POGIL Common Ion Effect on Solubility Extension Questions:<\/p>\n\n\n\n
Thank you!<\/p>\n\n\n\n
Certainly! Here are the correct answers followed by a detailed explanation of each:<\/p>\n\n\n\n
16. Would the four beakers in Model 1 have the same reading on a pH meter? Explain your reasoning.<\/strong><\/p>\n\n\n\n Answer:<\/strong> 17. Consider any of the beakers in Model 1. Predict what might happen to the solubility of the insoluble salt if a 1.0 M acid solution was added dropwise to the beaker. Hint: Which ion species in the beaker will react with the acid? How will this reaction alter the concentration of the common ion?<\/strong><\/p>\n\n\n\n Answer:<\/strong> The Common Ion Effect is a concept rooted in Le Ch\u00e2telier\u2019s Principle<\/strong>, which states that a system at equilibrium will adjust to counteract any changes. In Model 1, you likely observed several beakers containing an insoluble salt (e.g., calcium carbonate or silver chloride) in water, and in some cases, with a solution containing a common ion<\/strong> already dissolved.<\/p>\n\n\n\n Question 16:<\/strong> Question 17:<\/strong> This neutralization reduces the concentration<\/strong> of the common ion that was suppressing the salt\u2019s solubility. According to Le Ch\u00e2telier\u2019s Principle, the equilibrium will shift to dissolve more of the salt<\/strong> to restore the concentration of the removed ion. As a result, the solubility of the originally insoluble salt increases.<\/p>\n\n\n\n This effect is commonly exploited in chemical processes to enhance the solubility of salts, particularly when dealing with sparingly soluble compounds in acidic environments.<\/p>\n","protected":false},"excerpt":{"rendered":" POGIL Common Ion Effect on Solubility Extension Questions: Thank you! Certainly! Here are the correct answers followed by a detailed explanation of each: 16. Would the four beakers in Model 1 have the same reading on a pH meter? Explain your reasoning. Answer:No, the four beakers in Model 1 would not have the same pH […]<\/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-213426","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/213426","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=213426"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/213426\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=213426"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=213426"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=213426"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
No, the four beakers in Model 1 would not have the same pH readings.<\/p>\n\n\n\n
\n\n\n\n
The solubility of the insoluble salt will increase because the acid will react with the common ion (typically a basic anion like CO\u2083\u00b2\u207b or OH\u207b), reducing its concentration and shifting the equilibrium to dissolve more salt.<\/p>\n\n\n\n
\n\n\n\n\u2728 Detailed Explanation (300+ words):<\/h3>\n\n\n\n
Beakers with different solutes or added substances will have different pH values. For example, a beaker containing only pure water and an insoluble salt will have a neutral or near-neutral pH. However, if the salt dissociates into an ion like CO\u2083\u00b2\u207b (carbonate), which can accept hydrogen ions (H\u207a), the solution becomes basic. On the other hand, adding a solution that already contains an acid or acidic salt (e.g., NH\u2084\u207a from NH\u2084Cl) will lower the pH. Therefore, the pH readings differ due to the varying presence and nature of dissolved ions.<\/p>\n\n\n\n
Adding a 1.0 M acid solution dropwise introduces H\u207a ions into the beaker. If the common ion in solution is a basic anion like CO\u2083\u00b2\u207b or OH\u207b, it will react with H\u207a:<\/p>\n\n\n\n\n