In the laboratory, a general chemistry student measured the pH of a 0.372 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.201. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =
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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionFor 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.)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
- Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2In the laboratory, a general chemistry student measured the pH of a 0.327 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.228.Use the information she obtained to determine the Ka for this acid.Ka(experiment) =In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of phenol (a weak acid), C6H;OH to be 5.098. Use the information she obtained to determine the K, for this acid. K(experiment) =
- In the laboratory, a general chemistry student measured the pH of a 0.433 M aqueous solution of phenol (a weak acid), CoH5OH to be 5.167. Use the information she obtained to determine the K, for this acid. K₂(experiment) =In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of nitrous acid to be 1.865. Use the information she obtained to determine the Ka for this acid. Ka(experiment) = In the laboratory, a general chemistry student measured the pH of a 0.431 M aqueous solution of hydrofluoric acid to be 1.741. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =In the laboratory, a general chemistry student measured the pH of a 0.468 M aqueous solution of phenol (a weak acid), C6H5OH to be 5.179. Use the information she obtained to determine the K₂ for this acid. Ka(experiment) =
- The pH scale for acidity is defined by pH log H| where H"| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). Note: You may have to type in a lot of zeros. For example, an answer could be something like this 0.000000000000123. Or you can type your answer in scientific notation, such as 1.23*10-13 [H*] = (B) The pH of lemon juice is 2.0. Calculate the concentration of hydrogen ions in moles Niter (M). per [H*] =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) =In the laboratory, a general chemistry student measured the pH of a 0.371 M aqueous solution of acetylsalicylic acid (aspirin), HC,H-04 to be 1.991. Use the information she obtained to determine the Ka for this acid. K(experiment) =