{"id":984,"date":"2022-11-18T16:00:03","date_gmt":"2022-11-18T10:30:03","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=984"},"modified":"2022-11-19T16:31:35","modified_gmt":"2022-11-19T11:01:35","slug":"classification-of-salts","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/classification-of-salts\/","title":{"rendered":"Classification of Salts"},"content":{"rendered":"<h2><span style=\"color: #00ccff;\"><strong>Classification of Salts<\/strong><\/span><\/h2>\n<p><strong>What is a salt?<\/strong><\/p>\n<p>A salt is formed in a <strong>neutralisation reaction<\/strong> between an acid and a base.\u00a0Salt is a general term used for the substances that are formed when an acid and a base react with each other.<br \/>\nThis reaction is called a <strong>neutralization<\/strong> reaction.<br \/>\nAcid + base \u2192\u00a0salt + water<br \/>\nA <strong>salt<\/strong> is an <strong>ionic compound<\/strong> consisting of a <strong>cation<\/strong> such as a <strong>metal ion<\/strong> or an <strong>ammonium ion<\/strong> from a base and an anion from an <strong>acid<\/strong>.<\/p>\n<p><strong>Example:<\/strong><br \/>\nThe reaction between vinegar and baking soda is a neutralization reaction. Vinegar, as we already know, contains an acid and baking soda contains a base. When vinegar reacts with baking soda, a salt is formed. Water and carbon dioxide gas are also the products of this reaction.<br \/>\nSimilarly, common table salt is formed by the reaction of hydrochloric acid (HCl) with sodium hydroxide (NaOH).<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-111981\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-1.png\" alt=\"Classification of Salts 1\" width=\"796\" height=\"86\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-1.png 796w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-1-300x32.png 300w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-1-768x83.png 768w\" sizes=\"(max-width: 796px) 100vw, 796px\" \/><br \/>\nHCl(aq) + NaOH(aq) \u2192\u00a0NaCl(aq) + H<sub>2<\/sub>O(l)<\/p>\n<p>Hence, a salt can be defined as follows.<br \/>\nA <strong>salt<\/strong> is a compound formed when the hydrogen ion in an acid is replaced by a metal ion or an ammonium ion.<\/p>\n<p><strong>People also ask<\/strong><\/p>\n<ul>\n<li><a href=\"https:\/\/www.aplustopper.com\/general-properties-salts\/\">General Properties of Salts<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/the-uses-of-salts\/\">Uses of different salts in daily life<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/preparation-of-salts\/\">Preparation of Salts<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/describe-preparation-soluble-insoluble-salts\/\">Describe the preparation of soluble and insoluble salts<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/qualitative-analysis-salts\/\">Qualitative Analysis of Salts<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/action-heat-salts\/\">Action of Heat on Salts<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/test-cations-anions-aqueous-solutions\/\">Test for Cations and Anions in Aqueous Solutions<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/constructing-ionic-equations-using-continuous-variation-method\/\">Constructing ionic equations using the continuous variation method<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/stoichiometry-used-chemistry\/\">What is stoichiometry and why is it used in chemistry?<\/a><\/li>\n<\/ul>\n<p><strong>Table: Examples of salts from different acids<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" colspan=\"2\" width=\"180\"><strong>Acid<\/strong><\/td>\n<td style=\"text-align: center;\" colspan=\"3\" width=\"366\"><strong>Salt<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Hydrochloric acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">HCl<\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Chloride<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Sodium<strong> chloride<\/strong> Ammonium <strong>chloride<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">NaCl<br \/>\nNH<sub>3<\/sub>Cl<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Nitric acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">HNO<sub>3<\/sub><\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Nitrate<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Potassium <strong>nitrate<\/strong> Aluminium <strong>nitrate<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">KNO<sub>3<\/sub><br \/>\nAl(NO<sub>3<\/sub>)<sub>3<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Sulphuric acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Sulphate<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Ammonium <strong>sulphate<\/strong> Magnesium <strong>sulphate<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">(NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><br \/>\nMgSO<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Carbonic acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">H<sub>2<\/sub>CO<sub>3<\/sub><\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Carbonate<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Iron(ll) c<strong>arbonate<\/strong> Calcium <strong>carbonate<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">FeCO<sub>3<\/sub><br \/>\nCaCO<sub>3<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Phosphoric acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">H<sub>3<\/sub>PO<sub>4<\/sub><\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Phosphate<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Iron(lll) <strong>phosphate<\/strong> Ammonium <strong>phosphate<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">FePO<sub>4<\/sub><br \/>\n(NH<sub>4<\/sub>)<sub>3<\/sub>PO<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"106\">Ethanoic acid<\/td>\n<td style=\"text-align: center;\" width=\"74\">CH<sub>3<\/sub>COOH<\/td>\n<td style=\"text-align: center;\" width=\"84\"><strong>Ethanoate<\/strong><br \/>\nsalts<\/td>\n<td style=\"text-align: center;\" width=\"186\">Lead(ll) <strong>ethanoate<\/strong> Copper(ll) <strong>ethanoate<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\">Pb(CH<sub>3<\/sub>COO)<sub>2<\/sub><br \/>\nCu(CH<sub>3<\/sub>COO)<sub>2<\/sub><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Salts can be acidic, basic, or neutral. Acidic salts are formed when a strong acid reacts with a weak base. Basic salts are formed when a strong base reacts with a weak acid. When a strong acid reacts with a strong base, neutral salts are formed.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-111982\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-2.png\" alt=\"Classification of Salts 2\" width=\"833\" height=\"682\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-2.png 833w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-2-300x246.png 300w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-2-768x629.png 768w\" sizes=\"(max-width: 833px) 100vw, 833px\" \/><\/p>\n<p><span style=\"color: #993366;\"><strong>Types of Salts:<\/strong><\/span><br \/>\nThe different types of salts are: normal salt, acid salt, basic salt and double salt.<\/p>\n<p><span style=\"color: #993366;\"><strong style=\"line-height: 1.5;\">1. Normal salt<\/strong><\/span><span style=\"line-height: 1.5;\"><span style=\"color: #993366;\"> :<\/span> A salt that does not contain any replaceable hydrogen atoms or hydroxyl groups is called normal salt.<\/span><br \/>\n<strong>Examples :<\/strong><br \/>\nNa<sub>2<\/sub>SO<sub>4<\/sub> obtained in the reaction between H<sub>2<\/sub>SO<sub>4<\/sub> and NaOH is a normal salt because it is formed by the complete replacement of both the H atoms of H<sub>2<\/sub>SO<sub>4<\/sub>,<br \/>\nSimilarly, calcium su1phate (CaSO<sub>4<\/sub>), sodium phosphate (Na<sub>3<\/sub>PO<sub>4<\/sub>) and potassium phosphate (K<sub>3<\/sub>PO<sub>4<\/sub>) are also normal salts.<\/p>\n<p><span style=\"color: #993366;\"><strong style=\"line-height: 1.5;\">2. Acid salt :<\/strong><\/span><span style=\"line-height: 1.5;\"> When a polybasic acid is not completely neutralized by a base, the salt produced will contain replaceable hydrogen atoms. Hence, it may further take part in the reaction with the base as an acid. Such a salt is called an acid salt. For example, the salt NaHSO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\"> produced in the reaction between NaOH and H<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">SO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\"> is an acid salt because it is capable of further reaction with the base NaOH to produce the normal salt Na<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">SO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\">.<\/span><\/p>\n<p>H<sub>2<\/sub>SO<sub>4<\/sub> + NaOH \u00a0\u2192 \u00a0<span style=\"line-height: 1.5;\">NaHSO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\"> + H<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">O<\/span><br \/>\nNaHSO<sub>4<\/sub> + NaOH \u00a0\u2192 \u00a0<span style=\"line-height: 1.5;\">Na<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">SO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\"> + H<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">O<\/span><\/p>\n<p>Thus, an acid salt may be defined as follows.<br \/>\nA salt that contains replaceable hydrogen atoms is called an acid salt.<br \/>\n<strong>Examples :<\/strong><br \/>\nNaHSO<sub>4<\/sub>, NaH<sub>2<\/sub>PO<sub>4<\/sub> and Na<sub>2<\/sub>HPO<sub>4<\/sub> are examples of acid salts.<\/p>\n<p><span style=\"color: #993366;\"><strong style=\"line-height: 1.5;\">3. Basic salt :<\/strong><\/span><span style=\"line-height: 1.5;\"> When a polyacidic base reacts with lesser amount of acid than is necessary for complete neutralization, the salt produced contain hydroxyl group(s) (OH) also. Such a salt is called a basic salt.<\/span><br \/>\n<strong>Examples :<\/strong><br \/>\n1 mole of Pb(OH)<sub>2<\/sub> requires 2 moles of HCl for complete neutralization. But when 1 mole of Pb(OH)<sub>2<\/sub> is made to react with 1 mole of HCl, some Pb(OH)<sub>2<\/sub> is left unreacted. The salt produced is not PbCl<sub>2<\/sub>, but Pb(OH)Cl.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-111985\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-3.png\" alt=\"Classification of Salts 3\" width=\"321\" height=\"48\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-3.png 321w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-3-300x45.png 300w\" sizes=\"(max-width: 321px) 100vw, 321px\" \/><br \/>\nSimilarly, when one mole of Bi(OH)<sub>3<\/sub> is reacted with 1 mole of HNO<sub>3<\/sub>, the salt Bi(OH)<sub>2<\/sub>NO<sub>3<\/sub> is formed.<\/p>\n<p>Bi(OH)<sub>3<\/sub> + HNO<sub>3<\/sub>\u00a0 \u2192 \u00a0Bi(OH)<sub>2<\/sub>NO<sub>3<\/sub> + H<sub>2<\/sub>O<\/p>\n<p>Salts like Pb(OH)Cl and Bi(OH)<sub>2<\/sub>NO<sub>3<\/sub> contain the OH group. These salts are called basic salts, because they can further react with the acids to form H<sub>2<\/sub>O and the corresponding normal salts.<\/p>\n<p>Pb(OH)Cl + HCl \u00a0\u2192 \u00a0PbCl<sub>2<\/sub> +H<sub>2<\/sub>O<\/p>\n<p>Bi(OH)<sub>2<\/sub>NO<sub>3<\/sub> + HNO<sub>3<\/sub>\u00a0 \u2192 \u00a0Bi(OH)(NO<sub>3<\/sub>)<sub>2<\/sub> + H<sub>2<\/sub>O<\/p>\n<p>Bi(OH)(NO<sub>3<\/sub>)<sub>2<\/sub> + HNO<sub>3 \u00a0<\/sub>\u2192 \u00a0Bi(NO<sub>3<\/sub>)<sub>3<\/sub> + H<sub>2<\/sub>O<\/p>\n<p>Thus, a basic salt is formed when a poly acidic base reacts with a lesser amount of an acid than is necessary for the formation of a normal salt.<\/p>\n<p><span style=\"color: #993366;\"><strong style=\"line-height: 1.5;\">4. Double salt :<\/strong><\/span><span style=\"line-height: 1.5;\"> In a double salt, there are two different negative ions and\/or positive ions. For example, the mineral dolomite, CaCO<\/span><sub>3<\/sub><span style=\"line-height: 1.5;\">\u00b7MgCO<\/span><sub>3<\/sub><span style=\"line-height: 1.5;\">, contains both Ca<\/span><sup>2+<\/sup><span style=\"line-height: 1.5;\"> and Mg<\/span><sup>2+<\/sup><span style=\"line-height: 1.5;\"> ions. Hence, it is a double salt. Potash alum, K<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">SO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\">\u00b7Al<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">(SO<\/span><sub>4<\/sub><span style=\"line-height: 1.5;\">)<\/span><sub>3<\/sub><span style=\"line-height: 1.5;\">.24H<\/span><sub>2<\/sub><span style=\"line-height: 1.5;\">O, also is a double salt.<\/span><br \/>\nDouble salts exist only in the solid state. When dissolved in water, they break up into a mixture of two separate salts. For example, when potash alum is dissolved in water, it breaks up as follows.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-111986\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-4.png\" alt=\"Classification of Salts 4\" width=\"310\" height=\"108\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-4.png 310w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/04\/Classification-of-Salts-4-300x105.png 300w\" sizes=\"(max-width: 310px) 100vw, 310px\" \/><\/p>\n<h3><strong>Solubility of salts in water<\/strong><\/h3>\n<ol>\n<li>Salts are ionic compounds and they can dissolve in water. However, through experiments conducted by chemists not all salts are found to be soluble in water.<\/li>\n<li>For example, sodium chloride, NaCl dissolves readily in water, but silver chloride, AgCl cannot dissolve in water.<\/li>\n<li>Table lists out some common soluble and insoluble salts.<\/li>\n<\/ol>\n<p><strong>Table: Solubility of salts in water<\/strong><\/p>\n<table style=\"height: 224px;\" border=\"2\" width=\"627\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"97\"><strong>Type of salt<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"192\"><strong>Solubility in water<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Ammonium salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Sodium and potassium salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Ethanoate salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Nitrate salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Chloride salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble except AgCl, HgCI and PbCl<sub>2<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Sulphate salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are soluble except PbSO<sub>4<\/sub>, CaSO<sub>4<\/sub>, BaSO<sub>4<\/sub>, and Ag2SO<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Carbonate salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are insoluble except Na<sub>2<\/sub>CO<sub>3<\/sub>, K2CO<sub>3<\/sub>, and (NH<sub>4<\/sub>)2CO<sub>3<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"97\">Lead(ll) salts<\/td>\n<td style=\"text-align: center;\" width=\"192\">All are insoluble except Pb(NO<sub>3<\/sub>)<sub>2<\/sub> and Pb(CH<sub>3<\/sub>COO)<sub>2<\/sub><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><span style=\"color: #993366;\"><strong>Activity<\/strong><\/span><br \/>\n<strong>Aim:<\/strong> To demonstrate a neutralization reaction<br \/>\n<strong>Materials needed:<\/strong> Sodium hydroxide, dilute hydrochloric acid, and phenolphthalein<br \/>\n<strong>Method:<\/strong><br \/>\nTake 30 ml of dilute sodium hydroxide solution in a conical flask and add a drop of phenolphthalein to it. Now pour hydrochloric acid to it dropwise, usjng a dropper till there is some change in the colour of the solution.<br \/>\n<strong>Observation:<\/strong> The solution turns pink when phenolphthalein is added to sodium hydroxide. The solution turns colourless when the entire sodium hydroxide has reacted. On testing the colourless solution with litmus paper, there is no change either with red litmus or blue litmus paper.<br \/>\n<strong>Conclusion:<\/strong> There is no change in the colour of the litmus paper indicating that the solution has turned neutral.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Classification of Salts What is a salt? A salt is formed in a neutralisation reaction between an acid and a base.\u00a0Salt is a general term used for the substances that are formed when an acid and a base react with each other. This reaction is called a neutralization reaction. Acid + base \u2192\u00a0salt + water [&hellip;]<\/p>\n","protected":false},"author":2,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[151,153,4687,152,150,4685,149,4686],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v17.8 (Yoast SEO v17.8) - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Classification of Salts - A Plus Topper<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.aplustopper.com\/classification-of-salts\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Classification of Salts\" \/>\n<meta property=\"og:description\" content=\"Classification of Salts What is a salt? 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A salt is formed in a neutralisation reaction between an acid and a base.\u00a0Salt is a general term used for the substances that are formed when an acid and a base react with each other. This reaction is called a neutralization reaction. 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