Calculate the pH values in 20.00 mL of a 0.500 M solution of ammonia to which the following volumes (in mL) of a 0.500 M HBr solution are added in a titration (pKb of NH3 = 4.75). (5)
a. 0.00 b. 6.00 c. 10.00 d. 20.00 e. 30.00
Calculate the pH values in 20.00 mL of a 0.500 M solution of ammonia to which...
Consider titration of 20.0 mL of 0.100 M NH3 with 0.200 M HCl solution. Calculate the pH after the addition of the following volumes of HCl solution. The Kb of NH3 = 1.8 x 10^5 a. 0.00 mL b. 6.00 mL c. 10.00 mL d. 20.00 mL
Calculate the pH for 100. mL of a 0.500 M solution of ammonia, (NH3 Kb=1.8x10-5) being titrated with 0.500 M HCl at the following positions in the titration. i) The initial pH (before any HCl has been added). A. 9.44 B. 10.81 C. 11.48 D. 12.00 E. 11.75
2. Calculate the pH at the following point in the titration of 20.00 mL of0.500 M CH3COOH with 0.500 M NaOH. CH3COOH has a Ka = 1.8x10-5. (2.5 pts) a. pH before the addition of any NaOH. Include balanced chemical equation. b. pH after the addition of 8.00 mL of 0.500 M NaOH. Include balanced chemical equation. c. pH after the addition of 10.00 mL of 0.500 M NaOH. Include balanced chemical equation. d. pH after the addition of 20.00...
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.
11) (5 points) Calculate the pH of 100.0 mL of a 0.500 M solution of methylamin when it is titrated with 0.250 M HCl. Methylamine has a pKb of 3.36 a) 0 mL HCl added c) Equivalence point d) 10 mL past the equivalence point
Consider a buffer prepared by mixing 75ml of 0.03640 M ammonia (NH3) solution with 28ml of 0.02454 M ammonium chloride solution (pKb of ammonia is 4.75) 5. If you added 1 mL of 0.2550 M NaOH to 103 mL of pure water, what would the pH be?
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
Calculate the pH during the titration of 30.00 mL of
0.1000 M
KOH with 0.1000 M HBR solution after the following
additions of acid: (a) 0 mL (b) 18.00 mL (c) 30.00 mL (d) 35.10
mL
Titration Calculation Practice Problems 1. Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 0 mL (b) 18.00 mL (c) 30.00 mL (d) 35.10 ml
Part 4: Calculating pH values as a Titration Progresses - this is a tough question! Finally, consider a 20.00 mL aqueous solution of 0.20 M H2A, where "H2A" is some arbitrary diprotic acid (Ka1 = 4.35 x 10-7, Kaz = 4.85 x 10-11 Estimate the pH values of the solution after the addition of 0.00, 10.00, 20.00, 30.00, 40.00, and 60.00 mL of 0.20 M NaOH. d) Calculation M4 - 30.00 ml NaOH Added: Here we realize that 20 ml...
Titrating 30.00 mL of 0.160 M solution of Na3PO4 with 0.1200 M HCl, calculate the pH of the solution after: a) 20.00 mL of Titrant has been added b) 60.00 mL of Titrant has been added