{"id":205996,"date":"2025-03-26T06:43:24","date_gmt":"2025-03-26T06:43:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=205996"},"modified":"2025-03-26T06:43:26","modified_gmt":"2025-03-26T06:43:26","slug":"what-is-the-ph-ofa-6-50-x-10-3-m-koh-solution","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/26\/what-is-the-ph-ofa-6-50-x-10-3-m-koh-solution\/","title":{"rendered":"What is the pH ofa 6.50 x 10-3 M KOH solution"},"content":{"rendered":"\n

What is the pH ofa 6.50 x 10-3 M KOH solution?(Hint: this is a basic solution\u2013 concentration is of OH-)<\/p>\n\n\n\n

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

To determine the pH of a 6.50 \u00d7 10\u207b\u00b3 M KOH<\/strong> solution, follow these steps:<\/p>\n\n\n\n

Step 1: Identify Key Information<\/strong><\/h3>\n\n\n\n
    \n
  • KOH<\/strong> is a strong base, meaning it dissociates completely in water:
    [
    \\text{KOH} \\rightarrow \\text{K}^+ + \\text{OH}^-
    ]<\/li>\n\n\n\n
  • The concentration of hydroxide ions (\\text{OH}^-) is equal to the given concentration of KOH:
    [
    [\\text{OH}^-] = 6.50 \\times 10^{-3} M
    ]<\/li>\n<\/ul>\n\n\n\n

    Step 2: Calculate pOH<\/strong><\/h3>\n\n\n\n

    The pOH is calculated using the formula:
    [
    \\text{pOH} = -\\log [\\text{OH}^-]
    ]
    [
    \\text{pOH} = -\\log (6.50 \\times 10^{-3})
    ]
    Using a calculator:
    [
    \\text{pOH} \\approx 2.19
    ]<\/p>\n\n\n\n

    Step 3: Determine pH<\/strong><\/h3>\n\n\n\n

    Since the relationship between pH<\/strong> and pOH<\/strong> is:
    [
    \\text{pH} + \\text{pOH} = 14
    ]
    [
    \\text{pH} = 14 – 2.19
    ]
    [
    \\text{pH} \\approx 11.81
    ]<\/p>\n\n\n\n

    Final Answer:<\/strong><\/h3>\n\n\n\n

    The pH of the 6.50 \u00d7 10\u207b\u00b3 M KOH<\/strong> solution is 11.81<\/strong>, confirming it is a basic solution.<\/p>\n\n\n\n

    \n\n\n\n

    Explanation (300 Words)<\/strong><\/h3>\n\n\n\n

    The pH scale ranges from 0 to 14, where values below 7<\/strong> are acidic, above 7<\/strong> are basic, and exactly 7<\/strong> is neutral. Since potassium hydroxide (KOH) is a strong base, it dissociates completely in water to release hydroxide ions (OH\u207b<\/strong>), making the solution basic.<\/p>\n\n\n\n

    To find the pH, we first determine the pOH<\/strong> using the formula pOH = -log[OH\u207b]<\/strong>. Plugging in the concentration 6.50 \u00d7 10\u207b\u00b3 M<\/strong>, we obtain pOH \u2248 2.19<\/strong>. Since pH and pOH are related by the equation pH + pOH = 14<\/strong>, solving for pH gives pH \u2248 11.81<\/strong>.<\/p>\n\n\n\n

    A pH of 11.81<\/strong> confirms the solution is basic because it is significantly higher than 7. This makes sense because KOH is a strong base and contributes a relatively high concentration of hydroxide ions to the solution.<\/p>\n\n\n\n

    In practical applications, knowing the pH of a solution is important in chemistry, medicine, and environmental science. For example, alkaline solutions like KOH are used in soap-making, cleaning agents, and industrial processes where strong bases are needed.<\/p>\n\n\n\n

    This problem reinforces the importance of understanding logarithmic functions in pH calculations and highlights how strong bases completely dissociate in aqueous solutions.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    What is the pH ofa 6.50 x 10-3 M KOH solution?(Hint: this is a basic solution\u2013 concentration is of OH-) The correct answer and explanation is : To determine the pH of a 6.50 \u00d7 10\u207b\u00b3 M KOH solution, follow these steps: Step 1: Identify Key Information Step 2: Calculate pOH The pOH is calculated […]<\/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-205996","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205996","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=205996"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205996\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=205996"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=205996"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=205996"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}