NH3 is a weak base with a Kb value of 1.76x10–5. Suppose 25.0 mL of a0.180 MNH3 is titrate using HCl. The end point is reach after 35.0 mL HCl had been added. Calculate the pH of the resulting solution at the equivalence-point. Here is the titration equation:NH3(aq) + HCl(aq) →NH4Cl(aq)
NH3 is a weak base with a Kb value of 1.76x10–5. Suppose 25.0 mL of a0.180...
Consider the titration of 50.0 mL of 0.133 M NH3 (a weak base with Kb = 1.76 x 10-5 ) with 0.223 M HCl (a strong acid). Calculate the pH of the solution at each of the following points: 1. What is the pH of the solution before the titration is begun? 2. What is the pH of the solution after the addition of 15 mL of HCl? 3. What is the pH of the solution at the equivalence point?...
You have 15.00 mL of a 0.100 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
You have 25.00 mL of a 0.100 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...
In the titration of a 25 mL of 0.245 M weak base (Kb = 1.76*10^-5) being titrated by 0.365 M HCl determine the following: a. The PH at the initial point b. The PH after 12.3 mL of HCl has been added c. The PH at the equivalence point d. The PH after 18.4 mL of HCl has been added
Sera titrates a 10.00 mL sample of a 0.0750 M weak base (A4-) with 0.2500 M HCl, a strong monoprotic acid. The Kb values for this base are Kb1 = 2.00 x 10-3, Kb2 = 3.00 x 10-6, Kb3 = 4.00 x 10-9, and Kb4 = 5.00 x 10-11. Calculate the volume of HCL, in mL, needed to reach the first equivalence point of this titration. Calculate the pH of the titration solution after 4.50 mL of HCl has been...
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
In the titration of 12.1 mL of a 0.183 weak base solution (Kb = 7.7 × 10-7) with 0.22 M HCl solution, what is the pH at the equivalence point? (Hint: first find the equivalence volume and total volume)
3. Weak Base versus Strong Acid Derive a titration curve for the titration of 50.0 mL of 0.10 M NH3 (Kb=1.8 x 10-5) with 0.25 M HCl. Calculate the pH for the following volumes of HCl (0 mL, 10 mL, 15 mL, 20 ml, 25 mL, 30 mL, 35 mL). Volume of HCI, in milliters 0 pH (a) 10 15 (d) 20 |(f) 25 30 35 (g) pH at the equivalence point Specify your choice of indicator
what is the pH of a 0.150M NH4Cl solution? Kb of NH3 = 1.76x10^-5
1. (7 pts) 35.0 mL of a 0.275 M weak base is titrated with 0.325 M HCl. Determine each of the following and sketch the titration curve. If you do the problem on other paper, you will need to do a reasonable approximation of the graph. Ky of the weak base = 2.7 x 10-4 a. The volume of added acid required to reach the equivalence point. b. The initial pH. c. The pH when 5.0 mL of acid has...