Answered: concentration

Science

Chemistry

concentration

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...

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A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1488 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 14.11 mL of the standard solution. What is the concentration of the original sulfuric acid solution?
An aqueous solution of hydroiodic acid is standardized by titration with a 0.139 M solution of barium hydroxide.If 13.4 mL of base are required to neutralize 29.3 mL of the acid, what is the molarity of the hydroiodic acid solution?
What volume in mL of 0.1366 M NaOH is required to titrate 15.00 mL of 0.1021 M acetic acid (HAc)?
You titrated a 21.00 mL solution of 0.0500 M oxalic acid with a freshly prepared solution of KMnO4. If it took 49.49 mL of this solution, what was the molarity of the KMnO4?
An aqueous solution of perchloric acid is standardized by titration with a 0.130 M solution of barium hydroxide.If 13.6 mL of base are required to neutralize 10.7 mL of the acid, what is the molarity of the perchloric acid solution?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1463 M0.1463 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 18.47 mL18.47 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: ___________M
50.00 mL of a diprotic acid solution, whose concentration is unknown, is titrated with 12.54 mL of NaOH 0.135 M. What is the concentration of the diprotic acid?
You titrated a 25.00 mL solution of 0.0800 M oxalic acid with a freshly prepared solution of KMnO4. If it took 45.99 mL of this solution, what was the molarity of the KMnO4?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1437 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 18.80 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: M
What volume in mL of 0.1312 M NAOH is required to titrate 15.00 mL of 0.1021 M acetic acid (HAc)? mL
A 0.430 M solution of KCl needs to be prepared through dilution. A 2.00 M stock solution will be added to a 0.250 L volumetric flask and then water will be added to the 0.250 L mark. Determine the volume (in mL) of the 2.00 M stock solution of KCl needed to produce this solution.
A 25.00-mL sample of a commercial vinegar is diluted with de-ionized water to 100.0 mL. Then, a 10.00-mL portion of the dilute vinegar solution is titrated with 0.1125 M NaOH solution, and the titration requires 18.50 mL of the NaOH solution to neutralize the acetic acid in the dilute vinegar sample. Calculate the molar concentration of acetic acid in the original vinegar sample (before dilution). The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> NaC2H3O2(aq) + H2O(g) (A) 0.8325 M (B) 0.2081 M (C) 0.3330 M (D) 0.2432 M