QUESTION 1 A 25.00-ml sample of propionic acid. HC H 50 of unknown concentration was titrated...
Lone Star CHEM 412 EXamNan - 9.A 25.00-mL sample of propionic acid, HC3HO2, of unknown concentration was titrated with 0.183 M KOH The equivalence point was reached when 41.42 mL of base had been added. What is the hydroxide-ion concentration at the equivalence point? K, for propionic acid is 1.3 x 10-5 at 25°C. a. 1.0x 10-7 M b. 1.2 x 103 M c. 1.1 x 105 M Da S C d. 9.4 x 10 M (e>25Erehle y e. 1.5...
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Question 23 (2.5 points) Saved A 25.00-ml sample of propanoic acid, CH3CH2COOH, of unknown concentration was titrated with 0.143 M KOH. The equivalence point was reached when 35.28 mL of base had been added. What is the concentration of the propanoate ion at the equivalence point? 0.143 M 0.0837 M 0.202 M 0.128 M 0.147 M نعمه
a) A 25.00-mL sample of monoprotic acid was titrated with 0.0800 M potassium hydroxide solution. The equivalence point was reached after 18.75 mL of base was added. Calculate the concentration of the acid. b) A 15.00-mL sample of 0.120 M nitric acid was titrated with 0.0800 M potassium hydroxide. Calculate the pH of the sample when 10.00 mL of the base has been added.
Introductory Chemis Same 2018 "Name: 1. A 25.00-ml sample of an H SO, solution of unknown concentration is titrated with a 0.1322 M KOH solution. A volume of 41.22 ml. of KOH is required to reach the equivalence point. What is the concentration of the unknown H SO, solution? 2. What volume in milliliters of a 0.121 M sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 10.0-ml. sample of 0.102 M sulfuric...
What is the concentration of 25.00 mL of an unknown monoprotic acid if 18.24 mL of standardized 0.125 M sodium hydroxide solution was required to reach the equivalence point of the titration?
0.1945 M Question 14 0/1 point 25.00 ml of an unknown triprotic acid solution was titrated by 0.1729 M KOH. The third end point was observed when 44.55 mL KOH was delivered. What was the concentration of the unknown acid in the initial solution? 0.09180 M • 0.3081 M 0.1027 M 0.2628 M 0.03423 M
A 25.00 mL sample of an unknown sulfuric acid solution is titrated with 29.84 mL of a sodium hydroxide solution with a concentration of 0.150 M NaOH. What is the concentration of the sulfuric acid solution? H.SO.(aq) + 2NaOH(aq) → Na2SO4 (aq) + 2 H2O(1) Show your work Final Answer
P19. (Sec. 16.4) Two Part Titration Question: A propionic acid solution, HC3H5O2, will be titrated with a sodium hydroxide, NaOH, solution. Part 1: What is the pH of the solution after adding 36 mL of 0.15 M NaOH to 50 mL of 0.108 M HC3H5O2? [Hint: Equivalence Point). Part 2: What is the pH of the solution after adding 75 mL of 0.15 M NaOH to the 50 mL of 0.108 M HC3H5O2 solution? (Propionic Acid: Ka = 1.3 x...
An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH. What is the concentration of the acid? H3PO4 (aq) + 3 KOH(aq) - K3PO4 (aq) + 3 H2O) Initial volume of KOH solution 1.03 mL Final volume of KOH solution 15.02 mL Original volume of H3PO4 solution 24.68 mL O 0.001260M 0.05104 M 0.1531 M 0.4593M
An unknown concentration of phosphoric acid is titrated to its equivalence point with 0.2701 M KOH. What is the concentration of the acid? H3PO4 (aq) + 3 KOH(aq) – K3PO4 (aq) + 3 H200) Initial volume of KOH solution 1.03 mL Final volume of KOH solution 15.02 ml Original volume of H3PO, solution 24.68 ml O 0.001260M 0.4593 M 0.05104 M 0.1531M