calculations for: concentration of the unknown acid and values for pKa and Ka. Part E: pH...
Follow up questions 01. Find the accepted values for the pKa and Ka of acetic acid. How well do the accepted values compare with your calculated values? Explain. Lab 7 Determining Ka by the Half-Titration of a Weak Acid 1. Data table Titration Results NaOH volume at equivalence point NaOH volume at half equivalence point pH at the equivalence point pH at half equivalence point pKa of acetic acid Ka of acetic acid Trial 1 22.72 11.36 7.63 Trial2 23.26...
Data Table 2: Titration Curve Values pH Value Trial 1 pH Value Trial 2 pH Value (Average) Drops NaOH Added Half- Equivalence Point Equivalence Point ? ? ? ? ? ? 0 2.5 2.5 2.5 10 4.5 4.5 4.5 20 4.5 4.5 4.5 30 4.5 4.5 4.5 40 4.5 4.5 4.5 50 O7 5 5 60 5.5 5.5 5.5 70 6 6.5 6.25 80 12.5 13 12.75 90 13.5 13.5 13.5 100 13.5 13.5 13.5 110 14 14 14 120...
Find pKa of unkown acid
Find identitiy of unkown acid
83 Lab 11: Analysis of an unknown Acid Trial 2 Trial Volume of NaOH added to reach the equivalence point Volume of No added to reach the equivalence point ImL 4.925 4.925 pH at the equivalence point pk of unknown acid Average pk, of unknown acid: Possible identity of unknown weak acid: Molarity of unknown acid (show calculations): Average molarity of unknown acid Acid-Base Titration
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Part B: Determination of acid ionization constant (K.) and molar mass of an u Concentration of NaOH (mol/L) from bottle: 0.1053 Mass concentration of unknown acid (g/L) from bottle: 3.120 pH of unknown acid solution: 228 from pH meter. 1) Titration of unknown acid using indicator only Trial 2 Trial 1 1.593 30.851 090909 ml Mass of empty beaker Mass of beaker + unknown acid solution Mass of unknown acid solution Volume of unknown acid solution Initial volume of...
Based on the following information...
please answer A. B. and C.
TITRATION OF A WEAK ACID TRIAL #1 equivalence point halfway point 25 VOLUME OF BASE ADDED 30 35 40 TITRATION OF A WEAK ACID TRIAL #2 1 equivalence point Hd half-way point s 10 15 30 35 40 45 20 25 VOLUME OF BASE ADDED Trial 1 Trial 2 Mass of oxalic acid 0.2039 pH at equivalence point a Mass of oxalic acid 0.2099 at equivalence point nt 8,5...
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M NaOH. If a 100.-mL sample of the acid solution required exactly 10. mL of the NaOH solution to reach the equivalence point, what was the original concentration of the weak acid? 2) During the titration on problem (2B), after 5.0 mL of NaOH addition, the pH = 3.68. What is the Ka of the weak acid? please show steps i have an exam tomorrow
(1) A weak acid, HA, has a Ka of 6.5 x 10-6 and a concentration of 0.25 M. 25.5 mL of this weak acid is titrated with 0.10 M NaOH. What is the pH of the solution at the equivalence point? Report your answer with 3 decimal places. (2) The concentration of 16.6 mL of HCl is determined by titrating with NaOH. The titration reaches its endpoint after adding 18.4 mL of 0.829 M NaOH. What is the concentration of...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the primary standard KHP (potassium hydrogen phthalate, KHC8H4O4) had a potassium iodide impurity of approximately one percent by mass. How would this have influenced the calculated molarity of your sodium hydroxide solution? Would your calculated value be too low, too high, or unchanged? Explain your answer. b. Sketch a typical titration curve for a monoprotic weak acid titrated with a strong base. Label the axes...
DAY_ _INS LABORATORY REPORT FOR Part I Standardization of NaOH Trial 1 Weight of bottle + "KHP" 21.5350 Weight of bottle 20.7995 Weight of "KHP" used 0.8055 Equiv. Volume of NaOH from plot 3125 Equivalence Volume of NaOH 3125 (Equiv. Volume NaOH from plot minus initial volume NaOH) Molarity of NaOH 0.126 Average Molarity 0.126 M Part II - Titration of a Weak Acid Unknown weak acid code Trial 1 Trial 2 Volume of unknown acid 25.00 Equiv. Volume of...
A 0.100 molar solution of weak acid HA has pH of 2.45 What is pka? Hint, find [H+] from pH and plug it into into ICE as 'X' HA (+H20) А" <> H30* 0.100 M 0 0 С E 0.100 - X х х solve for Ka, then pka Ka = [H30*1 [A]/[HA] 39 24 6.1 45 5.4 Consider the titration of 25.00 ml of 0.100 MHA with 25.0 0.100 M NaOH. HA +H20 --> A™ + H307 The Ka...