dimethylamine (CH3)2NH, is a weak base with a Kb of 5.95*10-4. It is titrated with hydrochloric...
dimethylamine (CH3)2NH, is a weak base with a Kb of 5.95*10-4. It is titrated with hydrochloric acid (HCl).
A. Write the reaction with proper substances, arrows, and states of matter.
B. If 25.00mL of a 0.130 M (CH3)2NH are mixed with 8.00mL of 0.200 M HCl, what is the pH?
C. At what volume of 0.200 M HCl is required to reach the equivalence point?
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dimethylamine (CH3)2NH, is a weak base
with a Kb of 5.95*10-4. It is titrated with
hydrochloric...
13. (25 pts total) Dimethylamine, or (CH3)2 NH, is a weak base with a Ko of...
13. (25 pts total) Dimethylamine, or (CH3)2 NH, is a weak base with a Ko of 5.95 x 104. It is titrated with hydrochloric acid (Hc) (a) (5 pts) Write the reaction with proper substances, arrows, and states of matter. Note: I may accept several versions of this reaction, but use the entire chemical formula of the weak base. (b) (13 pts) If 25.00 mL of 0.130 M (CH3)2NH are mixed with 8.00 mL of 0.200 M HCI, what is...
A 21.5 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.269 M hydroiodic acid....
A 21.5 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.269 M hydroiodic acid. (1) Before the addition of any hydroiodic acid, the pH is (2) After adding 12.5 mL of hydroiodic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 46.1 mL of hydroiodic acid, the pH is Ka of (CH3)2NH is 5.9x10^-4
A 23.4 mL sample of 0.237 M dimethylamine, (CH3)2NH, is titrated with 0.368 M hydrolodic acid...
A 23.4 mL sample of 0.237 M dimethylamine, (CH3)2NH, is titrated with 0.368 M hydrolodic acid At the equivalence point, the pH is Use the Tables link in the References for any equilibrium constants that are required.
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a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ...
A 27.9 mL sample of 0.289 M dimethylamine, (CH3)2NH, is titrated with 0.286 M hydrobromic acid. ...
A 27.9 mL sample of 0.289 M dimethylamine, (CH3)2NH, is titrated with 0.286 M hydrobromic acid. (1) Before the addition of any hydrobromic acid, the pH is (2) After adding 12.0 mL of hydrobromic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 45.1 mL of hydrobromic acid, the pH is Use the Tables link on the toolbar for any equilibrium constants that are required.
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; Kb = 0.000540)...
Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 6.0 mL pH = (c) 12.0 mL pH = (d) 18.0 mL pH = (e) 24.0 mL pH = (f) 40.8 mL pH =
A 22.7 mL sample of 0.318 M dimethylamine, (CH3)2NH, is titrated with 0.257 M nitric acid. At the titration midpoint, th...
A 22.7 mL sample of 0.318 M dimethylamine, (CH3)2NH, is titrated with 0.257 M nitric acid. At the titration midpoint, the pH is ____.
A 29.5 mL sample of 0.300 M dimethylamine, (CH3)2NH, is titrated with 0.267 M hydrobromic acid....
A 29.5 mL sample of 0.300 M dimethylamine, (CH3)2NH, is titrated with 0.267 M hydrobromic acid. After adding 12.7 mL of hydrobromic acid, the pH is Use the Tables link in the References for any equilibrium constants that are required.
38.50mL of a 0.23M weak base (Kb= 1.8 x 10^-5) are titrated with 0.37M sulfuric acid,...
38.50mL of a 0.23M weak base (Kb= 1.8 x 10^-5) are titrated with 0.37M sulfuric acid, and it took 15.67mL of the acid to reach the equivalence point. Calculate the pH of the solution after 22.00mL of the acid has been added.
13. (25 pts total) Dimethylamine, or (CH3)2 NH, is a weak base with a Ko of 5.95 x 104. It is titrated with hydrochloric acid (Hc) (a) (5 pts) Write the reaction with proper substances, arrows, and states of matter. Note: I may accept several versions of this reaction, but use the entire chemical formula of the weak base. (b) (13 pts) If 25.00 mL of 0.130 M (CH3)2NH are mixed with 8.00 mL of 0.200 M HCI, what is...
A 23.4 mL sample of 0.237 M dimethylamine, (CH3)2NH, is titrated with 0.368 M hydrolodic acid At the equivalence point, the pH is Use the Tables link in the References for any equilibrium constants that are required.
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
A 29.5 mL sample of 0.300 M dimethylamine, (CH3)2NH, is titrated with 0.267 M hydrobromic acid. After adding 12.7 mL of hydrobromic acid, the pH is Use the Tables link in the References for any equilibrium constants that are required.
38.50mL of a 0.23M weak base (Kb= 1.8 x 10^-5) are titrated with 0.37M sulfuric acid, and it took 15.67mL of the acid to reach the equivalence point. Calculate the pH of the solution after 22.00mL of the acid has been added.
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