HSO3 \u00af is amphoteric. For H2SO3 Ka1 = 1.4 x 10-2 and Ka2 = 6.3 x 10-8 . a. Write a chemical reaction showing HSO3 \u00af acting as an acid in water. b. Write a chemical reaction showing HSO3 \u00af acting as a base in water. c. Will an aqueous solution of NaHSO3 be acidic, basic, or neutral?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Answer:<\/strong><\/p>\n\n\n\n a. When HSO\u2083\u207b acts as an acid in water: b. When HSO\u2083\u207b acts as a base in water: c. An aqueous solution of NaHSO\u2083 will be slightly acidic.<\/p>\n\n\n\n Explanation:<\/strong><\/p>\n\n\n\n The HSO\u2083\u207b ion, known as hydrogen sulfite or bisulfite, is amphoteric, meaning it can act as both an acid and a base. This behavior is due to its structure, where it has both a proton (H\u207a) that it can donate, and a negatively charged oxygen that allows it to accept an additional proton.<\/p>\n\n\n\n In part (a), we see HSO\u2083\u207b acting as an acid, donating a proton to water to form SO\u2083\u00b2\u207b and H\u2083O\u207a. The formation of H\u2083O\u207a ions demonstrates that HSO\u2083\u207b is capable of increasing the solution’s acidity.<\/p>\n\n\n\n In part (b), HSO\u2083\u207b acts as a base, accepting a proton from water to form H\u2082SO\u2083 (sulfurous acid) and OH\u207b. The generation of OH\u207b ions demonstrates that HSO\u2083\u207b can also increase the basicity of the solution.<\/p>\n\n\n\n To determine if an aqueous solution of NaHSO\u2083 is acidic, basic, or neutral, we need to consider the relative strengths of HSO\u2083\u207b as an acid and as a base. The acidity of HSO\u2083\u207b is quantified by its acid dissociation constants, ( K_a1 = 1.4 \\times 10^{-2} ) and ( K_a2 = 6.3 \\times 10^{-8} ). The first dissociation constant (Ka1) is larger, indicating that HSO\u2083\u207b has a stronger tendency to lose a proton and act as an acid rather than accept a proton and act as a base.<\/p>\n\n\n\n Therefore, in an aqueous solution, HSO\u2083\u207b will predominantly release H\u207a ions, making the solution slightly acidic.<\/p>\n","protected":false},"excerpt":{"rendered":" HSO3 \u00af is amphoteric. For H2SO3 Ka1 = 1.4 x 10-2 and Ka2 = 6.3 x 10-8 . a. Write a chemical reaction showing HSO3 \u00af acting as an acid in water. b. Write a chemical reaction showing HSO3 \u00af acting as a base in water. c. Will an aqueous solution of NaHSO3 be acidic, […]<\/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-163035","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/163035","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=163035"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/163035\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=163035"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=163035"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=163035"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
[
\\text{HSO}_3^- + \\text{H}_2\\text{O} \\rightarrow \\text{SO}_3^{2-} + \\text{H}_3\\text{O}^+
]<\/p>\n\n\n\n
[
\\text{HSO}_3^- + \\text{H}_2\\text{O} \\rightarrow \\text{H}_2\\text{SO}_3 + \\text{OH}^-
]<\/p>\n\n\n\n