Lone Star CHEM 412 EXamNan - 9.A 25.00-mL sample of propionic acid, HC3HO2, of unknown concentration...
QUESTION 1 A 25.00-ml sample of propionic acid. HC H 50 of unknown concentration was titrated with 0.151 M KOH. The equivalence point was reached when 41.28 ml of base had been added. What is the hydroxide ion concentration at the equivalence point? K, for propionic acid is 13 x 10 at 25°C. O A 1.1 x 10 M 93-8.5 x 10 M OC 1.5x 10M OD. 1.0 x 10PM O E 1.1 X 10M
thanks 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.
Consider the titration of 15.00 mL of 0.1800 M propionic acid (CH3CH2COOH), with 0.1555 M NaOH. Ka for propionic acid is 1.34 X 10-5 a. What volume of base is required to reach the equivalence point? b. When the equivalence point is reached, sodium propionate ionizes in water. Write the equation for the reaction. C. What is the pH at the equivalence point? (20 points) Consider the titration of 15.00 mL of 0.1800 M propionic acid (CH3CH2COOH), with 0.1555 M...
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?
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...
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 student titrated a 25.00-mL sample of a solution containing an unknown weak, diprotic acid (H2A) with NaOH. If the titration required 17.73 mL of 0.1036 M NaOH to completely neutralize the acid, calculate the concentration (in M) of the weak acid in the sample. (a) 9.184 x 10‒4 M (b) 3.674 x 10‒2 M (c) 7.304 x 10‒2 M (d) 7.347 x 10‒2 M (e) 1.469 x 10‒1 M
A 15 mL sample of hydrofluoric acid, Ka=6.8x10^-4 was titrated with .475 M KOH. The equivalence point was reached after addition of 19.35 mL of base. Determine the molar concentration of the original hydrofluoric acid solution, and find the pH of the solution.
The next 9 questions are related to the titration of 25.00 mL of a 0.1000 M acetic acid solution with 0.1000 M KOH. 1.What is the initial pH of the analyte solution? 2.What volume of KOH is required to reach the equivalence point of the titration (in mL)? 3.How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT) 4.What is the volume of the solution at the equivalence point (in mL)? 5.What is...