Calculate the molarity of a Ba(OH)2 solution if 1950 mL is completely titrated by 26.1 mL of 0.505 M HNO3<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n To calculate the molarity of the Ba(OH)\u2082 solution, we will use the concept of neutralization reactions and the stoichiometry of the reaction between Ba(OH)\u2082 and HNO\u2083.<\/p>\n\n\n\n The reaction between barium hydroxide (Ba(OH)\u2082) and nitric acid (HNO\u2083) is:<\/p>\n\n\n\n [ This equation shows that one mole of Ba(OH)\u2082 reacts with two moles of HNO\u2083.<\/p>\n\n\n\n We are given the volume and molarity of the HNO\u2083 solution. The formula to calculate moles is:<\/p>\n\n\n\n [ Where:<\/p>\n\n\n\n [ From the balanced equation, we see that 2 moles of HNO\u2083 react with 1 mole of Ba(OH)\u2082. Therefore, the moles of Ba(OH)\u2082 can be calculated as:<\/p>\n\n\n\n [ We are given the volume of Ba(OH)\u2082 solution as 1950 mL, which is 1.950 L. Molarity is defined as moles of solute per liter of solution:<\/p>\n\n\n\n [ [ The molarity of the Ba(OH)\u2082 solution is approximately 0.00338 M<\/strong>.<\/p>\n\n\n\n In this problem, we used the stoichiometry of the neutralization reaction between Ba(OH)\u2082 and HNO\u2083 to find the molarity of the Ba(OH)\u2082 solution. By first determining the number of moles of HNO\u2083 used in the titration, we applied the molar ratio from the balanced equation to calculate the moles of Ba(OH)\u2082. Finally, we divided the moles of Ba(OH)\u2082 by the volume of the Ba(OH)\u2082 solution to find its molarity. This approach ensures we account for the chemical relationship between the acid and base and the volume of the solutions involved.<\/p>\n","protected":false},"excerpt":{"rendered":" Calculate the molarity of a Ba(OH)2 solution if 1950 mL is completely titrated by 26.1 mL of 0.505 M HNO3 The Correct Answer and Explanation is: To calculate the molarity of the Ba(OH)\u2082 solution, we will use the concept of neutralization reactions and the stoichiometry of the reaction between Ba(OH)\u2082 and HNO\u2083. Step 1: Write […]<\/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-166132","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166132","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=166132"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166132\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=166132"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=166132"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=166132"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Write the balanced chemical equation<\/h3>\n\n\n\n
\\text{Ba(OH)}_2(aq) + 2\\text{HNO}_3(aq) \\rightarrow \\text{Ba(NO}_3)_2(aq) + 2\\text{H}_2\\text{O}(l)
]<\/p>\n\n\n\nStep 2: Calculate the moles of HNO\u2083 used<\/h3>\n\n\n\n
\\text{moles of HNO}_3 = M \\times V
]<\/p>\n\n\n\n\n
\\text{moles of HNO}_3 = 0.505 \\, \\text{mol\/L} \\times 0.0261 \\, \\text{L} = 0.0132 \\, \\text{mol}
]<\/p>\n\n\n\nStep 3: Use stoichiometry to calculate moles of Ba(OH)\u2082<\/h3>\n\n\n\n
\\text{moles of Ba(OH)}_2 = \\frac{\\text{moles of HNO}_3}{2} = \\frac{0.0132}{2} = 0.0066 \\, \\text{mol}
]<\/p>\n\n\n\nStep 4: Calculate the molarity of Ba(OH)\u2082<\/h3>\n\n\n\n
M = \\frac{\\text{moles of Ba(OH)}_2}{\\text{volume of Ba(OH)}_2 \\, \\text{in liters}}
]<\/p>\n\n\n\n
M = \\frac{0.0066 \\, \\text{mol}}{1.950 \\, \\text{L}} = 0.00338 \\, \\text{M}
]<\/p>\n\n\n\nFinal Answer:<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n