Both HCO3^- and HS^- are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n Both bicarbonate (( \\text{HCO}_3^- )) and hydrogen sulfide (( \\text{HS}^- )) are amphoteric species, meaning they can act both as acids and as bases, depending on the context. Amphoteric substances have the ability to donate or accept protons (H(^+)).<\/p>\n\n\n\n As an acid, ( \\text{HCO}_3^- ) can donate a proton (H(^+)) to form carbonate (( \\text{CO}_3^{2-} )):<\/p>\n\n\n\n [ As a base, ( \\text{HCO}_3^- ) can accept a proton (H(^+)) to form carbonic acid (( \\text{H}_2\\text{CO}_3 )):<\/p>\n\n\n\n [ As an acid, ( \\text{HS}^- ) can donate a proton to form sulfide (( \\text{S}^{2-} )):<\/p>\n\n\n\n [ As a base, ( \\text{HS}^- ) can accept a proton to form hydrogen sulfide (( \\text{H}_2\\text{S} )):<\/p>\n\n\n\n [ Bicarbonate (( \\text{HCO}_3^- )) and hydrogen sulfide (( \\text{HS}^- )) are amphoteric because they both have the ability to either donate or accept a proton. This behavior depends on the surrounding conditions. In an environment where there is a higher concentration of H(^+) ions (such as in an acidic solution), both bicarbonate and hydrogen sulfide will act as bases, accepting protons to form their respective acids (( \\text{H}_2\\text{CO}_3 ) and ( \\text{H}_2\\text{S} )).<\/p>\n\n\n\n Conversely, in a basic environment where the concentration of H(^+) ions is low, both ( \\text{HCO}_3^- ) and ( \\text{HS}^- ) can donate protons to form their conjugate bases (( \\text{CO}_3^{2-} ) and ( \\text{S}^{2-} )). This dual ability to act as either an acid or a base makes these substances amphoteric, which is an important characteristic in various biological and chemical systems, such as in the regulation of blood pH and in sulfur-based chemical reactions.<\/p>\n","protected":false},"excerpt":{"rendered":" Both HCO3^- and HS^- are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base. The correct answer and explanation is : Both bicarbonate (( \\text{HCO}_3^- )) and hydrogen sulfide (( \\text{HS}^- )) are amphoteric species, meaning they can […]<\/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-210754","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210754","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=210754"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/210754\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=210754"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=210754"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=210754"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Bicarbonate (( \\text{HCO}_3^- )) as an Acid:<\/h3>\n\n\n\n
\\text{HCO}_3^- \\rightarrow \\text{CO}_3^{2-} + \\text{H}^+
]<\/p>\n\n\n\nBicarbonate (( \\text{HCO}_3^- )) as a Base:<\/h3>\n\n\n\n
\\text{HCO}_3^- + \\text{H}^+ \\rightarrow \\text{H}_2\\text{CO}_3
]<\/p>\n\n\n\nHydrogen Sulfide (( \\text{HS}^- )) as an Acid:<\/h3>\n\n\n\n
\\text{HS}^- \\rightarrow \\text{S}^{2-} + \\text{H}^+
]<\/p>\n\n\n\nHydrogen Sulfide (( \\text{HS}^- )) as a Base:<\/h3>\n\n\n\n
\\text{HS}^- + \\text{H}^+ \\rightarrow \\text{H}_2\\text{S}
]<\/p>\n\n\n\nExplanation:<\/h3>\n\n\n\n