{"id":90939,"date":"2025-06-01T10:41:36","date_gmt":"2025-06-01T10:41:36","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=90939"},"modified":"2025-06-01T10:41:36","modified_gmt":"2025-06-01T10:41:36","slug":"water-is-a-good-solvent-for-dissolving-ionic-compounds-because","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/","title":{"rendered":"Water is a good solvent for dissolving ionic compounds because"},"content":{"rendered":"

Water is a good solvent for dissolving ionic compounds because<\/p>\n

[amp_mcq option1=”It has a high specific heat” option2=”It has no colour” option3=”It has a high dipole moment” option4=”It has a high boiling point” correct=”option3″]<\/p>\n

\n
\n
This question was previously asked in<\/div>\n
UPSC CAPF – 2024<\/div>\n<\/div>\n
Download PDF<\/a>Attempt Online<\/a><\/div>\n<\/div>\n
\nWater is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds.
\n<\/section>\n
\nWater’s ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.
\n<\/section>\n
\nThe process of dissolving an ionic compound in water is called dissociation and hydration. The hydrated ions are dispersed throughout the solution. Water is often referred to as the “universal solvent” because of its ability to dissolve a wide range of substances, including many ionic and polar covalent compounds.
\n<\/section>\n","protected":false},"excerpt":{"rendered":"

Water is a good solvent for dissolving ionic compounds because [amp_mcq option1=”It has a high specific heat” option2=”It has no colour” option3=”It has a high dipole moment” option4=”It has a high boiling point” correct=”option3″] This question was previously asked in UPSC CAPF – 2024 Download PDFAttempt Online Water is an excellent solvent for ionic compounds … <\/p>\n

Detailed SolutionWater is a good solvent for dissolving ionic compounds because<\/span><\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1085],"tags":[1103,1096,1155],"class_list":["post-90939","post","type-post","status-publish","format-standard","hentry","category-upsc-capf","tag-1103","tag-chemistry","tag-physical-and-chemical-changes-solution","no-featured-image-padding"],"yoast_head":"\nWater is a good solvent for dissolving ionic compounds because<\/title>\n<meta name=\"description\" content=\"Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds. Water's ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Water is a good solvent for dissolving ionic compounds because\" \/>\n<meta property=\"og:description\" content=\"Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds. Water's ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T10:41:36+00:00\" \/>\n<meta name=\"author\" content=\"rawan239\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"rawan239\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"1 minute\" \/>\n<!-- \/ Yoast SEO Premium plugin. -->","yoast_head_json":{"title":"Water is a good solvent for dissolving ionic compounds because","description":"Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds. Water's ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.","robots":{"index":"index","follow":"follow","max-snippet":"max-snippet:-1","max-image-preview":"max-image-preview:large","max-video-preview":"max-video-preview:-1"},"canonical":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/","og_locale":"en_US","og_type":"article","og_title":"Water is a good solvent for dissolving ionic compounds because","og_description":"Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds. Water's ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T10:41:36+00:00","author":"rawan239","twitter_card":"summary_large_image","twitter_misc":{"Written by":"rawan239","Est. reading time":"1 minute"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"WebPage","@id":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/","url":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/","name":"Water is a good solvent for dissolving ionic compounds because","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T10:41:36+00:00","dateModified":"2025-06-01T10:41:36+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds. Water's ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/water-is-a-good-solvent-for-dissolving-ionic-compounds-because\/#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/exam.pscnotes.com\/mcq\/"},{"@type":"ListItem","position":2,"name":"UPSC CAPF","item":"https:\/\/exam.pscnotes.com\/mcq\/category\/upsc-capf\/"},{"@type":"ListItem","position":3,"name":"Water is a good solvent for dissolving ionic compounds because"}]},{"@type":"WebSite","@id":"https:\/\/exam.pscnotes.com\/mcq\/#website","url":"https:\/\/exam.pscnotes.com\/mcq\/","name":"MCQ and Quiz for Exams","description":"","potentialAction":[{"@type":"SearchAction","target":{"@type":"EntryPoint","urlTemplate":"https:\/\/exam.pscnotes.com\/mcq\/?s={search_term_string}"},"query-input":"required name=search_term_string"}],"inLanguage":"en-US"},{"@type":"Person","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209","name":"rawan239","image":{"@type":"ImageObject","inLanguage":"en-US","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/image\/","url":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","contentUrl":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","caption":"rawan239"},"sameAs":["https:\/\/exam.pscnotes.com"],"url":"https:\/\/exam.pscnotes.com\/mcq\/author\/rawan239\/"}]}},"amp_enabled":true,"_links":{"self":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90939","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/comments?post=90939"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90939\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=90939"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=90939"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=90939"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}