Is the ionic compound CaCO3 soluble or insoluble, and does each of its ions tend to be soluble?<\/p>\n\n\n\n
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble<\/p>\n\n\n\n
Is the ionic compound NaNO3 soluble or insoluble, and does each of its ions tend to be soluble?<\/p>\n\n\n\n
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble<\/p>\n\n\n\n
Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?<\/p>\n\n\n\n
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble<\/p>\n\n\n\n
Is the ionic compound (NH4)3PO4 soluble or insoluble, and does each of its ions tend to be soluble?<\/p>\n\n\n\n
a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble<\/p>\n\n\n\n
Classify the solution properties of 1.0 M acetic acid.<\/p>\n\n\n\n
a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n 1. Is the ionic compound CaCO\u2083 soluble or insoluble, and does each of its ions tend to be soluble?<\/strong><\/p>\n\n\n\n Answer: d. Ions differ; insoluble<\/strong><\/p>\n\n\n\n Explanation: Calcium carbonate (CaCO\u2083) is largely insoluble<\/strong> in water. The solubility of ionic compounds depends on the ability of their ions to dissociate in water. While calcium (Ca\u00b2\u207a) ions are generally soluble in water (as seen in compounds like CaCl\u2082), carbonate (CO\u2083\u00b2\u207b) ions tend to form insoluble salts with many cations, particularly calcium. Therefore, CaCO\u2083 is insoluble, but the ions individually (Ca\u00b2\u207a and CO\u2083\u00b2\u207b) would typically be soluble if isolated in other compounds.<\/p>\n\n\n\n 2. Is the ionic compound NaNO\u2083 soluble or insoluble, and does each of its ions tend to be soluble?<\/strong><\/p>\n\n\n\n Answer: a. Both ions soluble<\/strong><\/p>\n\n\n\n Explanation: Sodium nitrate (NaNO\u2083) is soluble<\/strong> in water. Sodium ions (Na\u207a) and nitrate ions (NO\u2083\u207b) both tend to be soluble in water. Sodium salts are generally soluble due to their low lattice energies, and nitrates are generally soluble in water, with very few exceptions. Therefore, NaNO\u2083 dissolves completely, with both Na\u207a and NO\u2083\u207b ions being soluble.<\/p>\n\n\n\n 3. Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?<\/strong><\/p>\n\n\n\n Answer: c. Ions differ; soluble<\/strong><\/p>\n\n\n\n Explanation: Silver bromide (AgBr) is insoluble<\/strong> in water. However, silver (Ag\u207a) is generally soluble in many compounds, and bromide (Br\u207b) is soluble in most salts except those formed with heavy metals like Ag\u207a, Pb\u00b2\u207a, and Hg\u2082\u00b2\u207a. While Ag\u207a and Br\u207b tend to be soluble separately, their combination forms an insoluble salt (AgBr), due to the relatively low solubility product (Ksp) of AgBr.<\/p>\n\n\n\n 4. Is the ionic compound (NH\u2084)\u2083PO\u2084 soluble or insoluble, and does each of its ions tend to be soluble?<\/strong><\/p>\n\n\n\n Answer: a. Both ions soluble<\/strong><\/p>\n\n\n\n Explanation: Ammonium phosphate ((NH\u2084)\u2083PO\u2084) is soluble<\/strong> in water. Ammonium (NH\u2084\u207a) salts are typically soluble because ammonium is a weak acid and dissolves easily in water. Phosphate (PO\u2084\u00b3\u207b), despite its tendency to form insoluble salts with many other cations (like calcium), remains soluble in combination with ammonium. Therefore, both ions in (NH\u2084)\u2083PO\u2084 are soluble.<\/p>\n\n\n\n 5. Classify the solution properties of 1.0 M acetic acid.<\/strong><\/p>\n\n\n\n Answer: b. Weak electrolyte<\/strong><\/p>\n\n\n\n Explanation: Acetic acid (CH\u2083COOH) is a weak electrolyte<\/strong>. This means that it does not completely dissociate into ions when dissolved in water. Acetic acid only partially ionizes in water to form hydrogen ions (H\u207a) and acetate ions (CH\u2083COO\u207b), unlike strong electrolytes like hydrochloric acid (HCl), which dissociates completely. As a result, acetic acid is considered a weak electrolyte because it only partially conducts electricity due to its limited ionization in solution.<\/p>\n","protected":false},"excerpt":{"rendered":" Is the ionic compound CaCO3 soluble or insoluble, and does each of its ions tend to be soluble? a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble Is the ionic compound NaNO3 soluble or insoluble, and does each of its ions tend to be soluble? a. Both ions […]<\/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-187088","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187088","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=187088"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187088\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187088"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187088"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187088"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n
\n\n\n\n
\n\n\n\n
\n\n\n\n