25.99 mL of a weak monobasic substance, B, is 0.428 M. B is titrated with 17.92 mL of 8.113 M HCL. Calculate the pH. K = 6.78 x 18-4 1. Calculate the equivalence point of the titration. 2. Sketch the titration curve on your scratch paper and indicate the species present at each phase of the process. 3. Indicate where this data point would fall on the curve. 4. calculate the pH of the solution at this point. Record your answer here to two decimal places

25.99 mL of a weak monobasic substance, B, is 0.428 M. B is titrated with 17.92 mL of 8.113 M HCL. Calculate the pH. K = 6.78 x 18-4 1. Calculate the equivalence point of the titration. 2. Sketch the titration curve on your scratch paper and indicate the species present at each phase of the process. 3. Indicate where this data point would fall on the curve. 4. calculate the pH of the solution at this point. Record your answer here to two decimal places

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine the resulting pH when 0.0015 mol of solid Ba(OH)2 is added to a 0.350 L buffer containing 0.110 M weak acid, HA, and 0.220 M of its conjugate base, A-. The value of Ka for HA is 3.2 x 10-9. PREV 1 2 3 4 NEXT Based on your ICE table and definition of Ka, set up the expression for Ka in order to determine the unknown. Do not combine or simplify terms. Ка = 3.2 x 10-9 %3D 5 RESET [0] [0.110] [0.220] [0.101] [0.229] [0.106] [x] [2x] [0.110 + x] [0.110 - x] [0.220 + x] [0.220 - x] [0.101 + x] [0.101 - x] [0.229 + x] [0.229 - x] [0.106 + x] [0.106 - x]
3. Calculate the pH at the equivalence point in the titration of 27.0 mL of 0.792 M NH, with 0.255 M HBr. K. 1.8 x 105
= 0.01 x 0.100 = 0.001 001 50.0 X0-250 = 0.0125 0.0123 025 0.06 0.300 x0.01 0.100. X 0.01 B. 9.25 0.06 6A 10.0 mL solution of 0.300 M NH3 is titrated with 0.100 M HCI. Calculate the pH after the addition of 10.0 mL of acid. A. 9.55 0.001 -0.003 0.300 x 0.0 0.001 C. 8.95 0.02 PH = PKG +10g [0.0156 2.67=4.744+ [19165 TI-84 Plus TEXAS INSTRUMENTS D. 9.73 = Pl= 3.68 - 267 28.3. 0:3 0002 0.002 M Plt = -log = .05 U.2 E. 8.77 Pit=Pkg tog 20.015 = 1.01 [A] [HA]
12. A 1.00 L buffer solution is 0.150 M in weak organic acid HC₂H5O₂ and 0.250 M in LiC7H5O2. Calculate the pH of the solution after the addition of 0.01 mol HCI. The Ka for HC₂H5O2 is 6.5 x 10-5. (hint: the total volume after adding 100ml of HCl solution turn to 1.00L+100ml = 1.10 L, so molarity calculation should be based off the new volume)
10. Calculate the pH of a solution in which 32.0 ml of 0.150 M KOH has been added to 28.0 ml of 0.100 M HCI. 11. Calculate the pH of a buffer consisting of 1.25 M acetic acid and 0.75 M potassium acetate. Ka = 1.8 x 10 for acetic acid. %3D 12. Calculate the pH of a buffer consisting of 0.590 moles of ammonia and 1.57 moles ammonium chloride. K, = 1.8 x 10 for ammonia.
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HCIO is 2.9 × 108. Complete Parts 1-4 before submitting your answer. 1 2 4 NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HCIO(aq) + OH(aq) 0.013 0.003 Before (mol) Change (mol) -0.013 0.013 After (mol) 0.010 0.003 H₂O(I) + CIO (aq) 0.037 0.003 0.040 RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040
based on the titration curves, compare the three curves and make conclusions based on their shapes.
A student was titrating a solution of HC HO₂ with a Sr(OH), solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. The value of Ka for HC,H,O₂ is 1.5 x 10%. Complete Parts 1-4 before submitting your answer. A student was titrating a solution of HC H,O₂ with a Sr(OH), solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. The value of Ka for HCH,O, is 1.5 × 10°. Complete Parts 1-4 before submitting your answer. 1 2 3 4 NEXT> 40.0 mL of a 0.200 M HCH,O, solution was titrated with 10.0 mL of 0.100 M Sr(OH)2 (a strong base). Fill in the BCA table with the appropriate value for each involved species to determine the moles of reactant and product after the…
100.0mL sample of 0.10M NH3 is titrated with 0.10M NHO3 . Determine the pH of the solution before the addition of any HNO3 . The Kb of NH3 is 1.8 x 10-5.
24. How many moles of NH,Br must be added to 2 L of 0.1 M NH,OH to form a buffer whose pH is 9.00? (K, of NH,OH = 1.76 x 0*)
Consider the titration of 45.0 mL of 1.0 M KOH with 1.0 M HCI. a. What is the total solution volume at the equivalence point? Volume mL b. Without doing detailed calculations, indicate the approximate pH at the beginning of the titration and at the equivalence point. pH at the beginning = pH at the equivalence point
analytical chemistry, please solve question 8- Determine the K sp of calcium fluoride (Ca*F_{2}) given that its molar solubility is 2.14 * 10 ^ 4 a) 9.98 * 10 ^ - 12 b) 3.92 *10^ *11 c) 5.42 * 10 ^ - 10 d) 6.74 * 10 ^ - 14