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A chemist is asked to separate the components of a mixture composed of 1.00 g each of the two compounds shown below. The chemist has access to the following bases: 10% aqueous NaHCO3 and 10% aqueous NaOH. Which base and how many mLs of the base (i.e., the minimum amount) are needed to completely separate these compounds from each other by liquid-liquid extraction?

A chemist is asked to separate the components of a mixture composed of 1.00 g each of the two compounds shown below. The chemist has access to the following bases: 10% aqueous NaHCO3 and 10% aqueous NaOH. Which base and how many mLs of the base (i.e., the minimum amount) are needed to completely separate these compounds from each other by liquid-liquid extraction?

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
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A chemist is asked to separate the components of a mixture composed of 1.00 g each of the two compounds shown below. The chemist has access to the following bases: 10% aqueous NaHCO3 and 10% aqueous NaOH. Which base and how many mLs of the base (i.e., the minimum amount) are needed to completely separate these compounds from each other by liquid-liquid extraction?

### Understanding pKa Values in Organic Compounds When studying acidity and basicity in organic chemistry, it’s essential to understand and compare the pKa values of various compounds. The pKa value indicates the strength of an acid, which in turn influences how it reacts with bases. #### Chemical Structures and their pKa Values In the image provided, there are two organic molecules and their corresponding pKa values: 1. **First Compound:** - **Structure:** This molecule consists of three hexagonal carbon rings fused together with a hydroxyl group (OH) attached. - **pKa Value:** 9.5 2. **Second Compound:** - **Structure:** This molecule consists of two hexagonal carbon rings fused together with an additional ring and a hydroxyl group (OH) attached via a methylene group (CH2). - **pKa Value:** 16 ### Analysis - **pKa Comparison:** The first compound with a pKa of 9.5 is more acidic than the second compound with a pKa of 16. This is because a lower pKa value indicates a stronger acid. ### Interactive Section - **Base Needed:** The text asks for the type of base needed to deprotonate these compounds. Generally, the base should be stronger than the acid for deprotonation to occur. - **mLs of Base Needed:** The specific volume of base required for the reaction, which would depend on the concentration and the amount of the acid being used, should also be determined. ### Application Understanding the pKa values is vital for predicting the outcome of acid-base reactions and for designing chemical syntheses in organic chemistry. For example, knowing that the first compound is more acidic, a weaker base could be used for its deprotonation compared to the second compound. By evaluating these properties and filling in the necessary details for "Base needed" and "mLs of base needed," students and chemists can make informed decisions during laboratory practices and research.
Transcribed Image Text:### Understanding pKa Values in Organic Compounds When studying acidity and basicity in organic chemistry, it’s essential to understand and compare the pKa values of various compounds. The pKa value indicates the strength of an acid, which in turn influences how it reacts with bases. #### Chemical Structures and their pKa Values In the image provided, there are two organic molecules and their corresponding pKa values: 1. **First Compound:** - **Structure:** This molecule consists of three hexagonal carbon rings fused together with a hydroxyl group (OH) attached. - **pKa Value:** 9.5 2. **Second Compound:** - **Structure:** This molecule consists of two hexagonal carbon rings fused together with an additional ring and a hydroxyl group (OH) attached via a methylene group (CH2). - **pKa Value:** 16 ### Analysis - **pKa Comparison:** The first compound with a pKa of 9.5 is more acidic than the second compound with a pKa of 16. This is because a lower pKa value indicates a stronger acid. ### Interactive Section - **Base Needed:** The text asks for the type of base needed to deprotonate these compounds. Generally, the base should be stronger than the acid for deprotonation to occur. - **mLs of Base Needed:** The specific volume of base required for the reaction, which would depend on the concentration and the amount of the acid being used, should also be determined. ### Application Understanding the pKa values is vital for predicting the outcome of acid-base reactions and for designing chemical syntheses in organic chemistry. For example, knowing that the first compound is more acidic, a weaker base could be used for its deprotonation compared to the second compound. By evaluating these properties and filling in the necessary details for "Base needed" and "mLs of base needed," students and chemists can make informed decisions during laboratory practices and research.
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