Unknown amine (base), (pKb=?), is added to water. Determine the pKb of the unknown amine if a 0.015 M solution has a pH of 10.5
Unknown amine (base), (pKb=?), is added to water. Determine the pKb of the unknown amine if...
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
1.The pH of a 2.65×10-3 M solution of a weak base is 9.17. Calculate pKb for this base to two decimal places. 2.Determine the mass (in g) of sodium butanoate (NaC3H7COO) that must be added to 78.9 mL of 0.609 M butanoic acid to yield a pH of 6.43. Report your answer to 3 significant figures. Assume the volume of the solution does not change and that the 5% approximation is valid.
3) a) What is the pKb for a weak base if the pH of a 0.125M solution of this weak base was found to be 8.16? 4) When a weak acid is added to water to make a 0.250M solution, the acid was found to be 1.5% ionized. What is the Ka and pKa of this weak acid? 5) At 60°C, Kw = 9.6x10-14 (Kw increases as the temperature increases). a) For pure water at 60°C, what is the [H+] and pH....
Consider a weak base that has a pKb of 4.2. • What is the pKa of this solution? • What is the pH of a 0.2 M solution of this base? • If you were to mix 50 mL of the 0.2 M base with 50 mL of a 0.1 M solution of its conjugate acid, what would the pH of this buffer be, and what is its effective buffering range?
Strychnine is a weak base with a pKb of 5.74. A 150. mL sample of 0.076 M strychnine solution is titrated using 0.060 M hydrochloric acid. What is the pH of the solution at the following points: a) No acid has been added. b) 25.00 mL of acid have been added. c) 100.00 mL of acid have been added. d) The midpoint of the titration. e) The equivalence point of the titration. f) Sketch this titration curve, labeling the axes,...
Sodium acetate (Na CH3COO), (pKa=4.8), is added to water. Determine the pH of a 0.015 M solution of sodium acetate. (Hint CH3OO− is the conjugate baseof acetic acid CH3COOH
Calculate the pKb of a weak base BOH, which gives a pH of 10.5 when 0.01 moles of the base is dissolved in 500 mL of water. Select one: O a. 3.5 O b. 1.7 O c. 2.0 O d. 3.16 o e. 5.3
6) When 0.0100 moles of dimethyl amine ((CH3)2NH) is added to 1.000 liters of water, the pH of the water increases above the value pH = 7.0 found for neutral solutions. Based on this, we may conclude that a) dimethyl amide is a Lewis base b) dimethyl amide is a Bronsted base c) dimethyl amide is an Arrhenius base d) both b and c e) Both a and b and
6) When 0.0100 moles of dimethyl amine ((CH3)2NH) is added to 1.000 liters of water, the pH of the water increases above the value pH = 7.0 found for neutral solutions. Based on this, we may conclude that a) dimethyl amide is an Arrhenius base b) dimethyl amide is a Bronsted base c) dimethyl amide is a Lewis base d) both a and b e) Both a and b and c
6) When 0.0100 moles of dimethyl amine ((CH3)2NH) is added to 1.000 liters of water, the pH of the water increases above the value pH = 7.0 found for neutral solutions. Based on this, we may conclude that a) dimethyl amide is an Arrhenius base b) dimethyl amide is a Bronsted base c) dimethyl amide is a Lewis base d) both a and b e) Both a and b and c 3