{"id":240766,"date":"2025-07-03T11:43:49","date_gmt":"2025-07-03T11:43:49","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=240766"},"modified":"2025-07-03T11:43:51","modified_gmt":"2025-07-03T11:43:51","slug":"what-is-the-ph-of-a-0-85-m-hclo4-perchlorate-acid-a-strong-acid-solution-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/what-is-the-ph-of-a-0-85-m-hclo4-perchlorate-acid-a-strong-acid-solution-2\/","title":{"rendered":"What is the pH of a 0.85 M HClO4 (perchlorate acid, a strong acid) solution"},"content":{"rendered":"\n

What is the pH of a 0.85 M HClO4 (perchlorate acid, a strong acid) solution?<\/a><\/p>\n\n\n\n

The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n

The pH of a 0.85 M HClO\u2084 (perchloric acid) solution is 0.070<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

Perchloric acid (HClO\u2084) is a strong acid, meaning it dissociates completely in water. When a strong acid like HClO\u2084 dissolves in water, it releases hydrogen ions (H\u207a) or protons, which are responsible for the acidity of the solution. The dissociation equation for HClO\u2084 is:<\/p>\n\n\n\n

HClO\u2084(aq)\u2192H\u207a(aq)+ClO\u2084\u2212(aq)\\text{HClO\u2084} (aq) \\rightarrow \\text{H\u207a} (aq) + \\text{ClO\u2084}\u207b (aq)<\/p>\n\n\n\n

For a strong acid, the concentration of hydrogen ions ([H\u207a]) is equal to the concentration of the acid. In this case, the concentration of HClO\u2084 is 0.85 M, so the concentration of hydrogen ions is also 0.85 M.<\/p>\n\n\n\n

The pH is a measure of the concentration of hydrogen ions in a solution and is defined as: pH=\u2212log\u2061[H\u207a]\\text{pH} = -\\log[\\text{H\u207a}]<\/p>\n\n\n\n

Substitute the concentration of hydrogen ions into the equation: pH=\u2212log\u2061(0.85)\\text{pH} = -\\log(0.85)<\/p>\n\n\n\n

Using a calculator: pH=\u2212(\u22120.070)=0.070\\text{pH} = -(-0.070) = 0.070<\/p>\n\n\n\n

So, the pH of the solution is 0.070<\/strong>.<\/p>\n\n\n\n

Additional Notes:<\/h3>\n\n\n\n
    \n
  • Strong acids like HClO\u2084 dissociate completely, meaning there is no need to consider partial dissociation as is the case with weak acids.<\/li>\n\n\n\n
  • The pH scale ranges from 0 to 14, with 7 being neutral. A pH below 7 indicates an acidic solution, and a pH below 1 is strongly acidic.<\/li>\n\n\n\n
  • A pH of 0.070 indicates a very acidic solution, which is typical for strong acids at concentrations above 0.1 M.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

    What is the pH of a 0.85 M HClO4 (perchlorate acid, a strong acid) solution? The correct answer and explanation is: The pH of a 0.85 M HClO\u2084 (perchloric acid) solution is 0.070. Explanation: Perchloric acid (HClO\u2084) is a strong acid, meaning it dissociates completely in water. When a strong acid like HClO\u2084 dissolves in […]<\/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-240766","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240766","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=240766"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240766\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240766"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240766"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240766"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}