General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15, Problem 15.38CP
The following pictures represent solutions at various stages in the titration of sulfuric acid H2A (A2– = SO42–) with aqueous NaOH. (Na+ ions and water molecules have been omitted for clarity.)
- (a) To which of the following stages do solutions 1–4 correspond?
- (i) Halfway to the first equivalence point
- (ii) Halfway between the first and second equivalence points
- (iii) At the second equivalence point
- (iv) Beyond the second equivalence point
- (b) Draw a picture that represents the solution prior to addition of any NaOH.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Determine the pH during the titration of 67.3 mL of 0.459 M hypochlorous acid (K 3.5x108) by 0.459 M NaOH at the following points. (Assume the titration
is done at 25 °C.)
(a) Before the addition of any NaOH
X
(b) After the addition of 17.0 mL of NaOH
X
t
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
x
pt
(e) After the addition of 101 mL of NaOH 12.95
pt
pt
X
The samples of nitric and acetic acids shown here are bothtitrated with a 0.100 M solution of NaOH(aq).
Determine whether each of the following statements concerningthese titrations is true or false.(a) A larger volume of NaOH(aq) is needed to reach theequivalence point in the titration of HNO3.(b) The pH at the equivalence point in the HNO3 titrationwill be lower than the pH at the equivalence point inthe CH3COOH titration.(c) Phenolphthalein would be a suitable indicator for bothtitrations.
Determine the pH during the titration of 57.0 mL of 0.347 M nitrous
acid (K₂ = 4.5x10-4) by 0.347 M NaOH at the following points.
(Assume the titration is done at 25 °C.)
(a) Before the addition of any NaOH
(b) After the addition of 14.0 mL of NaOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 85.5 mL of NaOH
Chapter 15 Solutions
General Chemistry: Atoms First
Ch. 15.1 - Write balanced net ionic equations for the...Ch. 15.1 - Write balanced net ionic equations for the...Ch. 15.2 - Calculate the concentrations of all species...Ch. 15.2 - Calculate the pH in a solution prepared by...Ch. 15.2 - Prob. 15.5CPCh. 15.3 - The following pictures represent solutions that...Ch. 15.3 - Calculate the pH of 0.100 L of a buffer solution...Ch. 15.3 - Calculate the change in pH when 0.002 mol of HNO3...Ch. 15.4 - Use the HendersonHasselbalch equation to calculate...Ch. 15.4 - Prob. 15.10P
Ch. 15.4 - Suppose you are performing an experiment that...Ch. 15.4 - Prob. 15.12PCh. 15.6 - A 40.0 mL volume of 0.100 M HCl is titrated with...Ch. 15.6 - A 40.0 mL volume of 0.100 M NaOH is titrated with...Ch. 15.7 - The following pictures represent solutions at...Ch. 15.7 - Consider the titration of 100.0 mL of 0.016 M HOCl...Ch. 15.7 - The following acid-base indicators change color in...Ch. 15.9 - Assume that 40.0 mL of 0.0800 M H2SO3 (Ka1 = 1.5 ...Ch. 15.9 - Assume that 40.0 mL of a 0.0250 M solution of the...Ch. 15.10 - Write the equilibrium-constant expression for Ksp...Ch. 15.11 - A saturated solution of Ca3(PO4)2 has [Ca2+] =...Ch. 15.11 - Prob. 15.22PCh. 15.11 - Which has the greater molar solubility: AgCl with...Ch. 15.11 - Prob. 15.24CPCh. 15.12 - Calculate the molar solubility of MgF2 in 0.10 M...Ch. 15.12 - Which of the following compounds are more soluble...Ch. 15.12 - In an excess of NH3(aq), Cu2+ ion forms a deep...Ch. 15.12 - Silver bromide dissolves in aqueous sodium...Ch. 15.13 - Prob. 15.29PCh. 15.13 - Will a precipitate form on mixing 25 mL of 1.0 ...Ch. 15.14 - Prob. 15.31PCh. 15.15 - Prob. 15.32PCh. 15 - The following pictures represent solutions that...Ch. 15 - The following pictures represent solutions that...Ch. 15 - The strong acid HA is mixed with an equal molar...Ch. 15 - The following pictures represent solutions at...Ch. 15 - The following pictures represent solutions at...Ch. 15 - The following pictures represent solutions at...Ch. 15 - Prob. 15.40CPCh. 15 - Prob. 15.41CPCh. 15 - Prob. 15.42CPCh. 15 - Prob. 15.43CPCh. 15 - Is the pH greater than, equal to, or less than 7...Ch. 15 - Prob. 15.45SPCh. 15 - Which of the following mixtures has the higher pH?...Ch. 15 - Which of the following mixtures has the lower pH?...Ch. 15 - Phenol (C6H5OH, Ka = 1.3 1010) is a weak acid...Ch. 15 - Aniline (C6H5NH2, Kb = 4.3 1010) is a weak base...Ch. 15 - The equilibrium constant Kn for the neutralization...Ch. 15 - The equilibrium constant Kn for the neutralization...Ch. 15 - Prob. 15.52SPCh. 15 - Does the pH increase, decrease, or remain the same...Ch. 15 - Prob. 15.54SPCh. 15 - Calculate the pH of a solution prepared by mixing...Ch. 15 - Prob. 15.56SPCh. 15 - The pH of a solution of NH3 and NH4Br is 8.90....Ch. 15 - Prob. 15.58SPCh. 15 - Prob. 15.59SPCh. 15 - Prob. 15.60SPCh. 15 - Which of the following gives a buffer solution...Ch. 15 - Prob. 15.62SPCh. 15 - Prob. 15.63SPCh. 15 - Calculate the pH of a buffer solution that is 0.20...Ch. 15 - Prob. 15.65SPCh. 15 - Calculate the pH of 0.250 L of a 0.36 M formic...Ch. 15 - Calculate the pH of0.375 L of a 0.18 M acetic...Ch. 15 - Prob. 15.68SPCh. 15 - Use the HendersonHasselbalch equation to calculate...Ch. 15 - Prob. 15.70SPCh. 15 - Give a recipe for preparing a CH3CO2HCH3CO2Na...Ch. 15 - Prob. 15.72SPCh. 15 - Prob. 15.73SPCh. 15 - What is the Ka of the amino acid leucine if it is...Ch. 15 - Prob. 15.75SPCh. 15 - Prob. 15.76SPCh. 15 - Make a rough plot of pH versus milliliters of acid...Ch. 15 - Prob. 15.78SPCh. 15 - Consider the titration of 50.0 mL of 0.116 M NaOH...Ch. 15 - Consider the titration of 40.0 mL of 0.250 M HF...Ch. 15 - A 100.0 mL sample of 0.100 M methylamine (CH3NH2,...Ch. 15 - Prob. 15.82SPCh. 15 - Consider the titration of 25.0 mL of 0.0200 M...Ch. 15 - Prob. 15.84SPCh. 15 - The equivalence point was reached in titrations of...Ch. 15 - Prob. 15.86SPCh. 15 - What is the pH at the equivalence point for the...Ch. 15 - Prob. 15.88SPCh. 15 - Prob. 15.89SPCh. 15 - Prob. 15.90SPCh. 15 - Prob. 15.91SPCh. 15 - Prob. 15.92SPCh. 15 - Prob. 15.93SPCh. 15 - Prob. 15.94SPCh. 15 - Prob. 15.95SPCh. 15 - Prob. 15.96SPCh. 15 - Prob. 15.97SPCh. 15 - Use Le Chteliers principle to explain the...Ch. 15 - Use Le Chteliers principle to predict whether the...Ch. 15 - Calculate the molar solubility of PbCrO4 in:...Ch. 15 - Calculate the molar solubility of SrF2 in:...Ch. 15 - Which of the following compounds are more soluble...Ch. 15 - Which of the following compounds are more soluble...Ch. 15 - Prob. 15.104SPCh. 15 - Is the solubility of Fe(OH)3 increased, decreased,...Ch. 15 - Prob. 15.106SPCh. 15 - Prob. 15.107SPCh. 15 - Prob. 15.108SPCh. 15 - Prob. 15.109SPCh. 15 - Calculate the molar solubility of AgI in: (a)Pure...Ch. 15 - Calculate the molar solubility of Cr(OH)3 in 0.50...Ch. 15 - What compound, if any, will precipitate when 80 mL...Ch. 15 - Prob. 15.113SPCh. 15 - Prob. 15.114SPCh. 15 - In qualitative analysis, Al3+ and Mg2+ are...Ch. 15 - Prob. 15.116SPCh. 15 - Can Co2+ be separated from Zn2+ by bubbling H2S...Ch. 15 - Prob. 15.118SPCh. 15 - Prob. 15.119SPCh. 15 - Prob. 15.120SPCh. 15 - Give a method for separating the following pairs...Ch. 15 - Assume that you have three white solids: NaCl,...Ch. 15 - On the same graph, sketch pH titration curves for...Ch. 15 - Prob. 15.124CHPCh. 15 - Prob. 15.125CHPCh. 15 - A saturated solution of Mg(OH)2 in water has pH =...Ch. 15 - Prob. 15.128CHPCh. 15 - In qualitative analysis, Ag+, Hg22+, and Pb2+ are...Ch. 15 - Calculate the molar solubility of MnS in a 0.30 M...Ch. 15 - Prob. 15.131CHPCh. 15 - Prob. 15.132CHPCh. 15 - Prob. 15.133CHPCh. 15 - Prob. 15.134CHPCh. 15 - Prob. 15.135CHPCh. 15 - A 100.0 mL sample of a solution that is 0.100 M in...Ch. 15 - A 0.0100 mol sample of solid Cd(OH)2 (Ksp = 5.3 ...Ch. 15 - Zinc hydroxide, Zn(OH)2 (Ksp = 4.1 1017), is...Ch. 15 - Prob. 15.139CHPCh. 15 - Prob. 15.140MPCh. 15 - Ethylenediamine (NH2CH2CH2NH2, abbreviated en) is...Ch. 15 - A 40.0 mL sample of a mixture of HCl and H3PO4 was...Ch. 15 - A 1.000 L sample of HCl gas at 25 C and 732.0 mm...Ch. 15 - Prob. 15.144MPCh. 15 - Consider the reaction that occurs on mixing 50.0...Ch. 15 - In qualitative analysis, Ca2+ and Ba2+ are...Ch. 15 - A railroad tank car derails and spills 36 tons of...Ch. 15 - Prob. 15.148MP
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
- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardWrite the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forward(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after the addition of 0.030 mol HCl? note: Ka (NH4+) = 5.6 x 10 -10 NH3 (aq) + H+ (aq) → NH4+ (aq) (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.arrow_forward
- Calculate the pH for each of the following cases in the titration of 60.0 mL of 0.250-M hydrobromic acid, HBr(aq), with 0.250 M NaOH: (HBr is a strong acid) (a) before addition of any NaOH, (b) after addition of 30.0 mL of NaOH, (c) after addition of 50.0 mL of NaOH, (d) after addition of 60.0 mL of NaOH, and (e) after addition of 80.0 mL of NaOHarrow_forwardA solution NH 3 that contains 78 mL of 0.043 M ammonia, NH 3, is titrated with 0.083 M HCI. The K₁ of ammonia is 1.8×10-5. (a) What volume of 0.083 M HCI would be added to reach the equivalence point? Give the volume in mL. 40.41 mL (b) At the equivalence point, what is the pH of the solution? (Assume that volumes are additive.) 4.56arrow_forwardDetermine the pH during the titration of 59.7 mL of 0.392 M hypochlorous acid (K₂ = 3.5×10-8) by 0.392 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 13.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.6 mL of KOH Submit Show Approach Show Tutor Stepsarrow_forward
- In the titration of 60.0 mL of 1.0 M methylamine, CH3NH₂ (K₁ = 4.4 x 10-4), with 0.50 M HCI, calculate the pH under the following conditions. (a) after 0.00 mL of 0.50 M HCI has been added 4.0 (b) after 20.0 mL of 0.50 M HCI has been added 4.0✔ (c) after 60.0 mL of 0.50 M HCI has been added 4.0✔ (d) at the stoichiometric point 4.0✔ (e) after 200.00 mL of 0.50 M HCI has been added 4.0arrow_forward4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.arrow_forwardA solution NH3 that contains 72 mL of 0.043 M ammonia, NH3, is titrated with 0.083 M HCl. The Kb of ammonia is 1.8x10-5. (a) What volume of 0.083 M HCI would be added to reach the equivalence point? Give the volume in mL. 49 37 mL (b) At the equivalence point, what is the pH of the solution? (Assume that volumes are additive.) 40 8.98 X whawhat "at onubralence point" implies about the quantities of the combined acids and bases? Did you rememberarrow_forward
- Hh.39.arrow_forwardNear the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.arrow_forwardDetermine the pH during the titration of 59.5 mL of 0.490 M hypochlorous acid (Ką = 3.5×10-8) by 0.490 M NaOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOHarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
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
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
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
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
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
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
Acid-Base Equilibrium; Author: Bozeman Science;https://www.youtube.com/watch?v=l5fk7HPmo5g;License: Standard YouTube License, CC-BY
Introduction to Titrimetric analysis; Author: Vidya-mitra;https://www.youtube.com/watch?v=uykGVfn9q24;License: Standard Youtube License