Correct Order of Br\u00f8nsted Acidity (Strongest to Weakest):<\/h3>\n\n\n\n
HBr > HF > H2O > NH3 > CH4<\/strong><\/p>\n\n\n\n Now, match this with the given compounds: Br\u00f8nsted acids are substances that donate protons (H\u207a ions). The strength of a Br\u00f8nsted acid depends on how easily it can donate this proton. This is influenced by several factors including bond strength, electronegativity of the bonded atom, and the stability of the conjugate base formed after deprotonation.<\/p>\n\n\n\n Let us analyze the compounds in the list:<\/p>\n\n\n\n In summary, acid strength generally increases as the stability of the conjugate base increases and the bond holding the proton becomes weaker. This explains the ranking: Arrange the given compounds based on their relative Br\u00f8nsted acidities. Strongest Br\u00f8nsted acid H-Br H-OH H-NH2 H-F H-CH3 Weakest Br\u00f8nsted acid The Correct Answer and Explanation is: Correct Order of Br\u00f8nsted Acidity (Strongest to Weakest): HBr > HF > H2O > NH3 > CH4 Now, match this with the given compounds:H\u2013Br > H\u2013F > H\u2013OH […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-238151","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238151","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=238151"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238151\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=238151"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=238151"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=238151"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
H\u2013Br > H\u2013F > H\u2013OH > H\u2013NH2 > H\u2013CH3<\/strong><\/p>\n\n\n\nExplanation<\/h3>\n\n\n\n
\n
This is a strong acid. The H\u2013Br bond is weak and easily broken, and the Br\u207b ion is very stable due to its large size and ability to disperse negative charge. Therefore, H\u2013Br donates protons easily.<\/li>\n\n\n\n
Although fluorine is very electronegative, the H\u2013F bond is extremely strong. This makes HF less willing to donate a proton than HBr. However, HF is still more acidic than water due to the high electronegativity of fluorine stabilizing the resulting F\u207b ion.<\/li>\n\n\n\n
Water is a very weak acid. It can donate a proton to form OH\u207b, but this does not happen easily compared to strong acids. The oxygen in OH\u207b is electronegative and can stabilize the negative charge, but not as effectively as halide ions.<\/li>\n\n\n\n
The nitrogen atom is less electronegative than oxygen and halogens, making the NH2\u207b conjugate base less stable. As a result, ammonia is a weaker acid than water.<\/li>\n\n\n\n
Methane is an extremely weak acid. Carbon is not electronegative enough to stabilize a negative charge, and the C\u2013H bond is very strong. The CH3\u207b ion is highly unstable, making methane essentially non-acidic.<\/li>\n<\/ol>\n\n\n\n
HBr > HF > H2O > NH3 > CH4<\/strong>.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner5-695.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"