25.0 ml of a 0.100 M trimethylamine (CH3)3N (a base like ammonia) Kb = 6.3×10−5, are transferred in an Erlenmeyer flask and titrated with 0.100 M of HCl. Predict pH, pOH, concentration of trimethylamine, concentration of the conjugated acid (CH3)3NH+, and concentration of HCl in the Erlenmeyer flask when: (a) 0 mL of HCl solution are added to the Erlenmeyer flask (a) 12.5 mL of HCl solution are added to the Erlenmeyer flask (c) 25 mL of HCl solution are added to the Erlenmeyer flask (d) 30 mL of HCl solution are added to the Erlenmeyer flask (e) Based on the information from points a-d, draw the expected titration curve (pH vs volume of HCl (ml))
25.0 ml of a 0.100 M trimethylamine (CH3)3N (a base like ammonia) Kb = 6.3×10−5, are transferred in an Erlenmeyer flask and titrated with 0.100 M of HCl. Predict pH, pOH, concentration of trimethylami...
A 25.0-mL sample of a 0.250 M solution of aqueous trimethylamine is titrated with a 0.313 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0. and 30.0 ml of acid have been added; pKb of (CH3)3N = 4.19 at 25degreeC. pH after 10.0 mL of acid have been added; 4.19 Number Did you find the pH or the pOH of this solution? pH after 20.0 mL of acid have been added: Number 3.65 pH after 30.0...
A 25.0 mL sample of a 0.1300 M solution of aqueous trimethylamine is titrated with a 0.1625 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C.
A 25.0 mL sample of a 0.2800 M solution of aqueous trimethylamine is titrated with a 0.3500 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C. pH after 20.0 mL of acid have been added =
Calculate the pH during the titration of 20.00 mL of 0.1000 M trimethylamine, (CH3)3N(aq), with 0.1000 M HCl(aq) after 21 mL of the acid have been added. Kb of trimethylamine = 6.5 x 10-5.
A 25.0 mL sample of a 0.2400 M solution of aqueous trimethylamine is titrated with a 0.3000 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C. mostly need help with part 3. I keep doing it incorrectly part 1: pH after 10 ml acid added part 2: pH after 20 ml acid added part 3: pH after 30 ml acid added
5.00 mL of 0.250 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl). The Kb for ammonia is 1.75 x 10-5 What is the pH of the ammonia solution prior to the addition of any HCl? What is the pH of the solution after 5.00 mL of HCl has been added?
44. A 25.0 mL sample of a 0.100 M solution of aqueous trimethylamine is titrated with a 0.125 M solution of HCI. What is the pH of the solution after 10.0, 20.0 and 30.0 mL of acid have been added? Acids К. Acetic 1.76 x 105 Bases Кь Ammonia Methylamine Dimethylamine Trimethylamine 1.76 x 10 4.4x 104 5.9 x 104 6.46 x 105 Salts Кар 3.3 x 108 PbF2 PbCl2 1.7 x 10 5.3 х 10° CaF2
a. Determine the pH during the titration of 31.3 mL of 0.264 M trimethylamine ((CH3)3N, Kb = 6.3×10-5) by 0.264 M HI 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 HI ____ (b) After the addition of 12.6 mL of HI ____ (c) At the titration midpoint ____ (d) At the equivalence point ____ (e) After adding 43.8...
A 25.0 mL aqueous sample of 0.220 M triethylamine, (CH3CH2)3N, where Kb = 5.2*10^-4 is titrated with 0.500 M HCl(aq). 1) What is the pH before any titrant has been added? (Show all work.) 2) What is the pH at the midpoint of the titration? (Show all work.) 3) What is the pH after a total of 8.0 mL of HCl has been added? (Show all work) 4) What is the pH at the equivalence point of the titration? (Show...
Ka * Kb = Kw = 1.0 X 10-14 A 25.0 ml sample of a 0.100 M solution of aqueo us ammonia is titrated with a 0.125 M solution of HCI. Calculate the pH of the solution after 0.00, 10.0, 20.0, 30.00, and 40.0 mL of acid have been added; Kb of NH3= 1.8 X 10-5 at 25 °C. Hint: First find the moles after each 10.00 ml of acid is added. Then find the concentration after equilibrium is reached.