{"id":246812,"date":"2025-07-07T13:06:57","date_gmt":"2025-07-07T13:06:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=246812"},"modified":"2025-07-07T13:06:59","modified_gmt":"2025-07-07T13:06:59","slug":"write-both-answers-to-at-least-two-decimal-places","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/07\/write-both-answers-to-at-least-two-decimal-places\/","title":{"rendered":"Write both answers to at least two decimal places."},"content":{"rendered":"\n<p>Write both answers to at least two decimal places. Calculate the pH of a 0.150 M solution of KOH. Calculate the pOH of a 0.150 M solution of KOH.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the <strong>pH<\/strong> and <strong>pOH<\/strong> of a 0.150 M solution of KOH (potassium hydroxide), we need to consider the basic nature of KOH, which dissociates completely in water.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Understanding the dissociation of KOH<\/h3>\n\n\n\n<p>KOH is a strong base, meaning it dissociates completely in water according to the following reaction:KOH\u2192K++OH\u2212\\text{KOH} \\rightarrow \\text{K}^+ + \\text{OH}^-KOH\u2192K++OH\u2212<\/p>\n\n\n\n<p>Since KOH dissociates completely, the concentration of hydroxide ions (<strong>OH\u207b<\/strong>) will be equal to the concentration of KOH. Therefore, in a 0.150 M solution of KOH, the concentration of <strong>OH\u207b<\/strong> ions will also be <strong>0.150 M<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculating pOH<\/h3>\n\n\n\n<p>The <strong>pOH<\/strong> is calculated using the formula:pOH=\u2212log\u2061[OH\u2212]\\text{pOH} = -\\log[\\text{OH}^-]pOH=\u2212log[OH\u2212]<\/p>\n\n\n\n<p>Substituting the concentration of <strong>OH\u207b<\/strong>:pOH=\u2212log\u2061(0.150)=0.82391\u22480.82\\text{pOH} = -\\log(0.150) = 0.82391 \\approx 0.82pOH=\u2212log(0.150)=0.82391\u22480.82<\/p>\n\n\n\n<p>So, the <strong>pOH<\/strong> of the 0.150 M KOH solution is <strong>0.82<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculating pH<\/h3>\n\n\n\n<p>To calculate the <strong>pH<\/strong>, we can use the relationship between <strong>pH<\/strong> and <strong>pOH<\/strong>:pH+pOH=14\\text{pH} + \\text{pOH} = 14pH+pOH=14<\/p>\n\n\n\n<p>Now, substitute the value of <strong>pOH<\/strong>:pH=14\u2212pOH=14\u22120.82=13.18\\text{pH} = 14 &#8211; \\text{pOH} = 14 &#8211; 0.82 = 13.18pH=14\u2212pOH=14\u22120.82=13.18<\/p>\n\n\n\n<p>Thus, the <strong>pH<\/strong> of the 0.150 M KOH solution is <strong>13.18<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>pOH<\/strong> = <strong>0.82<\/strong><\/li>\n\n\n\n<li><strong>pH<\/strong> = <strong>13.18<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Both values are calculated to two decimal places, and these results are consistent with the expected values for a strong base like KOH in this concentration. The pH is very high, reflecting the strong basic nature of the solution, while the pOH is quite low, indicating a high concentration of hydroxide ions.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-947.jpeg\" alt=\"\" class=\"wp-image-246813\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Write both answers to at least two decimal places. Calculate the pH of a 0.150 M solution of KOH. Calculate the pOH of a 0.150 M solution of KOH. The Correct Answer and Explanation is: To calculate the pH and pOH of a 0.150 M solution of KOH (potassium hydroxide), we need to consider the [&hellip;]<\/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-246812","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246812","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=246812"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246812\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246812"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246812"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246812"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}