{"id":25857,"date":"2025-06-19T07:09:02","date_gmt":"2025-06-19T07:09:02","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=25857"},"modified":"2025-06-19T07:09:04","modified_gmt":"2025-06-19T07:09:04","slug":"identify-the-conjugate-base-for-each-acid","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/identify-the-conjugate-base-for-each-acid\/","title":{"rendered":"Identify the conjugate base for each acid."},"content":{"rendered":"\n<p>Identify the conjugate base for each acid. conjugate base of<br>: \\boxed{\\hspace{1cm}}$<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"700\" height=\"335\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-36.png\" alt=\"\" class=\"wp-image-25859\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-36.png 700w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/image-36-300x144.png 300w\" sizes=\"auto, (max-width: 700px) 100vw, 700px\" \/><\/figure>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-green-cyan-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The <strong>conjugate base<\/strong> of H\u2082S is <strong>HS\u207b<\/strong>.<\/p>\n\n\n\n<p>When identifying a conjugate base, we follow the principle that a conjugate base forms when an acid donates a proton (H\u207a). This idea comes from the Bronsted-Lowry theory, which defines acids as proton donors and bases as proton acceptors.<\/p>\n\n\n\n<p>Hydrosulfuric acid (H\u2082S) is a weak diprotic acid, meaning it can donate two protons, but it does so step by step. The first deprotonation involves H\u2082S donating one proton to produce the hydrosulfide ion (HS\u207b):<\/p>\n\n\n\n<p><strong>H\u2082S \u2192 H\u207a + HS\u207b<\/strong><\/p>\n\n\n\n<p>Here, H\u2082S acts as the acid because it donates a proton, and HS\u207b is its conjugate base\u2014the species remaining after the loss of a proton. This conjugate base is capable of accepting a proton again, returning to H\u2082S under suitable conditions.<\/p>\n\n\n\n<p>Conceptually, the acid and its conjugate base form a pair that is linked by the gain or loss of a single hydrogen ion. The stronger the acid, the weaker its conjugate base, and the weaker the acid, the stronger its conjugate base. Since H\u2082S is a weak acid, HS\u207b is considered a relatively strong conjugate base by comparison, although not among the strongest bases overall.<\/p>\n\n\n\n<p>Understanding conjugate pairs helps in predicting reaction directions, analyzing buffer systems, and calculating equilibrium constants. In buffer solutions, weak acids and their conjugate bases work together to resist drastic changes in pH. For instance, if HS\u207b is present in solution, it can help moderate acidity by accepting excess protons.<\/p>\n\n\n\n<p>To summarize: the conjugate base of H\u2082S is HS\u207b, created when the acid donates one hydrogen ion. This transformation reflects the foundational ideas in acid-base chemistry and highlights the reversible nature of proton transfer reactions.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"722\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-4.jpeg\" alt=\"\" class=\"wp-image-25861\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-4.jpeg 722w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner10-4-212x300.jpeg 212w\" sizes=\"auto, (max-width: 722px) 100vw, 722px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Identify the conjugate base for each acid. conjugate base of: \\boxed{\\hspace{1cm}}$ The Correct Answer and Explanation is: The conjugate base of H\u2082S is HS\u207b. When identifying a conjugate base, we follow the principle that a conjugate base forms when an acid donates a proton (H\u207a). This idea comes from the Bronsted-Lowry theory, which defines acids [&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-25857","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/25857","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=25857"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/25857\/revisions"}],"predecessor-version":[{"id":25862,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/25857\/revisions\/25862"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=25857"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=25857"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=25857"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}