Acetic Acid Dissociates As, CH3COOH →CH3COO - Vedantu

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• Acetic acid dissociates as CH3...

AnswerQuestion Answers for Class 12Class 12 BiologyClass 12 ChemistryClass 12 EnglishClass 12 MathsClass 12 PhysicsClass 12 Social ScienceClass 12 Business StudiesClass 12 EconomicsQuestion Answers for Class 11Class 11 EconomicsClass 11 Computer ScienceClass 11 BiologyClass 11 ChemistryClass 11 EnglishClass 11 MathsClass 11 PhysicsClass 11 Social ScienceClass 11 AccountancyClass 11 Business StudiesQuestion Answers for Class 10Class 10 ScienceClass 10 EnglishClass 10 MathsClass 10 Social ScienceClass 10 General KnowledgeQuestion Answers for Class 9Class 9 General KnowledgeClass 9 ScienceClass 9 EnglishClass 9 MathsClass 9 Social ScienceQuestion Answers for Class 8Class 8 ScienceClass 8 EnglishClass 8 MathsClass 8 Social ScienceQuestion Answers for Class 7Class 7 ScienceClass 7 EnglishClass 7 MathsClass 7 Social ScienceQuestion Answers for Class 6Class 6 ScienceClass 6 EnglishClass 6 MathsClass 6 Social ScienceQuestion Answers for Class 5Class 5 ScienceClass 5 EnglishClass 5 MathsClass 5 Social ScienceQuestion Answers for Class 4Class 4 ScienceClass 4 EnglishClass 4 MathsAcetic acid dissociates as, ${\text{C}}{{\text{H}}_3}{\text{COOH }} \to {\text{C}}{{\text{H}}_3}{\text{CO}}{{\text{O}}^ - }{\text{ + }}{{\text{H}}^ + }$ . If a little amount of sodium acetate is added to its aqueous solution then:A)the acid dissociates furtherB)the ${{\text{H}}^ + }$ ion concentration increasesC)the acid dissociation is suppressedD)the equilibrium is unaffectedAnswerVerified591.6k+ viewsHint: To solve this question, it is required to have knowledge about the common ion effect and how pH of the solution is affected. The common-ion effect refers to the decrease in solubility of an ionic precipitate by the addition to the solution of a soluble compound with an ion in common with the precipitate. pH of a solution is dependent on the concentration of hydrogen ions in a solution.Complete step by step answer:As we know that, the common ion effect occurs when a compound containing an ion which is common to one of the ion present in the solution is added to the solution, it results in decrease in solubility of that ion. This occurs according to the Le-Chatelier principle. When the solution dissociates and will be present at equilibrium the rate of forward and backward reaction will be the same. If a compound is added with a common ion, the concentration of that ion in the solution increases and thus, the equilibrium will shift in the opposite direction of the dissociation. Thus, the extra ions will precipitate in the solution.In the question given, acetate ion is present in equilibrium. When sodium acetate is added to the solution, it will dissociate as:${\text{C}}{{\text{H}}_3}{\text{COONa}} \to {\text{CHCO}}{{\text{O}}^ - }{\text{ + }}{\text{ N}}{{\text{a}}^ + }$Thus, the concentration of acetate ions will increase in the solution. According to Le-Chartelier’s principle, the equilibrium will shift backwards. As a result, the concentrate of the acetate ion as well as the hydrogen ion will decrease. This means that the dissociation of the acid will be suppressed.$\therefore $ The correct option is option C, i.e. the acid dissociation is suppressed.Note:In this question, as the concentration of hydrogen ions will decrease, the pH of the solution will also increase. This means the solution will become less acidic. The solution of a weak acid and its salt is also known as an acidic buffer solution. This means that the pH of the solution will remain unaffected by addition of base in the solution until a certain amount.Recently Updated PagesMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for SuccessMaster Class 11 Chemistry: Engaging Questions & Answers for SuccessMaster Class 11 Business Studies: Engaging Questions & Answers for SuccessMaster Class 11 Computer Science: Engaging Questions & Answers for SuccessMaster Class 11 Economics: Engaging Questions & Answers for SuccessMaster Class 11 Social Science: Engaging Questions & Answers for SuccessMaster Class 11 English: Engaging Questions & Answers for SuccessMaster Class 11 Chemistry: Engaging Questions & Answers for Success

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