{"id":182569,"date":"2025-01-14T11:41:28","date_gmt":"2025-01-14T11:41:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182569"},"modified":"2025-01-14T11:41:30","modified_gmt":"2025-01-14T11:41:30","slug":"compare-the-relative-solubilities-of-bacro4-and-bacr2o7","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/14\/compare-the-relative-solubilities-of-bacro4-and-bacr2o7\/","title":{"rendered":"Compare the relative solubilities of BaCrO4 and BaCr2O7"},"content":{"rendered":"\n<p>it is a lab question, Compare the relative solubilities of BaCrO4 and BaCr2O7. Explain why?\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026..<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>The solubilities of BaCrO\u2084 (barium chromate) and BaCr\u2082O\u2087 (barium dichromate) are quite different, with BaCrO\u2084 being much less soluble in water compared to BaCr\u2082O\u2087.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Solubility Comparison:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>BaCrO\u2084 (Barium Chromate)<\/strong>: BaCrO\u2084 is known for its low solubility in water. It is classified as an insoluble salt. The solubility product constant (Ksp) of BaCrO\u2084 is very small, indicating that only a tiny amount of BaCrO\u2084 dissolves in water. The low solubility is due to the strong ionic lattice formed between Ba\u00b2\u207a and CrO\u2084\u00b2\u207b ions, which makes it difficult for water molecules to break the lattice and dissolve the compound.<\/li>\n\n\n\n<li><strong>BaCr\u2082O\u2087 (Barium Dichromate)<\/strong>: BaCr\u2082O\u2087, on the other hand, is more soluble in water. This can be attributed to its ability to dissociate into two chromate ions (Cr\u2082O\u2087\u00b2\u207b) per barium ion. The chromate ion, Cr\u2082O\u2087\u00b2\u207b, has a relatively larger solubility product compared to the CrO\u2084\u00b2\u207b ion, making BaCr\u2082O\u2087 more soluble.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Reason for Difference in Solubility:<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Ion Interaction:<\/strong> BaCrO\u2084 is less soluble because it involves the chromate ion (CrO\u2084\u00b2\u207b), which has a smaller dissociation constant and a higher tendency to form a stable crystal lattice structure. In comparison, BaCr\u2082O\u2087 dissociates into two Cr\u2082O\u2087\u00b2\u207b ions, which increases the disorder (entropy) of the system, leading to greater solubility.<\/li>\n\n\n\n<li><strong>Chemical Structure:<\/strong> The structure of Cr\u2082O\u2087\u00b2\u207b (dichromate) is more complex, and it has a higher charge density, meaning that the ions interact more favorably with water molecules, aiding in dissociation. In contrast, CrO\u2084\u00b2\u207b (chromate) is simpler and interacts less effectively with water molecules, making it less soluble.<\/li>\n\n\n\n<li><strong>Precipitation Behavior:<\/strong> BaCrO\u2084, due to its low solubility, tends to form precipitates in solutions containing Ba\u00b2\u207a and CrO\u2084\u00b2\u207b ions. In contrast, BaCr\u2082O\u2087 can dissolve more easily when placed in a solution, especially in acidic conditions, where the dichromate ion is more stable than the chromate ion.<\/li>\n<\/ol>\n\n\n\n<p>Thus, the difference in solubility is due to the different properties of the chromate and dichromate ions and their ability to interact with water molecules, leading to the solubility disparity between BaCrO\u2084 and BaCr\u2082O\u2087.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>it is a lab question, Compare the relative solubilities of BaCrO4 and BaCr2O7. Explain why?\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026\u2026.. The Correct Answer and Explanation is : The solubilities of BaCrO\u2084 (barium chromate) and BaCr\u2082O\u2087 (barium dichromate) are quite different, with BaCrO\u2084 being much less soluble in water compared to BaCr\u2082O\u2087. Solubility Comparison: Reason for Difference in Solubility: Thus, 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-182569","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182569","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=182569"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182569\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182569"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182569"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182569"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}