Chemistry: Structure And Properties: Custom Edition For University Of Maryland, College Park
4th Edition
ISBN: 9781323738832
Author: Tro
Publisher: PEARSON C
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Chapter 17, Problem 70E
Interpretation Introduction
To determine:
To calculate the pH of propionic acid when added base, and to find its equivalence point, one half equivalence point and to sketch its titration curve.
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Check out a sample textbook solutionChapter 17 Solutions
Chemistry: Structure And Properties: Custom Edition For University Of Maryland, College Park
Ch. 17 - What is the pH range of human blood? How is human...Ch. 17 - What is a buffer? How does a buffer work? How does...Ch. 17 - What is the common ion effect?Ch. 17 - What is the HendersonHasselbalch equation, and why...Ch. 17 - What is the pH of a buffer when the concentrations...Ch. 17 - Suppose that a buffer contains equal amounts of a...Ch. 17 - How do you use the Henderson—Hasselbalch equation...Ch. 17 - What factors influence the effectiveness of a...Ch. 17 - What is the effective pH range of a buffer...Ch. 17 - Describe acidbase titration. What is the...
Ch. 17 - The pH at the equivalence point of the titration...Ch. 17 - The volume required to reach the equivalence point...Ch. 17 - In the titration of a strong acid with a strong...Ch. 17 - In the titration of a weak acid with a strong...Ch. 17 - The titration of a diprotic acid with sufficiently...Ch. 17 - In the titration of a polyprotic acid, the volume...Ch. 17 - What is the difference between the endpoint and...Ch. 17 - What is an indicator? How can an indicator signal...Ch. 17 - What is the solubility-product constant? Write a...Ch. 17 - What is molar solubility? How do you obtain the...Ch. 17 - How does a common ion affect the solubility of a...Ch. 17 - How is the solubility of an ionic compound with a...Ch. 17 - For a given solution containing an ionic compound,...Ch. 17 - What is selective precipitation? Under which...Ch. 17 - In which of these solutions does HNO2 ionize less...Ch. 17 - A formic acid solution has a pH of 3.25. Which of...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Calculate the percent ionization of a 0.15 M...Ch. 17 - Calculate the percent ionization of a 0.13 M...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - A buffer contains significant amounts of acetic...Ch. 17 - A buffer contains significant amounts of ammonia...Ch. 17 - Use the HendersonHasselbalch equation to calculate...Ch. 17 - Use the Henderson—Hasselbalch equation to...Ch. 17 - Use the Henderson—Hasselbalch equation to...Ch. 17 - Use the Henderson—Hasselbaich equation to...Ch. 17 - Calculate the pH of the solution that results from...Ch. 17 - Calculate the pH of the solution that results from...Ch. 17 - Calculate the ratio of NaF to HF required to...Ch. 17 - Calculate the ratio of CH3NH2 to CH3NH3Cl...Ch. 17 - What mass of sodium benzoate should you add to...Ch. 17 - What mass of ammonium chloride should you add to...Ch. 17 - A 250.0-mL buffer solution is 0.250 M in acetic...Ch. 17 - A 100.0-mL buffer solution is 0.175 M in HCIO and...Ch. 17 - For each solution, calculate the initial and final...Ch. 17 - For each solution, calculate the initial and final...Ch. 17 - A 350.0-mL buffer solution is 0.150 in HF and...Ch. 17 - A 100.0-mL buffer solution is 0.100 M ¡n NH3 and...Ch. 17 - Determine whether the mixing of each pair of...Ch. 17 - Determine whether the mixing of each pair of...Ch. 17 - Blood s buffered by carbonic acid and the...Ch. 17 - The fluids within cells are buffered by H2PO4 and...Ch. 17 - Which buffer system is the best choice to create a...Ch. 17 - Which buffer system is the best choice to create a...Ch. 17 - A 500.0-mL buffer solution is 0.100 M in HNO2 and...Ch. 17 - Prob. 58ECh. 17 - The graphs labeled (a) and (b) are the titration...Ch. 17 - Two 25.0-mL samples, one 0.100 M HCI and the other...Ch. 17 - Two 20.0-mL samples, one 0.200 M KOH and the other...Ch. 17 - Prob. 62ECh. 17 - Consider the curve shown here for the titration of...Ch. 17 - Consider the curve shown here for the titration of...Ch. 17 - Consider the titration of a 35.0-mL sample of...Ch. 17 - A 20.0-mL sample of 0.125 M HNO3 is titrated with...Ch. 17 - Consider the titration of a 25.0-mL sample of...Ch. 17 - Prob. 68ECh. 17 - Prob. 69ECh. 17 - Prob. 70ECh. 17 - Consider the titration of a 25.0-mL sample of...Ch. 17 - Prob. 72ECh. 17 - Prob. 73ECh. 17 - Prob. 74ECh. 17 - Prob. 75ECh. 17 - Prob. 76ECh. 17 - Prob. 77ECh. 17 - Prob. 78ECh. 17 - Methyl red has a pKaof 5.0 and is red in its acid...Ch. 17 - Phenolphthalein has a pKaof 9.7. It is colorless...Ch. 17 - Referring to Table 17.1pick an indicator for use...Ch. 17 - Referring to Table 17.1 pick an indicator for use...Ch. 17 - Write balanced equations and expressions for...Ch. 17 - Prob. 84ECh. 17 - Refer to the Kspvalues in Table 17.2 to calculate...Ch. 17 - Prob. 86ECh. 17 - Use the given molar solubilities in pure water to...Ch. 17 - Prob. 88ECh. 17 - Two compounds with general formulas AX and AX2...Ch. 17 - Consider the compounds with the generic formulas...Ch. 17 - Refer to the Ksp value from Table 17.2 to...Ch. 17 - Prob. 92ECh. 17 - Calculate the molar solubility of barium fluoride...Ch. 17 - Prob. 94ECh. 17 - Calculate the molar solubility of calcium...Ch. 17 - Calculate the solubility (in grams per 1.00102 of...Ch. 17 - Is each compound more soluble in acidic solution...Ch. 17 - Is each compound more soluble in acidic solution...Ch. 17 - A solution containing sodium fluoride is mixed...Ch. 17 - A solution containing potassium bromide is mixed...Ch. 17 - Predict whether a precipitate forms if you mix...Ch. 17 - Prob. 102ECh. 17 - Prob. 103ECh. 17 - Prob. 104ECh. 17 - A solution is 0.010 M in Ba2+ and 0.020 M in Ca2+...Ch. 17 - Prob. 106ECh. 17 - A solution is made 1.1103M in Zn(NO3)2 and 0.150 M...Ch. 17 - A 120.0-mL sample of a solution that is 2.8103M in...Ch. 17 - Use the appropriate values of Kspand Kfto find the...Ch. 17 - Prob. 110ECh. 17 - A 1.500-mL solution contains 2.05 g of sodium...Ch. 17 - A solution ¡s made by combining 10.0 ml of 17.5 M...Ch. 17 - A buffer is created by combining 150.0 mL of 0.25...Ch. 17 - A buffer is created by combining 3.55 g of NH3...Ch. 17 - A 1.0-L buffer solution initially contains 0.25...Ch. 17 - A 250.0-mL buffer solution initially contains...Ch. 17 - In analytical chemistry, bases used for titrations...Ch. 17 - A 0.5224-g sample of an unknown monoprotic acid...Ch. 17 - A 0.25-mol sample of a weak acid with an unknown...Ch. 17 - A 5.55-g sample of a weak acid with Ka=1.3104 is...Ch. 17 - A 0.552-g sample of ascorbic acid (vitamin C) is...Ch. 17 - Sketch the titration curve from Problem 121by...Ch. 17 - One of the main components of hard water is CaCO3....Ch. 17 - Gout—a condition that results in joint swelling...Ch. 17 - Pseudogout, a condition with symptoms similar to...Ch. 17 - Calculate the solubility of silver chloride in a...Ch. 17 - Calculate the solubility of CuX ¡n a solution that...Ch. 17 - Aniline, C6H5NH2, is an important organic base...Ch. 17 - The Kbof hydroxylamine, NH2OH is 1.0108 . A buffer...Ch. 17 - Prob. 130ECh. 17 - Prob. 131ECh. 17 - Prob. 132ECh. 17 - What relative masses of dimethyl amine and...Ch. 17 - You are asked to prepare 2.0 L of a HCN/NaCN...Ch. 17 - Prob. 135ECh. 17 - Prob. 136ECh. 17 - Prob. 137ECh. 17 - Prob. 138ECh. 17 - When excess solid Mg(OH)2 is shaken with 1.00 L of...Ch. 17 - Prob. 140ECh. 17 - Calculate the solubility of Au(OH)3 in (a) water...Ch. 17 - Calculate the concentration of I in a solution...Ch. 17 - Prob. 143ECh. 17 - Prob. 144ECh. 17 - Find the pH of a solution prepared from 1.0 L of a...Ch. 17 - Prob. 146ECh. 17 - Prob. 147ECh. 17 - Prob. 148ECh. 17 - Consider three solutions: 0.10 M solution of a...Ch. 17 - Prob. 150ECh. 17 - Prob. 151ECh. 17 - Prob. 152ECh. 17 - Prob. 153ECh. 17 - Prob. 154ECh. 17 - A certain town gets its water from an underground...Ch. 17 - Prob. 156ECh. 17 - Prob. 157ECh. 17 - A buffer is 0.100 M in NH4CI and 0.100 M in NH3....Ch. 17 - What is the pH of a buffer that is 0.120 M in...Ch. 17 - Prob. 3SAQCh. 17 - Prob. 4SAQCh. 17 - Prob. 5SAQCh. 17 - Prob. 6SAQCh. 17 - Prob. 7SAQCh. 17 - A 10.0-mL sample of 0.200 M hydrocyanic acid (HCN)...Ch. 17 - Prob. 9SAQCh. 17 - Prob. 10SAQCh. 17 - Prob. 11SAQCh. 17 - Prob. 12SAQCh. 17 - Calculate the molar solubility of magnesium...Ch. 17 - Prob. 14SAQCh. 17 - Prob. 15SAQ
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- For the titration of 50.0 mL of 0.100-M HCl with 0.100-M NaOH, calculate the pH when these volumes of NaOH have been added: (a) 10.0 mL (b) 25.00 mL (c) 45.0 mL (d) 50.5 mLarrow_forwardThe titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.arrow_forwardFor the titration of 50.0 mL of 0.150 M ethylamine. C2H5NH2, with 0.100 M HCl, find the pH at each of the following points, and then use that information to sketch the titration curve and decide on an appropriate indicator. (a) At the beginning, before HCl is added (b) At the halfway point in the titration (c) When 75% of the required acid has been added (d) At the equivalence point (e) When 10.0 mL more HCl has been added than is required (f) Sketch the titration curve. (g) Suggest an appropriate indicator for this titration.arrow_forward
- Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.arrow_forwardFifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).arrow_forwardCalculate the pH during the titration of 50.00 mL of 0.100 M Sr(OH)2 with 0.100 M HNO3 after 0, 50.00, 100.00, and 150.00 mL nitric acid have been added. Graph the titration curve and compare with the titration curve obtained in Exercise 16.22.arrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY