Calculate the pH at the following points in a titration of 40 mL (0.040 L) of...
Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.132 M acrylic acid (K= 5.6 x10) with 0.132 M KOH. (Assume Kw = 1.01 x 1014.) (a) no KOH added 4.0 (b) 20. mL of KOH solution added 4.0 (c) 39 mL of KOH solution added 4.0 (d) 40. mL of KOH solution added 4.0 (e) 41 mL of KOH solution added 4.0
Calculate the pH at the following points in a titration of 40 ml (0.040 L) of 0.100 M barbituric acid (Kà= 9.8x10^-5) with 0.100 M KOHa. no KOH addedb. 20 ml of KOH solution added c. 39 ml of KOH solution addedd. 40 ml of KOH solution addede. 41 ml of KOH solution added
The next three (3) problems deal with the titration of 431 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.7 M KOH. What is the pH of the solution at the 2nd equivalence point? What will the pH of the solution be when 0.2045 L of 1.7 M KOH are added to the 431 mL of 0.501 M carbonic acid? How many mL of the 1.7 M KOH are needed...
QUESTION 14 Calculate the pH at each of the following points for the titration of 50.0 mL of 0.320 M HA with 0.320 M KOH. The Ka for HA is 6.5x10-6 at 0 mL of KOH added the pH = at 15.0 mL of KOH added the pH- at 25.0 mL of KOH added the pH = at 50.0 mL of KOH added the pH = at 60.0 mL of KOH added the pH =
3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka = 1.80 x 10-4) with 0.100 M NaOH: VNaOH = 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VNAOH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 59.3 mlL of 0.335 M nitrous acid (K-4.5x104) by 0.335 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.0 mL of KOH
20. Calculate the pH at the following points in the titration of 25.00 ml of 0.400 M HCIO with 0.400 M KOH. Ka=3.0x10 a. Before the addition of any KOH b. After the addition of 5.00 ml of 0.400 M KOH c. After the addition of 12.50 ml of 0.400 M KOH d. After the addition of 25.00 ml of 0.400 M KOH e. After the addition of 30.00 ml of 0.400 M KOH
Calculate the pH at each of the following points along the titration of 25.0 mL of 0.185 M HNO2 with 0.185 M NaOH. [K, = 4.3x10-61 pka = -109(4.3x10-6 - 5136 5.36 +log 185/. 185 = 5. 4 5 20 0 5.0 odstoty D oonboe 3.1 HOMO 4 5: 2 . SI. OLD 0 mL of NaOH added pH = _ 8.5 mL of NaOH added pH = 12.5 mL of NaOH added pH = 22.0 mL of NaOH added...
- Calculating the pH at equivalence of a titration A chemist titrates 180.0 ml of a 0.1215 M nitrous acid (HNO) solution with 0.5478 M KOH solution at 25 "C. Calculate the pH at equivalence. The pk of nitrous acid is 3.35. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. PHU X 5 ?
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb = 4.4 x 104, with a 0.200 M HCl solution before any acid is added, after adding 0.0mL, 15.0 mL, 25.0 mL, 35.0 mL and 50 mL of HCl. Plot (using graph paper) the titraticn curve from your results (label all relevant points). 1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb =...