In the titration of 30.0 mL of 0.200 M (CH3)2NH with 0.300 M HI. Determine the...

In the titration of 30.0 mL of 0.200 M (CH3)2NH with 0.300 M HI. Determine the pH at the 1/4 of the waypoint in this titration. Determine the pH at the eqivalence point in this titration. Compare both answers and explain if they make sense. (Thanks for the help!)

Sorry! The value for Ka is 3.2 x 10^9 and Kb is 5.4 x 10^-4

Expert Solution

As dimethyl amine is basic in nature so when we make a solution of it we get a solution at high pH.

When we start titration with HI the pH of the solution will start decreasing because HI is acidic in nature.and neutralize the base and at the 1/4 of way point its pH is 11.33.

when we add more acid and reach at equivalence point the pH of the solution becomes less & it is 5.826.

queen_honey_blossom answered 1 year ago

Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540)...

Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 5.3 mL pH = (c) 10.5 mL pH = (d) 15.8 mL pH = (e) 21.0 mL pH = (f) 33.6 mL pH =

Determine the pH during the titration of 34.6 mL of 0.350 M dimethylamine ((CH3)2NH , Kb...

Determine the pH during the titration of 34.6 mL of 0.350 M dimethylamine ((CH3)2NH , Kb = 5.9×10-4) by 0.350M HCl at the following points. (a) Before the addition of any HCl-? (b) After the addition of 14.0 mL of HCl-? (c) At the titration midpoint -? (d) At the equivalence point -? (e) After adding 50.5 mL of HCl-?

In the titration of 30.0 mL of a 0.200 M solution of a hypothetical compound NaH2M,...

In the titration of 30.0 mL of a 0.200 M solution of a hypothetical compound NaH2M, what is the pH of the solution after the addition of 30.0 mL of 0.100 M NaOH? For H3M, pKa1 = 3.00, pKa2 = 6.00, and pKa3 = 9.00.? The answer is 6.0 which is not what I got in my work. Please help me out !

A titration is performed by adding 0.300 M KOH to 30.0 mL of 0.400 M HCl....

A titration is performed by adding 0.300 M KOH to 30.0 mL of 0.400 M HCl. a) Calculate the pH before addition of any KOH. b) Calculate the pH after the addition of 10.0, 25.0 and 39.5 mL of the base. c) Calculate the volume of base needed to reach the equivalence point. d) Calculate the pH at the equivalence point. e) Calculate the pH after adding 5.00 mL of KOH past the endpoint. f) Sketch the titration curve based...

Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540)...

Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. 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) 26.4 mL pH =

Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH (Ka=1.8×10−5) with 0.200 M...

Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH (Ka=1.8×10−5) with 0.200 M NaOH. Determine each quantity: Part A: What is the volume of base required to reach the equivalence point? Express your answer using one decimal place. Part B: What is the pH after 10.0 mL of base have been added? Express your answer using two decimal places. Part C What is the pH at the equivalence point? Express your answer using two decimal places. Part...

Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05)...

Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = _________ (b) 5.3 mL pH = __________ (c) 10.5 mL pH = ____________ (d) 15.8 mL pH = _____________ (e) 21.0 mL pH =___________ (f) 39.9 mL pH = __________

Which indicator would be the best to use for a titration between 0.30 M (CH3)2NH with...

Which indicator would be the best to use for a titration between 0.30 M (CH3)2NH with 0.30 M HI? You will probably need to consult the appropriate table in the book.1. alizarin yellow R, color change at pH 10-122. methyl red, color change at pH 4-63. bromothymol blue, color change at pH 6-84. thymol blue, color change at pH 8-105. phenol red, color change at pH 7-9

Determine the pH during the titration of 38.2 mL of 0.207 M diethylamine ((C2H5)2NH, Kb =...

Determine the pH during the titration of 38.2 mL of 0.207 M diethylamine ((C2H5)2NH, Kb = 6.9×10-4) by 0.207 M HNO3 at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HNO3 _______ (b) After the addition of 14.6 mL of HNO3 ______ (c) At the titration midpoint ________ (d) At the equivalence point _______ (e) After adding 59.2 mL...

2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH....

2. Consider the titration of 25.00 mL of 0.300 M H3 PO4 with 0.300 M NaOH. 2A. Write the net ionic equation for the reaction of phosphoric acid with NaOH to form sodium phosphate and water: 2. What is the pH of the titration medium after the addition of the following volumes of NaOH titrant: 2B. 0.00 mL : 2C. 12.50 mL: 2D. 15.00 mL: 2E. 25.00 mL: 2F. 37.50 mL: 2G: 50.00 mL 2H.60.00 mL 2I. 62.50 mL: 2J....

Question