob. 17.27QPCh. 17 - Prob. 17.28QPCh. 17 - Prob. 17.29QPCh. 17 - Prob. 17.30QPCh. 17 - Prob. 17.31QPCh. 17 - Prob. 17.32QPCh. 17 - Prob. 17.33QPCh. 17 - Prob. 17.34QPCh. 17 - A 25.0-,L solution of 0n100 M CH3COOH is titrated...Ch. 17 - A 10.0-mL solution of 0.300 M NH3 is titratee with...Ch. 17 - Prob. 17.37QPCh. 17 - Prob. 17.38QPCh. 17 - Prob. 17.39QPCh. 17 - Prob. 17.40QPCh. 17 - Diagrams (a) through (d) represent solutions at...Ch. 17 - Prob. 17.42QPCh. 17 - Prob. 17.43QPCh. 17 - Prob. 17.44QPCh. 17 - Write balanced equations and solubility product...Ch. 17 - Prob. 17.46QPCh. 17 - Prob. 17.47QPCh. 17 - Prob. 17.48QPCh. 17 - Prob. 17.49QPCh. 17 - Prob. 17.50QPCh. 17 - Prob. 17.51QPCh. 17 - The solubility of an ionic compound MX (molar mass...Ch. 17 - Prob. 17.53QPCh. 17 - Prob. 17.54QPCh. 17 - Prob. 17.55QPCh. 17 - Prob. 17.56QPCh. 17 - Prob. 17.57QPCh. 17 - A volume of 75 mL of 0.060 M NaF is mixed with 25...Ch. 17 - Prob. 17.59QPCh. 17 - Prob. 17.60QPCh. 17 - Prob. 17.5VCCh. 17 - Prob. 17.6VCCh. 17 - Prob. 17.7VCCh. 17 - How would the concentration of silver ion in the...Ch. 17 - Prob. 17.61QPCh. 17 - Prob. 17.62QPCh. 17 - Prob. 17.63QPCh. 17 - Prob. 17.64QPCh. 17 - The solubility product of PbBr2 is 8.9 106....Ch. 17 - Prob. 17.66QPCh. 17 - Calculate the molar solubility of BaSO4 in (a)...Ch. 17 - Prob. 17.68QPCh. 17 - Prob. 17.69QPCh. 17 - Prob. 17.70QPCh. 17 - Prob. 17.71QPCh. 17 - Prob. 17.72QPCh. 17 - Calculate the concentrations of Cd2+, Cd(CN)42 ,...Ch. 17 - Prob. 17.74QPCh. 17 - Prob. 17.75QPCh. 17 - (a) Calculate the molar solubility of...Ch. 17 - Prob. 17.77QPCh. 17 - Prob. 17.78QPCh. 17 - Prob. 17.79QPCh. 17 - Prob. 17.80QPCh. 17 - Prob. 17.81QPCh. 17 - Prob. 17.82QPCh. 17 - Prob. 17.83QPCh. 17 - Prob. 17.84QPCh. 17 - In a group 1 analysis, a student adds HCl acid to...Ch. 17 - Prob. 17.86QPCh. 17 - Prob. 17.87QPCh. 17 - Sketch the titration curve of a weak acid with a...Ch. 17 - Prob. 17.89QPCh. 17 - Prob. 17.90QPCh. 17 - Prob. 17.91QPCh. 17 - Tris [tris(hydroxymethyl)aminomethane] is a common...Ch. 17 - Prob. 17.93QPCh. 17 - Prob. 17.94QPCh. 17 - Prob. 17.95QPCh. 17 - Prob. 17.96QPCh. 17 - Prob. 17.97QPCh. 17 - Find the approximate pH range suitable for...Ch. 17 - Prob. 17.99QPCh. 17 - Prob. 17.100QPCh. 17 - Prob. 17.101QPCh. 17 - Prob. 17.102QPCh. 17 - Barium is a toxic substance that can seriously...Ch. 17 - The pKa of phenolphthalein is 9.10. Over what pH...Ch. 17 - Prob. 17.105QPCh. 17 - Prob. 17.106QPCh. 17 - Prob. 17.107QPCh. 17 - The molar mass of a certain metal carbonate, MCO3,...Ch. 17 - Prob. 17.109QPCh. 17 - Prob. 17.110QPCh. 17 - Describe how you would prepare a 1 -L 0.20 M...Ch. 17 - Phenolphthalein is the common indicator for the...Ch. 17 - Prob. 17.113QPCh. 17 - Prob. 17.114QPCh. 17 - Prob. 17.115QPCh. 17 - Prob. 17.116QPCh. 17 - Prob. 17.117QPCh. 17 - Prob. 17.118QPCh. 17 - When lemon juice is added to tea, the color...Ch. 17 - How many milliliters of 1.0 M NaOH must be added...Ch. 17 - Prob. 17.121QPCh. 17 - Prob. 17.122QPCh. 17 - Prob. 17.123QPCh. 17 - Prob. 17.124QPCh. 17 - Calcium oxalate is a major component of kidney...Ch. 17 - Water containing Ca2+ and Mg2+ ions is called hard...Ch. 17 - Prob. 17.127QPCh. 17 - Prob. 17.128QPCh. 17 - Prob. 17.129QPCh. 17 - (a) Referring to Figure 17.4, describe how you...Ch. 17 - Prob. 17.131QPCh. 17 - Prob. 17.132QPCh. 17 - Prob. 17.133QPCh. 17 - Prob. 17.134QPCh. 17 - Prob. 17.135QPCh. 17 - Prob. 17.136QPCh. 17 - A sample of 0.96 L of HCl gas at 372 mmHg and 22C...Ch. 17 - Prob. 17.138QPCh. 17 - The solutions (a) through (f) represent various...Ch. 17 - Prob. 17.140QPCh. 17 - Prob. 17.141QP
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
- Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?arrow_forwardWrite a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitratearrow_forwardA chemist combines 53.5 mL of 0.350 M potassium bromide with 23.9 mL of 0.533 M lead nitrate. (a) How many grams of lead bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the lead or bromide ion, whichever one is in excess? (а) g PbBr2 (b) M Kt (c) Мехсess ionarrow_forward
- 6. A student mixes equal volumes of 1.0 M solutions of tin(II) chloride and copper (II) sulfate and observes that no precipitate forms. Then the student mixes equal volumes of 1.0 M solutions of zinc (II) sulfate and tin (II) fluoride and observes the formation of a precipitate. The formula of the precipitate must be (A) SnF2 (B) SnSO4 (C) Sn(SO4)2 (D) ZnF (E) ZnF2arrow_forwardDetermine the molar concentration of each ion present in the solutions that result from each of the following mixtures: (Disregard the concentration of H+ and OH- from water and assume that volumes are additive.) (a) 57.4 mL of 0.79 M HCl and 77.3 mL of 1.48 M HCl: (b) 120 mL of 0.59 M CaCl2 and 120 mL of 0.27 M CaCl2 (c) 31.9 mL of 0.369 M NaOH and 20.2 mL of 0.278 M HCl (d) 14.0 mL of 0.724 M H2SO4 and 20.3 mL of 0.110 M NaOHarrow_forwardFor each statement, indicate whether it is true or false.(a) The solubility of a slightly soluble salt can be expressedin units of moles per liter.(b) The solubility product of a slightly soluble salt is simplythe square of the solubility.(c) The solubility of a slightly soluble salt is independent ofthe presence of a common ion.(d) The solubility product of a slightly soluble salt is independentof the presence of a common ion.arrow_forward
- In the following acid-base titration experiment NaOH(aq) + HNO3(aq) ———> NaNO3(aq) + H2O(1). What is the molarity of the HNO3 solution if 18.3 mL of 0.115 M NaOH was used to neutralize 25 mL of HNO3? (a) 0.157 M (b) 0.0842 M (c) 3.978 M (d) 0.0157 Marrow_forwardA chemist combines 53.9 mL of 0.372 M potassium bromide with 23.1 mL of 0.451 M silver nitrate. (a) How many grams of silver bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the silver or bromide ion, whichever one is in excess? (а) g AgBr (b) M K* (c) Мехсess ionarrow_forwardGive detailed Solution with explanation neededarrow_forward
- What is the equilibrium concentration of CN ion after mixing the following solutions? (Hint: Mixing the solutions dilutes the reactants.) (a) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M NH3? Kc = 0.71 4.0✔ NH3(aq) + HCN(aq) ⇒ NH4+ (aq) + CN ¯(aq) M (b) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M K₂S? S² (aq) + HCN(aq) = HS¯(aq) + CN −(aq) Kc = 3.1 x 10³ XM 4.0 5.0e2 (c) mixing 50.0 mL of 0.100 M HCN with 50.0 mL of 0.100 M KF? F (aq) + HCN(aq) = HF(aq) + CN ¯(aq) Kc = 5.6 x 10-7 M 4.0 3.7e-5arrow_forward5. Limestone consists mainly of mineral calcite, CaCO3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO₂. (a). Write the chemical reaction describing this reaction. (b). If the access HCl required 39.96 mL of 0.1004 M NaOH to neutralize, find the weight percent of calcite in the limestone.arrow_forwardConsider the reaction: CaCl(aq) + 2AgNO3(aq) - > Ca( NOz)2(aq) + 2AgC|(s) How many grams of CaCl would be needed to precipitate the Ag* ions from 20.50 mL of a 0.0150 M AgNOs solution? The molar mass of CaCk is 110.98 g/mol.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 Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY