Question 1 3 pts Question 2 6 pts In the laboratory you dissolve 16.6 g of potassium hydroxide in a volumetric flask and add water to a total volume of 500 mL. Question 3 6 pts What is the molarity of the solution? M. Question 4 3 pts What is the concentration of the potassium cation? M. Question 5 6 pts What is the concentration of the hydroxide anion? М. Question 6 4 pts Question 7 4 pts Submit Answer Try Another Version 1 item attempt remaining Question 8 4 pts Question 9 3 pts

Question 1 3 pts Question 2 6 pts In the laboratory you dissolve 16.6 g of potassium hydroxide in a volumetric flask and add water to a total volume of 500 mL. Question 3 6 pts What is the molarity of the solution? M. Question 4 3 pts What is the concentration of the potassium cation? M. Question 5 6 pts What is the concentration of the hydroxide anion? М. Question 6 4 pts Question 7 4 pts Submit Answer Try Another Version 1 item attempt remaining Question 8 4 pts Question 9 3 pts

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 23QAP

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In the final titration, the amount of salicylic acid (the active ingredient) in aspirin is calculated. If 0.1000 grams of aspirin tablets are dissolved in water and titrated with the NaOH from an initial volume of 15.90mL to a final volume of 18.80mL, what is the % mass of salicylic acid in the aspirin? HINTS: You will need to use your NaOH concentration from the 1st question: 0.1186 Mass percent here would be mass of (salicylic acid/mass of aspirin) x 100% You will need to use the molar mass of salicylic acid
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1. Forgetful Freddy weighed his KHP sample, but forgot to bring his report sheet along, so he recorded the mass of KHP on a paper towel. During his titration, which required18.46 mL of base, he spilled some base on his hands. He remembered to wash his hands, but forgot about the data on the towel, and used it to dry his hands. When he went to calculate the molarity of his base, Freddy discovered that he didn’t have the mass of his KHP. His kindhearted instructor told Freddy that his base was 0.2987 M. Calculate the mass of Freddy’s KHP sample. 2. What mass of solid NaOH would be needed to make 645 mL of Freddy’s NaOH solution?
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