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1. To determine the potassium content of a sample, 1.275 g of the sample was dissolved in water and reacted with sodium tetraphenylborate, NaB(C6H5)4. This reaction produced the insoluble precipitate potassium phenylborate, KB(CHs)4 (FM = 358.33 g/mol). The potassium phenylborate precipitate was weighed and had a mass of 0.955 g. Calculate the percentage by mass of K (FM = 39.098 g/mol) in the sample. (Inspired by problem 7-6 in the Harris text). %3D

1. To determine the potassium content of a sample, 1.275 g of the sample was dissolved in water and reacted with sodium tetraphenylborate, NaB(C6H5)4. This reaction produced the insoluble precipitate potassium phenylborate, KB(CHs)4 (FM = 358.33 g/mol). The potassium phenylborate precipitate was weighed and had a mass of 0.955 g. Calculate the percentage by mass of K (FM = 39.098 g/mol) in the sample. (Inspired by problem 7-6 in the Harris text). %3D

Chemistry
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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1. To determine the potassium content of a sample, 1.275 g of the sample was dissolved in water and reacted with sodium tetraphenylborate, NaB(C6H5)4. This reaction produced the insoluble precipitate potassium phenylborate, KB(C¿Hs)4 (FM = 358.33 g/mol). The potassium phenylborate precipitate was weighed and had a mass of 0.955 g. Calculate the percentage by mass of K (FM= 39.098 g/mol) in the sample. (Inspired by problem 7-6 in the Harris text).
Transcribed Image Text:1. To determine the potassium content of a sample, 1.275 g of the sample was dissolved in water and reacted with sodium tetraphenylborate, NaB(C6H5)4. This reaction produced the insoluble precipitate potassium phenylborate, KB(C¿Hs)4 (FM = 358.33 g/mol). The potassium phenylborate precipitate was weighed and had a mass of 0.955 g. Calculate the percentage by mass of K (FM= 39.098 g/mol) in the sample. (Inspired by problem 7-6 in the Harris text).
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