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1. The solid acids chosen for the analysis were typically monoprotic acidic salts such as NaIISO₁. KIISO₁. etc. Explain why such salts behave as strong enough acids to be titrated with NaOH using phenolphthalein as indicator. 2. Commercial vinegar is generally 5.0+ 0.5% acetic acid by weight. Assuming this to be the true value for your unknown, by how much were you in error in your analysis? 1.62./.

1. The solid acids chosen for the analysis were typically monoprotic acidic salts such as NaIISO₁. KIISO₁. etc. Explain why such salts behave as strong enough acids to be titrated with NaOH using phenolphthalein as indicator. 2. Commercial vinegar is generally 5.0+ 0.5% acetic acid by weight. Assuming this to be the true value for your unknown, by how much were you in error in your analysis? 1.62./.

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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Could you please help me with both questions. Please define the first question and for the second question how do I obtain the percent error. The measured value I found is 1.62%. Thank You!
1. The solid acids chosen for the analysis were typically monoprotic acidic salts such as NalISO₁, KIISO₁. etc. Explain why such salts behave as strong enough acids to be titrated with NaOH using phenolphthalein as indicator. 2. Commercial vinegar is generally 5.0+ 0.5% acetic acid by weight. Assuming this to be the true value for your unknown, by how much were you in error in your analysis? 1.62./.
Transcribed Image Text:1. The solid acids chosen for the analysis were typically monoprotic acidic salts such as NalISO₁, KIISO₁. etc. Explain why such salts behave as strong enough acids to be titrated with NaOH using phenolphthalein as indicator. 2. Commercial vinegar is generally 5.0+ 0.5% acetic acid by weight. Assuming this to be the true value for your unknown, by how much were you in error in your analysis? 1.62./.
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