naoh
ca(oh)2<\/li>\n\n\n\n
none of the above
b. write the net ionic equation for the acid-base hydrolysis equilibrium that is established when barium fluoride is dissolved in water. (use the lowest possible coefficients. be sure to specify states such as (aq) or (s). if a box is not needed, leave it blank) h2o (1) –> + +
this solution is: acidic, basic, neutral<\/li>\n<\/ul>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n A Bronsted-Lowry base<\/strong> is defined as a substance that accepts protons (H\u207a ions) in an aqueous solution. Let’s go through the substances one by one to see which can behave as Bronsted-Lowry bases:<\/p>\n\n\n\n Answer to Part a:<\/strong><\/p>\n\n\n\n When Barium Fluoride (BaF\u2082)<\/strong> dissolves in water, it dissociates into Ba\u00b2\u207a and F\u207b ions. The fluoride ion (F\u207b), being the conjugate base of a weak acid (HF), will undergo hydrolysis to react with water, forming hydroxide ions (OH\u207b) and hydrofluoric acid (HF).<\/p>\n\n\n\n The relevant equilibrium for this reaction is: Net Ionic Equation:<\/strong> Since the fluoride ions accept protons from water and produce OH\u207b ions, the solution will be basic<\/strong>.<\/p>\n\n\n\n I will now generate an image that visually represents the dissolution and hydrolysis process.<\/p>\n\n\n\n Here is the image illustrating the dissolution of barium fluoride (BaF\u2082) in water and the subsequent hydrolysis of fluoride ions (F\u207b) with water to form HF and OH\u207b. It visually represents the basic nature of the resulting solution. Let me know if you need further details!<\/p>\n\n\n\n a. which of the following can behave as bronsted-lowry bases in aqueous solution? The Correct Answer and Explanation is : Part a: Bronsted-Lowry Bases in Aqueous Solution A Bronsted-Lowry base is defined as a substance that accepts protons (H\u207a ions) in an aqueous solution. Let’s go through the substances one by one to see which […]<\/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-192236","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192236","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=192236"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192236\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192236"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192236"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192236"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Part a: Bronsted-Lowry Bases in Aqueous Solution<\/h3>\n\n\n\n
\n
KOH dissociates in water to form K\u207a and OH\u207b ions. The OH\u207b ion can accept a proton, so KOH can act as a Bronsted-Lowry base.<\/li>\n\n\n\n
Similar to KOH, NaOH dissociates in water to form Na\u207a and OH\u207b ions. The OH\u207b ion can accept a proton, so NaOH is also a Bronsted-Lowry base.<\/li>\n\n\n\n
Ca(OH)\u2082 dissociates in water to produce Ca\u00b2\u207a and OH\u207b ions. As with KOH and NaOH, the OH\u207b ion acts as a Bronsted-Lowry base, so Ca(OH)\u2082 can also behave as a Bronsted-Lowry base.<\/li>\n\n\n\n
The fluoride ion is the conjugate base of HF (hydrofluoric acid). When F\u207b accepts a proton (H\u207a), it forms HF. Thus, F\u207b can also behave as a Bronsted-Lowry base.<\/li>\n<\/ol>\n\n\n\n\n
Part b: Net Ionic Equation for Barium Fluoride Dissolution<\/h3>\n\n\n\n
[ F^-(aq) + H_2O(l) \\rightleftharpoons HF(aq) + OH^-(aq) ]<\/p>\n\n\n\n
[ F^-(aq) + H_2O(l) \\rightleftharpoons HF(aq) + OH^-(aq) ]<\/p>\n\n\n\nSolution Type<\/h3>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
\n
[
BaF_2(s) \\rightarrow Ba^{2+}(aq) + 2F^-(aq)
]<\/li>\n\n\n\n
[
F^-(aq) + H_2O(l) \\rightleftharpoons HF(aq) + OH^-(aq)
] In this reaction, the fluoride ion (F\u207b) accepts a proton (H\u207a) from water, producing hydroxide ions (OH\u207b) and hydrofluoric acid (HF).<\/li>\n\n\n\nImage Generation<\/h3>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-783.png\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"