I need help with 15:57 please I’m stuck in that part e: water or10-11 in anx 10-8 ind?strengthsndter, thebound is the-, dissolveshe formulaHrochlorice.lactic acids solution,me of its K?in part tobreakdownEd is 1.23%acid.M solutionine theiallyntrationsoreresent asa 50%les of HNO3lue of HNO₂?s formicculate thecan shrubecauseon ofK, of the acid?n theerage pH ofQuestions and Problems 781c. Calculate the [OH-] concentration of a 4.25 ×10-4 Msolution of aminoethanol.15.58. Food Dye Quinoline is a weakly basic liquid used in themanufacture of quinolone yellow, a greenish-yellow dye forfoods, and in the production of niacin. Its pK, is 9.15.a. What is the pH of a 0.0752 M solution of quinolone?b. What is the hydroxide ion concentration of the solutionin part (a)?15.59. Painkillers Morphine is an effective painkiller but isalso highly addictive. Codeine is a popular prescriptionpainkiller because it is much less addictive than morphine.Codeine contains a basic nitrogen atom that can beprotonated to give the conjugate acid of codeine.a. Calculate the pH of a 1.8 x 10-3 M solution ofmorphine if its pK, = 5.79.b. Calculate the pH of a 2.7 X 10 M solution of codeineif the pK, of the conjugate acid is 8.21.15.60. The awful odor of dead fish is due mostly totrimethylamine, (CH3)3N, one of three compounds relatedto ammonia in which methyl groups replace 1, 2, or all 3 ofthe H atoms in ammonia.a. The K of trimethylamine [(CH3)3N] is 6.5 x 10-5 at25°C. Calculate the pH of a 3.00 x 10-4 M solution oftrimethylamine.b. The K, of methylamine [(CH3)NH₂] is 4.4 X 10 at25°C. Calculate the pH of a 2.88 X 10-³ M solution ofmethylamine.*c. The K, of dimethylamine [(CH3)2NH] is 5.9 X 10 at25°C. What concentration of dimethylamine is neededfor the solution to have the same pH as the solution inpart (b)?Polyprotic AcidsConcept Review15.61. Why is the K, value of phosphoric acid less than its K₁,value but greater than its K, value?15.62. In calculating the pH of a 1.0 M solution of H₂SO3, wecan ignore the H* ions produced by the ionization of thebisulfate (HSO3) ion; however, in calculating the pH ofa 1.0 M solution of sulfuric acid, we cannot ignore the H*ions produced by the ionization of the bisulfate ion. Why?15.63. Carbonic acid, H₂CO3, is a very weak diprotic acid(K,= 4.3 x 10-7), but germanic acid, H₂GeO3, is evenweaker (K,,= 9.8 x 10-10). Suggest a reason why.15.64. Figure P15.64 contains skeletal structures of two782CHAPTER15.67. Ascorbic acidthe pH of a 0.15.68. Rhubarb Pie Tconcentrationsand must be rerhubarb pie. Woxalic acid?15.69. Nicotine Addictproperties of tosolution of nice15.70. Pseudoephedricommon ingreepK, 9.22. Win pseudoephedHOFFIGURE P15.7015.71. Malaria Treatme-the cinchona trefor malaria. Calquinine in water15.72. Dozens of pharmsickness to Viagorganic compourFigure P15.72.a. Solutions of pKb = 2.15 Xsolution of pip*b. Draw the struwould be presNHNHFIGURE P15.7Acid Strength andConcept Review15.73. Explain why the KCLEO escfluoroacetic acid has a pH of 1.44, what is the K, of the acid?15.55. Acid Rain I A weather system moving through theAmerican Midwest produced rain with an average pH of5.02. By the time the system reached New England, therain it produced had an average pH of 4.66. How muchmore acidic was the rain falling in New England?15.56. Acid Rain II A newspaper reported that the "level ofacidity" in a sample taken from an extensively studiedwatershed in New Hampshire in 1998 was "an astounding200 times lower than the worst measurement" taken in thepreceding 23 years. What is this difference expressed inunits of pH?15.57. The K, of aminoethanol, HOCH₂CH₂NH2, is 3.1 X 10.a. Is aminoethanol a stronger or weaker base thanethylamine, pK, = 3.36?b. Calculate the pH of a 1.67 x 10-² M solution ofaminoethanol.!1@ 2#315.63.15.64.Ga10seHOFIGUProblems15.65. What15.66. What

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I need help with 15:57 please I’m stuck in that part e: water or10-11 in anx 10-8 ind?strengthsndter, thebound is the-, dissolveshe formulaHrochlorice.lactic acids solution,me of its K?in part tobreakdownEd is 1.23%acid.M solutionine theiallyntrationsoreresent asa 50%les of HNO3lue of HNO₂?s formicculate thecan shrubecauseon ofK, of the acid?n theerage pH ofQuestions and Problems 781c. Calculate the [OH-] concentration of a 4.25 ×10-4 Msolution of aminoethanol.15.58. Food Dye Quinoline is a weakly basic liquid used in themanufacture of quinolone yellow, a greenish-yellow dye forfoods, and in the production of niacin. Its pK, is 9.15.a. What is the pH of a 0.0752 M solution of quinolone?b. What is the hydroxide ion concentration of the solutionin part (a)?15.59. Painkillers Morphine is an effective painkiller but isalso highly addictive. Codeine is a popular prescriptionpainkiller because it is much less addictive than morphine.Codeine contains a basic nitrogen atom that can beprotonated to give the conjugate acid of codeine.a. Calculate the pH of a 1.8 x 10-3 M solution ofmorphine if its pK, = 5.79.b. Calculate the pH of a 2.7 X 10 M solution of codeineif the pK, of the conjugate acid is 8.21.15.60. The awful odor of dead fish is due mostly totrimethylamine, (CH3)3N, one of three compounds relatedto ammonia in which methyl groups replace 1, 2, or all 3 ofthe H atoms in ammonia.a. The K of trimethylamine [(CH3)3N] is 6.5 x 10-5 at25°C. Calculate the pH of a 3.00 x 10-4 M solution oftrimethylamine.b. The K, of methylamine [(CH3)NH₂] is 4.4 X 10 at25°C. Calculate the pH of a 2.88 X 10-³ M solution ofmethylamine.*c. The K, of dimethylamine [(CH3)2NH] is 5.9 X 10 at25°C. What concentration of dimethylamine is neededfor the solution to have the same pH as the solution inpart (b)?Polyprotic AcidsConcept Review15.61. Why is the K, value of phosphoric acid less than its K₁,value but greater than its K, value?15.62. In calculating the pH of a 1.0 M solution of H₂SO3, wecan ignore the H* ions produced by the ionization of thebisulfate (HSO3) ion; however, in calculating the pH ofa 1.0 M solution of sulfuric acid, we cannot ignore the H*ions produced by the ionization of the bisulfate ion. Why?15.63. Carbonic acid, H₂CO3, is a very weak diprotic acid(K,= 4.3 x 10-7), but germanic acid, H₂GeO3, is evenweaker (K,,= 9.8 x 10-10). Suggest a reason why.15.64. Figure P15.64 contains skeletal structures of two782CHAPTER15.67. Ascorbic acidthe pH of a 0.15.68. Rhubarb Pie Tconcentrationsand must be rerhubarb pie. Woxalic acid?15.69. Nicotine Addictproperties of tosolution of nice15.70. Pseudoephedricommon ingreepK, 9.22. Win pseudoephedHOFFIGURE P15.7015.71. Malaria Treatme-the cinchona trefor malaria. Calquinine in water15.72. Dozens of pharmsickness to Viagorganic compourFigure P15.72.a. Solutions of pKb = 2.15 Xsolution of pip*b. Draw the struwould be presNHNHFIGURE P15.7Acid Strength andConcept Review15.73. Explain why the KCLEO escfluoroacetic acid has a pH of 1.44, what is the K, of the acid?15.55. Acid Rain I A weather system moving through theAmerican Midwest produced rain with an average pH of5.02. By the time the system reached New England, therain it produced had an average pH of 4.66. How muchmore acidic was the rain falling in New England?15.56. Acid Rain II A newspaper reported that the &#34;level ofacidity&#34; in a sample taken from an extensively studiedwatershed in New Hampshire in 1998 was &#34;an astounding200 times lower than the worst measurement&#34; taken in thepreceding 23 years. What is this difference expressed inunits of pH?15.57. The K, of aminoethanol, HOCH₂CH₂NH2, is 3.1 X 10.a. Is aminoethanol a stronger or weaker base thanethylamine, pK, = 3.36?b. Calculate the pH of a 1.67 x 10-² M solution ofaminoethanol.!1@ 2#315.63.15.64.Ga10seHOFIGUProblems15.65. What15.66. What

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15.57. The K, of aminoethanol, HOCH₂CH₂NH₂, is 3.1 x 10-5. a. Is aminoethanol a stronger or weaker base than ethylamine, pK, = 3.36? b. Calculate the pH of a 1.67 X 102 M solution of aminoethanol.