Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
15th Edition
ISBN: 9781269935678
Author: Nivaldo J. Tro
Publisher: Pearson Education
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Chapter 18, Problem 15E
The titration of a diprotic acid with sufficiently different pKa’s displays two equivalence points. Why?
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The titration of a polyprotic acid with sufficiently different pKa ’s displays two equivalence points. Why?
When a buffer contains equal concentration of the acid and its conjugate base, the pH of the buffer is equal to pKa of the acid.
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Why is the titration curve steepest at the equivalence point?
Chapter 18 Solutions
Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
Ch. 18 - A buffer is 0.100 M in NH4CI and 0.100 M in NH3....Ch. 18 - What is the pH of a buffer that is 0.120 M in...Ch. 18 - Prob. 3SAQCh. 18 - Prob. 4SAQCh. 18 - Prob. 5SAQCh. 18 - Prob. 6SAQCh. 18 - Prob. 7SAQCh. 18 - A 10.0-mL sample of 0.200 M hydrocyanic acid (HCN)...Ch. 18 - Prob. 9SAQCh. 18 - Prob. 10SAQ
Ch. 18 - Prob. 11SAQCh. 18 - Prob. 12SAQCh. 18 - Calculate the molar solubility of magnesium...Ch. 18 - Prob. 14SAQCh. 18 - Prob. 15SAQCh. 18 - What is the pH range of human blood? How is human...Ch. 18 - What is a buffer? How does a buffer work? How does...Ch. 18 - What is the common ion effect?Ch. 18 - What is the HendersonHasselbalch equation, and why...Ch. 18 - What is the pH of a buffer when the concentrations...Ch. 18 - Suppose that a buffer contains equal amounts of a...Ch. 18 - How do you use the Henderson—Hasselbalch equation...Ch. 18 - What factors influence the effectiveness of a...Ch. 18 - What is the effective pH range of a buffer...Ch. 18 - Describe acidbase titration. What is the...Ch. 18 - The pH at the equivalence point of the titration...Ch. 18 - The volume required to reach the equivalence point...Ch. 18 - In the titration of a strong acid with a strong...Ch. 18 - In the titration of a weak acid with a strong...Ch. 18 - The titration of a diprotic acid with sufficiently...Ch. 18 - In the titration of a polyprotic acid, the volume...Ch. 18 - What is the difference between the endpoint and...Ch. 18 - What is an indicator? How can an indicator signal...Ch. 18 - What is the solubility-product constant? Write a...Ch. 18 - What is molar solubility? How do you obtain the...Ch. 18 - How does a common ion affect the solubility of a...Ch. 18 - How is the solubility of an ionic compound with a...Ch. 18 - For a given solution containing an ionic compound,...Ch. 18 - What is selective precipitation? Under which...Ch. 18 - In which of these solutions does HNO2 ionize less...Ch. 18 - A formic acid solution has a pH of 3.25. Which of...Ch. 18 - Solve an equilibrium problem (using an ICE table)...Ch. 18 - Solve an equilibrium problem (using an ICE table)...Ch. 18 - Calculate the percent ionization of a 0.15 M...Ch. 18 - Calculate the percent ionization of a 0.13 M...Ch. 18 - Solve an equilibrium problem (using an ICE table)...Ch. 18 - Solve an equilibrium problem (using an ICE table)...Ch. 18 - A buffer contains significant amounts of acetic...Ch. 18 - A buffer contains significant amounts of ammonia...Ch. 18 - Use the HendersonHasselbalch equation to calculate...Ch. 18 - Use the Henderson—Hasselbalch equation to...Ch. 18 - Use the Henderson—Hasselbalch equation to...Ch. 18 - Use the Henderson—Hasselbaich equation to...Ch. 18 - Calculate the pH of the solution that results from...Ch. 18 - Calculate the pH of the solution that results from...Ch. 18 - Calculate the ratio of NaF to HF required to...Ch. 18 - Calculate the ratio of CH3NH2 to CH3NH3Cl...Ch. 18 - What mass of sodium benzoate should you add to...Ch. 18 - What mass of ammonium chloride should you add to...Ch. 18 - A 250.0-mL buffer solution is 0.250 M in acetic...Ch. 18 - A 100.0-mL buffer solution is 0.175 M in HCIO and...Ch. 18 - For each solution, calculate the initial and final...Ch. 18 - For each solution, calculate the initial and final...Ch. 18 - A 350.0-mL buffer solution is 0.150 in HF and...Ch. 18 - A 100.0-mL buffer solution is 0.100 M ¡n NH3 and...Ch. 18 - Determine whether the mixing of each pair of...Ch. 18 - Determine whether the mixing of each pair of...Ch. 18 - Blood s buffered by carbonic acid and the...Ch. 18 - The fluids within cells are buffered by H2PO4 and...Ch. 18 - Which buffer system is the best choice to create a...Ch. 18 - Which buffer system is the best choice to create a...Ch. 18 - A 500.0-mL buffer solution is 0.100 M in HNO2 and...Ch. 18 - Prob. 58ECh. 18 - The graphs labeled (a) and (b) are the titration...Ch. 18 - Two 25.0-mL samples, one 0.100 M HCI and the other...Ch. 18 - Two 20.0-mL samples, one 0.200 M KOH and the other...Ch. 18 - Prob. 62ECh. 18 - Consider the curve shown here for the titration of...Ch. 18 - Consider the curve shown here for the titration of...Ch. 18 - Consider the titration of a 35.0-mL sample of...Ch. 18 - A 20.0-mL sample of 0.125 M HNO3 is titrated with...Ch. 18 - Consider the titration of a 25.0-mL sample of...Ch. 18 - Prob. 68ECh. 18 - Prob. 69ECh. 18 - Prob. 70ECh. 18 - Consider the titration of a 25.0-mL sample of...Ch. 18 - Prob. 72ECh. 18 - Prob. 73ECh. 18 - Prob. 74ECh. 18 - Prob. 75ECh. 18 - Prob. 76ECh. 18 - Prob. 77ECh. 18 - Prob. 78ECh. 18 - Methyl red has a pKaof 5.0 and is red in its acid...Ch. 18 - Phenolphthalein has a pKaof 9.7. It is colorless...Ch. 18 - Referring to Table 17.1pick an indicator for use...Ch. 18 - Referring to Table 17.1 pick an indicator for use...Ch. 18 - Write balanced equations and expressions for...Ch. 18 - Prob. 84ECh. 18 - Refer to the Kspvalues in Table 17.2 to calculate...Ch. 18 - Prob. 86ECh. 18 - Use the given molar solubilities in pure water to...Ch. 18 - Prob. 88ECh. 18 - Two compounds with general formulas AX and AX2...Ch. 18 - Consider the compounds with the generic formulas...Ch. 18 - Refer to the Ksp value from Table 17.2 to...Ch. 18 - Prob. 92ECh. 18 - Calculate the molar solubility of barium fluoride...Ch. 18 - Prob. 94ECh. 18 - Calculate the molar solubility of calcium...Ch. 18 - Calculate the solubility (in grams per 1.00102 of...Ch. 18 - Is each compound more soluble in acidic solution...Ch. 18 - Is each compound more soluble in acidic solution...Ch. 18 - A solution containing sodium fluoride is mixed...Ch. 18 - A solution containing potassium bromide is mixed...Ch. 18 - Predict whether a precipitate forms if you mix...Ch. 18 - Prob. 102ECh. 18 - Prob. 103ECh. 18 - Prob. 104ECh. 18 - A solution is 0.010 M in Ba2+ and 0.020 M in Ca2+...Ch. 18 - Prob. 106ECh. 18 - A solution is made 1.1103M in Zn(NO3)2 and 0.150 M...Ch. 18 - A 120.0-mL sample of a solution that is 2.8103M in...Ch. 18 - Use the appropriate values of Kspand Kfto find the...Ch. 18 - Prob. 110ECh. 18 - A 1.500-mL solution contains 2.05 g of sodium...Ch. 18 - A solution ¡s made by combining 10.0 ml of 17.5 M...Ch. 18 - A buffer is created by combining 150.0 mL of 0.25...Ch. 18 - A buffer is created by combining 3.55 g of NH3...Ch. 18 - A 1.0-L buffer solution initially contains 0.25...Ch. 18 - A 250.0-mL buffer solution initially contains...Ch. 18 - In analytical chemistry, bases used for titrations...Ch. 18 - A 0.5224-g sample of an unknown monoprotic acid...Ch. 18 - A 0.25-mol sample of a weak acid with an unknown...Ch. 18 - A 5.55-g sample of a weak acid with Ka=1.3104 is...Ch. 18 - A 0.552-g sample of ascorbic acid (vitamin C) is...Ch. 18 - Sketch the titration curve from Problem 121by...Ch. 18 - One of the main components of hard water is CaCO3....Ch. 18 - Gout—a condition that results in joint swelling...Ch. 18 - Pseudogout, a condition with symptoms similar to...Ch. 18 - Calculate the solubility of silver chloride in a...Ch. 18 - Calculate the solubility of CuX ¡n a solution that...Ch. 18 - Aniline, C6H5NH2, is an important organic base...Ch. 18 - The Kbof hydroxylamine, NH2OH is 1.0108 . A buffer...Ch. 18 - Prob. 130ECh. 18 - Prob. 131ECh. 18 - Prob. 132ECh. 18 - What relative masses of dimethyl amine and...Ch. 18 - You are asked to prepare 2.0 L of a HCN/NaCN...Ch. 18 - Prob. 135ECh. 18 - Prob. 136ECh. 18 - Prob. 137ECh. 18 - Prob. 138ECh. 18 - When excess solid Mg(OH)2 is shaken with 1.00 L of...Ch. 18 - Prob. 140ECh. 18 - Calculate the solubility of Au(OH)3 in (a) water...Ch. 18 - Calculate the concentration of I in a solution...Ch. 18 - Prob. 143ECh. 18 - Prob. 144ECh. 18 - Find the pH of a solution prepared from 1.0 L of a...Ch. 18 - Prob. 146ECh. 18 - Prob. 147ECh. 18 - Prob. 148ECh. 18 - Consider three solutions: 0.10 M solution of a...Ch. 18 - Prob. 150ECh. 18 - Prob. 151E
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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 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_forwardGiven three acid-base indicators—methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)—which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acidarrow_forwardCacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to prepare buffered solutions. Calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500.0 mL of a pH = 6.60 buffer so that the buffer has a total of arsenic-containing species equal to 0.25 M, that is, so that: [(CH3)2AsO2H] + [(CH3)2AsO2] = 0.25 Marrow_forward
- After a buffer solution of carbonic acid (with pKa of 3.75) was added with 1ml of sulfuric acid, the resulting pH of the carbonic acid buffer solution is 1.25. Do you think the carbonic buffer system still works effectively after the addition of the said acid?arrow_forwardA student starts a titration without phenolphthalein in the Erlenmeyer flask.The student realizes the mistake and adds the phenolphthalein during the titration.Once the phenolphthalein is added,the solution in the Erlenmeyer flask remains colorless.Can the results of this titration be used? Concisely explain.arrow_forwardHow does the titration curve of a monoprotic acid differ from that of a diprotic acid?arrow_forward
- What is the difference between endpoint and equivalence point in acid-base titration?arrow_forwardYou need to prepare an acetate buffer of pH 5.42 from a 0.774 M acetic acid solution and a 2.96 M KOH solution. If you have 880 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.42? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures. mLarrow_forwardYou need to prepare an acetate buffer of pH 5.27 from a 0.895 M acetic acid solution and a 2.71 M KOH solution. If you have 880 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.27? The pKą of acetic acid is 4.76. Be sure to use appropriate significant figures.arrow_forward
- Acetic acid’s pKa is 4.75 and nitrous acid’s pKa is 3.16. If you made one buffer of equal parts acetic acid and its conjugate base, then a second buffer of equal parts nitrous acid and its conjugate base, how would the two buffers’ pHs compare to each other? Why? Note: no math is required to address this question.arrow_forwardThe pKa for Bis-Tris buffer is 6.5. What is the concentration of Bis-Tris Base if the pH is 6.9 and the concentration of Tris Acid is 4 mM (4x10-3M)?arrow_forwardWhich of the following species will contribute to the errors of a Mohr titration when it is done in a basic medium? -chromic acid -sodium hydroxide -silver hydroxide -sodium dichromatearrow_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