urgent help plese **Question:** Which of the following acids has the lowest pKa?**Options:** - **A:** An acid with the structure of 2-Chloropropanoic acid.- **B:** An acid with the structure of 3-Chloropropanoic acid.- **C:** An acid with the structure of 2-Chloro-2-methylpropanoic acid.- **D:** An acid with the structure of 2-Chloroethanol.**Explanation of Structures:**- **Option A:** The molecular structure shows a chlorine atom attached to the second carbon in the chain, with a carboxylic acid group at the end.- **Option B:** The structure has a chlorine atom attached to the third carbon, with a carboxylic acid group at the end.- **Option C:** The structure includes a chlorine atom attached to a tertiary carbon (with a methyl group) adjacent to a carboxylic acid group.- **Option D:** The structure shows a chlorine atom attached to the second carbon, with an alcohol group at the end.**Important Concepts:**- pKa is a measure of the strength of an acid in solution; the lower the pKa, the stronger the acid.- Electronegative groups such as chlorine can increase acid strength when located closer to the carboxylic group due to inductive effects.**Conclusion:**To determine which acid has the lowest pKa, consider the position and effect of chlorine in each structure on the stability of the conjugate base.

Answered: Which of the following acids has the…

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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Step 1-Introduction

An acid is a substance that can increase the concentration of hydrogen ions or $H^{+}$ ions in an aqueous solution. If the dissocation of the acid is not 100%, then the acid is termed as the weak acid. The dissociation reaction of the weak acids in an aqueous solution should be represented by the equilibrium reaction.

Moreover, the extent of the dissocation of the weak acid can be denoted by the dissociation constant, $K a$ . Mathematically, the magnitude of $K a$ is related to $p K a$ as follows:

$p K a = - \log_{10} K a$

Higher the value of $K a$ or lower the value of $p K a$ indicates the greater will be the dissociation of the acid (stronger acid).