Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
bartleby

Concept explainers

Question
Chapter 17, Problem 112IL

(a)

Interpretation Introduction

Interpretation: The chloride salt of lead is converted to its chromate salt to test its presence, the reason has to be confirmed.

Concept introduction: Metal ions present in a solution can be identified by a set procedure known as qualitative analysis. Different metal ions show different reactions with different reagent and thus either through the color of the precipitate formed or by smell the gas evolved the metal ion present can be identified.

Some metal ions when present in an aqueous solution containing anions or neutral species called Lewis base or ligands having a tendency to donate electron pairs to metal ions then complex ion formation will take place. Complex ions are stable and thus formation of these increase the solubility of the salt containing the metal ions same as in complex ions.

Example of metal ions that form complex ions includes Ag+,Cd2+,Fe2+,Zn2+,Ni2+ etc.

Example of Lewis bases includes,NH3,OH etc.

(b)

Interpretation Introduction

Interpretation: The presence of Ag+ and Cu2+ ions in the solution has to be confirmed using complex ion  method.

Concept introduction: Metal ions present in a solution can be identified by a set procedure known as qualitative analysis. Different metal ions show different reactions with different reagent and thus either through the color of the precipitate formed or by smell the gas evolved the metal ion present can be identified.

Some metal ions when present in an aqueous solution containing anions or neutral species called Lewis base or ligands having a tendency to donate electron pairs to metal ions then complex ion formation will take place. Complex ions are stable and thus formation of these increase the solubility of the salt containing the metal ions same as in complex ions.

Example of metal ions that form complex ions includes Ag+,Cd2+,Fe2+,Zn2+,Ni2+ etc.

Example of Lewis bases includes,NH3,OH etc.

Blurred answer
Students have asked these similar questions
Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation.  Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.
A student did not notice that the test tube in which she obtained her saturated calcium iodate solution had some water in it. Discuss the effect of this error on the calculated value of the solubility product—was her Ksp value likely to be higher or lower as a result?
If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility =  mol/L

Chapter 17 Solutions

Chemistry & Chemical Reactivity

Ch. 17.3 - The titration of 0.100 M acetic acid with 0.100 M...Ch. 17.3 - Calculate the pH after 75.0 mL of 0.100 M HO has...Ch. 17.3 - 1. What is the pH after 25.0 ml of 0.100 M NaOH...Ch. 17.3 - 2. What is the pH at the equivalence point in the...Ch. 17.3 - Prob. 3RCCh. 17.3 - Phosphate ions are abundant in cells, both as the...Ch. 17.3 - A typical total phosphate concentration in a cell,...Ch. 17.4 - The barium ion concentration, [Ba2+], in a...Ch. 17.4 - Calculate the solubility of AgCN in moles per...Ch. 17.4 - Calculate the solubility of Ca(OH)2 in moles per...Ch. 17.4 - Calculate the solubility of BaSO4 (a) in pure...Ch. 17.4 - 12. Calculate the solubility of Zn(CN)2 at 25°C...Ch. 17.4 - What is the Ksp expression for silver carbonate?...Ch. 17.4 - 2. Using Ksp values, predict which salt in each...Ch. 17.4 - What is the solubility of PbSO4 in water at 25C?...Ch. 17.4 - 4. What is the solubility of PbSO4 in water at...Ch. 17.4 - Prob. 5RCCh. 17.5 - Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker...Ch. 17.5 - Prob. 2CYUCh. 17.5 - Prob. 3CYUCh. 17.5 - 1. Will SrSO4 precipitate from a solution...Ch. 17.6 - Silver nitrate (0.0050 mol) is added to 1.00 L of...Ch. 17.6 - 1. Iron(II) chloride (0.025 mol) is added to 1.00...Ch. 17.7 - Calculate the value of the equilibrium constant,...Ch. 17.7 - 1. What is the equilibrium constant for the...Ch. 17.7 - Prob. 1QCh. 17.7 - What is the minimum volume of 0.0071 M NaCN(aq)...Ch. 17.7 - Use the formation constant of [Au(CN)2] in...Ch. 17.7 - Silver undergoes similar reactions as those shown...Ch. 17.7 - Write a balanced chemical equation for the...Ch. 17 - Does the pH of the solution increase, decrease or...Ch. 17 - Does the pH of the solution increase, decrease, or...Ch. 17 - What is the pH of a solution that consists of 0.20...Ch. 17 - What is the pH of 0.15 M acetic acid to which 1.56...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the buffer solution that...Ch. 17 - Lactic acid (CH3CHOHCO2H) is found in sour milk,...Ch. 17 - What mass of sodium acetate, NaCH3CO2, must he...Ch. 17 - What mass of ammonium chloride, NH4Cl, must be...Ch. 17 - Calculate the pH of a solution that has an acetic...Ch. 17 - Calculate the pH of a solution that has an...Ch. 17 - What must the ratio of acetic acid to acetate ion...Ch. 17 - What must the ratio of H2PO4 to HPO42 be to have a...Ch. 17 - A buffer is composed of formic acid and its...Ch. 17 - A buffer solution is composed of 1.360 g of KH2PO4...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Describe how to prepare a buffer solution from...Ch. 17 - Describe how to prepare a buffer solution from NH3...Ch. 17 - Determine the volume (in mL) of 1.00 M NaOH that...Ch. 17 - Determine the volume (in mL) of 1.00 M HC1 that...Ch. 17 - A buffer solution was prepared by adding 4.95 g of...Ch. 17 - You dissolve 0.425 g of NaOH in 2.00 L of a buffer...Ch. 17 - A buffer solution is prepared by adding 0.125 mol...Ch. 17 - What is the pH change when 20.0 mL of 0.100 M NaOH...Ch. 17 - Phenol, C6H5OH, is a weak organic acid. Suppose...Ch. 17 - Assume you dissolve 0.235 g of the weak acid...Ch. 17 - You require 36.78 mL of 0.0105 M HCl to reach the...Ch. 17 - A titration of 25.0 mL of a solution of the weak...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - You titrate 25.0 mL of 0.10 M NH3 with 0.10 M HCl....Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Name two insoluble salts of each of the following...Ch. 17 - Prob. 38PSCh. 17 - Using the solubility guidelines (Figure 3.10),...Ch. 17 - Predict whether each of the fallowing is insoluble...Ch. 17 - For each of the following insoluble salts, (1)...Ch. 17 - Prob. 42PSCh. 17 - When 1.55 g of solid thallium(I) bromide is added...Ch. 17 - At 20 C, a saturated aqueous solution of silver...Ch. 17 - When 250 mg of SrF2, strontium fluoride, is added...Ch. 17 - Calcium hydroxide, Ca(OH)2, dissolves in water to...Ch. 17 - You add 0.979 g of Pb(OH)2 to 1.00 L of pure water...Ch. 17 - You place 1.234 g of solid Ca(OH)2 in 1.00 L of...Ch. 17 - Estimate the solubility of silver iodide in pure...Ch. 17 - What is the molar concentration of Au+(aq) in a...Ch. 17 - Prob. 51PSCh. 17 - Estimate the solubility of lead(II) bromide (a) in...Ch. 17 - The Ksp value for radium sulfate, RaSO4, is 4.2 ...Ch. 17 - If 55 mg of lead(II) sulfate is placed in 250 mL...Ch. 17 - Prob. 55PSCh. 17 - Prob. 56PSCh. 17 - Calculate the molar solubility of silver...Ch. 17 - Calculate the solubility of silver bromide, AgBr,...Ch. 17 - Compare the solubility, in milligrams per...Ch. 17 - What is the solubility, in milligrams per...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Which insoluble compound in each pair should be...Ch. 17 - Which compound in each pair is more soluble in...Ch. 17 - You have a solution that has a lead(II) ion...Ch. 17 - Sodium carbonate is added to a solution in which...Ch. 17 - If the concentration of Zn2+ in 10.0 mL of water...Ch. 17 - You have 95 mL of a solution that has a lead(II)...Ch. 17 - Prob. 69PSCh. 17 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 17 - Zinc hydroxide is amphoteric (Section 16.10). Use...Ch. 17 - Solid silver iodide, AgI, can be dissolved by...Ch. 17 - What amount of ammonia (moles) must be added to...Ch. 17 - Can you dissolve 15.0 mg of AuCl in 100.0 mL of...Ch. 17 - What is the solubility of AgCl (a) in pure water...Ch. 17 - Prob. 76PSCh. 17 - Prob. 77GQCh. 17 - Prob. 78GQCh. 17 - Prob. 79GQCh. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - For each of the following cases, decide whether...Ch. 17 - Prob. 83GQCh. 17 - A sample of hard water contains about 2.0 103 M...Ch. 17 - What is the pH of a buffer solution prepared from...Ch. 17 - Prob. 86GQCh. 17 - Describe the effect on the pH of the following...Ch. 17 - What volume of 0.120 M NaOH must be added to 100....Ch. 17 - A buffer solution is prepared by dissolving 1.50 g...Ch. 17 - What volume of 0.200 M HCl must be added to 500.0...Ch. 17 - What is the equilibrium constant for the following...Ch. 17 - Calculate the equilibrium constant for the...Ch. 17 - Prob. 93GQCh. 17 - The solubility product constant for calcium...Ch. 17 - In principle, the ions Ba2+ and Ca2+ can be...Ch. 17 - A solution contains 0.10 M iodide ion, I, and 0.10...Ch. 17 - A solution contains Ca2+ and Pb2+ ions, both at a...Ch. 17 - Prob. 98GQCh. 17 - Prob. 99GQCh. 17 - Prob. 100GQCh. 17 - Each pair of ions below is found together in...Ch. 17 - Each pair of ions below is found together in...Ch. 17 - The cations Ba2+ and Sr2+ can be precipitated as...Ch. 17 - You will often work with salts of Fe3+, Pb2+, and...Ch. 17 - Aniline hydrochloride, (C6H5NH3)Cl, is a weak...Ch. 17 - The weak base ethanolamine. HOCH2CH2NH2, can be...Ch. 17 - For the titration of 50.0 mL of 0.150 M...Ch. 17 - A buffer solution with it pH of 12.00 consists of...Ch. 17 - To have a buffer with a pH of 2.50, what volume of...Ch. 17 - What mass of Na3PO4 must be added to 80.0 mL of...Ch. 17 - You have a solution that contains AgNO3, Pb(NO3)2,...Ch. 17 - Prob. 112ILCh. 17 - Suggest a method for separating a precipitate...Ch. 17 - Prob. 114SCQCh. 17 - Prob. 115SCQCh. 17 - Two acids, each approximately 0.01 M in...Ch. 17 - Composition diagrams, commonly known as alpha...Ch. 17 - The composition diagram, or alpha plot, for the...Ch. 17 - The chemical name for aspirin is acetylsalicylic...Ch. 17 - Prob. 120SCQ
Knowledge Booster
Chemistry
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
    • SEE MORE QUESTIONS
    Recommended textbooks for you
  • Principles of Modern Chemistry
    Chemistry
    ISBN:9781305079113
    Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
    Publisher:Cengage Learning
  • Principles of Modern Chemistry
    Chemistry
    ISBN:9781305079113
    Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
    Publisher:Cengage Learning