{"id":39883,"date":"2025-06-27T10:35:48","date_gmt":"2025-06-27T10:35:48","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=39883"},"modified":"2025-06-27T10:35:49","modified_gmt":"2025-06-27T10:35:49","slug":"what-is-the-conjugate-acid-of-hco3-2","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/what-is-the-conjugate-acid-of-hco3-2\/","title":{"rendered":"What is the conjugate acid of HCO3 2"},"content":{"rendered":"\n<p>What is the conjugate acid of HCO3 2 A. HCO32- B. CO3- c H2CO3 D CO32- E. HCO3<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct answer is <strong>C. H\u2082CO\u2083<\/strong>.<\/p>\n\n\n\n<p>To understand why, let us break this down using fundamental acid-base theory. The bicarbonate ion, HCO\u2083\u207b, acts as a <em>Br\u00f8nsted-Lowry base<\/em> because it can accept a proton (H\u207a). When it does, it becomes its conjugate acid, which contains one more proton than the base itself. Adding a proton to HCO\u2083\u207b forms <strong>H\u2082CO\u2083<\/strong>, known as carbonic acid.<\/p>\n\n\n\n<p>The conjugate acid\u2013base relationship is defined by the addition or removal of one proton. In this context:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Base:<\/strong> HCO\u2083\u207b<\/li>\n\n\n\n<li><strong>Conjugate acid:<\/strong> H\u2082CO\u2083<\/li>\n<\/ul>\n\n\n\n<p>This behavior is central in buffer systems. The carbonic acid\u2013bicarbonate buffer system, for example, helps regulate blood pH. Here, HCO\u2083\u207b can act either as a base or an acid depending on the environment, making it <strong>amphiprotic<\/strong>. However, when asked for the conjugate acid specifically, we consider the scenario in which HCO\u2083\u207b accepts a proton.<\/p>\n\n\n\n<p>Let us now look at the distractors:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>A. HCO\u2083\u00b2\u207b<\/strong> is not chemically valid, as HCO\u2083\u207b does not easily lose another electron to become doubly negative.<\/li>\n\n\n\n<li><strong>B. CO\u2083\u207b<\/strong> is not a standard species in acid-base chemistry.<\/li>\n\n\n\n<li><strong>D. CO\u2083\u00b2\u207b<\/strong> is the conjugate base of HCO\u2083\u207b, not its conjugate acid.<\/li>\n\n\n\n<li><strong>E. HCO\u2083\u207b<\/strong> is the original species, not its own conjugate acid.<\/li>\n<\/ul>\n\n\n\n<p>Therefore, the conjugate acid of HCO\u2083\u207b is <strong>H\u2082CO\u2083<\/strong>, formed by the addition of a single proton. This reaction is reversible and plays a key role in physiological pH regulation, particularly in respiratory and renal function.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1193.jpeg\" alt=\"\" class=\"wp-image-39894\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1193.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1193-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1193-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the conjugate acid of HCO3 2 A. HCO32- B. CO3- c H2CO3 D CO32- E. HCO3 The Correct Answer and Explanation is: The correct answer is C. H\u2082CO\u2083. To understand why, let us break this down using fundamental acid-base theory. The bicarbonate ion, HCO\u2083\u207b, acts as a Br\u00f8nsted-Lowry base because it can accept [&hellip;]<\/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-39883","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39883","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=39883"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39883\/revisions"}],"predecessor-version":[{"id":39895,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39883\/revisions\/39895"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39883"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39883"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39883"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}