What is the pH of a solution prepared by dissolving 3.00 g of the weak acid HA (molar mass - 13812 g/mol. ka = 1.05 X 10) in 50.0 mL of 0.113 M NaOH and diluting the mixture to 500 mL? 1. 03.25 2. 02.25 3. 05.52 4. 0641 5. 02.52 Previous Next

What is the pH of a solution prepared by dissolving 3.00 g of the weak acid HA (molar mass - 13812 g/mol. ka = 1.05 X 10) in 50.0 mL of 0.113 M NaOH and diluting the mixture to 500 mL? 1. 03.25 2. 02.25 3. 05.52 4. 0641 5. 02.52 Previous Next

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.27QE

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For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
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The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
(i) Calculate the mass of NaHCO3 (84.007 g mol) must be added to 4.00 g of K2CO3 (138.206 g mol 1) to give a pH of 10.80 in 500 mL of water? H2CO3 : Ka1 = 4.45 x10-7, Ka2 = 4.69 x 10-11 %3D (ii) Determine the pH of 100 mL of 0.100 M HCl is added to the solution in (i). (iii) Determine the volume of 0.320 M HNO3 that should be added to 4.00 g K2CO3 to give a pH of 10.00 in 250 mL.
In the laboratory, a general chemistry student measured the pH of a 0.527 M aqueous solution of methylamine, CH3NH₂ to be 12.159. Use the information she obtained to determine the Kb for this base. Kb (experiment) = Show Transcribed Text In the laboratory, a general chemistry student measured the pH of a 0.524 M aqueous solution of pyridine, C,HSN to be 9.461. Use the information she obtained to determine the K, for this base. Kb (experiment) =
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Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.
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A solution containing 0.0138 M maleic acid and 0.0188 M disodium maleate. The K₁ values for maleic acid are 1.20 x 10-2 (Kal) and 5.37 x 10-7 (Ka2). pH = A solution containing 0.0384 M succinic acid and 0.022 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 10-5 (Kal) and 2.31 x 10-6 (Ka2). pH =