Which of the following occurs when HCl is added to a buffer containing (CH3)3N and (CH3)3NH+?<\/p>\n\n\n\n
The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n Correct Answer:<\/strong> Explanation (300 words):<\/strong> When a strong acid like hydrochloric acid (HCl)<\/strong> is added to this buffer, it introduces hydrogen ions (H\u207a)<\/strong> into the solution. These hydrogen ions would normally lower the pH sharply in a solution that lacks a buffering component. However, the role of a buffer is to resist changes in pH<\/strong> by neutralizing added acids or bases.<\/p>\n\n\n\n In this buffer system, (CH\u2083)\u2083N<\/strong> acts as the base. It reacts with the added H\u207a ions<\/strong> from HCl according to this chemical reaction:<\/p>\n\n\n\n (CH\u2083)\u2083N + H\u207a \u2192 (CH\u2083)\u2083NH\u207a<\/strong><\/p>\n\n\n\n This reaction shows that the base (CH\u2083)\u2083N accepts the proton (H\u207a) and gets converted into its conjugate acid (CH\u2083)\u2083NH\u207a. Because the base component of the buffer consumes the added acid, the pH does not change significantly. Only a small change occurs due to the altered ratio of base to conjugate acid.<\/p>\n\n\n\n This is the key function of a buffer system: it uses the components present to neutralize added acids or bases. The result is a solution that maintains a relatively constant pH. Since the added HCl reacts specifically with (CH\u2083)\u2083N and not with (CH\u2083)\u2083NH\u207a, the correct answer is that (CH\u2083)\u2083N reacts with HCl to form (CH\u2083)\u2083NH\u207a<\/strong>, preserving the buffering action.<\/p>\n\n\n\n This behavior is typical of acid-base equilibrium reactions in buffer solutions, and it demonstrates the importance of having both components of the conjugate pair present to handle incoming acids or bases effectively.<\/p>\n","protected":false},"excerpt":{"rendered":" Which of the following occurs when HCl is added to a buffer containing (CH3)3N and (CH3)3NH+? The correct answer and explanation is: Correct Answer:(CH\u2083)\u2083N reacts with HCl to form (CH\u2083)\u2083NH\u207a. Explanation (300 words):A buffer solution is made from a weak base and its conjugate acid or from a weak acid and its conjugate base. In […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-38574","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38574","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=38574"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38574\/revisions"}],"predecessor-version":[{"id":38575,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/38574\/revisions\/38575"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=38574"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=38574"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=38574"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
(CH\u2083)\u2083N reacts with HCl to form (CH\u2083)\u2083NH\u207a.<\/strong><\/p>\n\n\n\n
A buffer solution is made from a weak base and its conjugate acid or from a weak acid and its conjugate base. In this case, the buffer contains trimethylamine<\/strong> ((CH\u2083)\u2083N), which is a weak base, and its conjugate acid trimethylammonium ion<\/strong> ((CH\u2083)\u2083NH\u207a).<\/p>\n\n\n\n