{"id":13178,"date":"2022-11-18T16:00:43","date_gmt":"2022-11-18T10:30:43","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=13178"},"modified":"2022-11-19T16:31:45","modified_gmt":"2022-11-19T11:01:45","slug":"qualitative-analysis-salts","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/qualitative-analysis-salts\/","title":{"rendered":"Qualitative Analysis of Salts"},"content":{"rendered":"<h2><strong>Qualitative Analysis of Salts<\/strong><\/h2>\n<p><strong>What is qualitative analysis?<\/strong><\/p>\n<ol>\n<li><strong>Qualitative analysis<\/strong> of a salt Analysis is a chemical technique used to identify the <strong>ions<\/strong> present in a salt by analysing its physical and chemical properties and hence determine the identity of the salt.<\/li>\n<li>It determines only the presence or absence of a particular ion in a given salt. This method does not determine how much of a particular ion is present.<\/li>\n<li>For example, a student did a chemical analysis on a sample of salt X. His results showed the presence of sodium ions and bromide ions. His conclusion was the salt must be sodium bromide.<\/li>\n<li>The procedure for testing salts in the laboratory consists of the following general steps.\n<ol>\n<li>Make initial observations of the physical properties of the salt.<\/li>\n<li>Study the action of heat on the salt.<\/li>\n<li>Make aqueous solution of the salt to test for anions and cations present.<\/li>\n<li>Carry out confirmatory tests for cations and anions.<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>People also ask<\/strong><\/p>\n<ul>\n<li><a href=\"https:\/\/www.aplustopper.com\/classification-of-salts\/\">Classification of Salts<\/a><\/li>\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\/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<h2><strong>Examining the colour and solubility of salts in water<\/strong><\/h2>\n<ol>\n<li>Preliminary examination on the physical properties of a salt such as <strong>colour<\/strong> and <strong>solubility<\/strong> in water can help to indicate that certain cations and anions might be present.<\/li>\n<li>Observations of physical properties only allow you to make inferences on the <strong>possibility<\/strong> of the presence of certain ions in the salts. This is because it is possible to have more than one salt sharing the same physical properties. For example:<br \/>\n(a) Iron(II) ions, nickel(II) ions and chromium(III) ions dissolve in water to produce green solutions.<br \/>\n(b) Sodium chloride and potassium carbonate are white solids. Both solids dissolve in water to produce colourless solutions.<\/li>\n<li>Hence, observations of physical properties of salts cannot be used to confirm the identities of the ions. Its main purpose is to help us narrow down the choices of cations and anions present in a salt. Chemical tests still have to be carried out to confirm these ions.<\/li>\n<\/ol>\n<p><strong>Table lists the colours of some common salts.<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" rowspan=\"2\" width=\"215\"><strong>Salt<\/strong><\/td>\n<td style=\"text-align: center;\" colspan=\"2\" width=\"186\"><strong>Colour<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"90\"><strong>Solid<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"96\"><strong>Aqueous solution<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\">Potassium salts<br \/>\nSodium salts<br \/>\nAmmonium salts<br \/>\nAluminium salts<br \/>\nCalcium salts<br \/>\nLead(ll) salts<br \/>\nZinc salts<br \/>\n(with colourless anions)<\/td>\n<td style=\"text-align: center;\" width=\"90\">White<\/td>\n<td style=\"text-align: center;\" width=\"96\">Colourless<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\">Carbonate salts<br \/>\nChloride salts<br \/>\nNitrate salts<br \/>\nSulphate salts<br \/>\n(with colourless cations)<\/td>\n<td style=\"text-align: center;\" width=\"90\">White<\/td>\n<td style=\"text-align: center;\" width=\"96\">Colourless<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\"><strong>Iron(II) salts:<\/strong><br \/>\nIron(II) chloride Iron(II) nitrate iron(II) sulphate<\/td>\n<td style=\"text-align: center;\" width=\"90\">Green<\/td>\n<td style=\"text-align: center;\" width=\"96\">Green<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\"><strong>Iron(III) salts:<\/strong><br \/>\nIron(III) chloride<br \/>\nIron(III) nitrate<br \/>\nIron(III) sulphate<\/td>\n<td style=\"text-align: center;\" width=\"90\">Brown<\/td>\n<td style=\"text-align: center;\" width=\"96\">Brown<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\"><strong>Copper(II) salts:<\/strong><br \/>\nCopper(II) chloride<br \/>\nCopper(II) nitrate<br \/>\nCopper(II) sulphate<\/td>\n<td style=\"text-align: center;\" width=\"90\">Blue<\/td>\n<td style=\"text-align: center;\" width=\"96\">Blue<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"215\">\u00a0Copper(II) carbonate<\/td>\n<td style=\"text-align: center;\" width=\"90\">\u00a0Green<\/td>\n<td style=\"text-align: center;\" width=\"96\">(Insoluble)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>Table shows the solubility of some common compounds.<\/strong><\/p>\n<table style=\"height: 330px;\" border=\"2\" width=\"714\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"127\"><strong>Compound<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"161\"><strong>Solubility in water<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Sodium, potassium and ammonium salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are soluble<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Nitrate salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are soluble<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Ethanoate salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are soluble<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Chloride salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are soluble except AgCl, HgCl and PbCl<sub>2<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Sulphate salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are soluble except BaSO<sub>4<\/sub>, PbSO<sub>4<\/sub> and CaSO<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Carbonate salts<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are insoluble except Na<sub>2<\/sub>CO<sub>3<\/sub>, K2CO<sub>3<\/sub> and (NH<sub>4<\/sub>)<sub>2<\/sub>CO<sub>3<\/sub><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Metal oxides<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are insoluble except Na<sub>2<\/sub>O, K<sub>2<\/sub>O and CaO (slightly soluble)<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"127\">Metal hydroxides<\/td>\n<td style=\"text-align: center;\" width=\"161\">All are insoluble except NaOH, KOH and Ba(OH)<sub>2<\/sub><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>Example:\u00a0<\/strong>Preliminary examination of solid X gave the following observations. Identify solid X. Explain your answer.<\/p>\n<ul>\n<li>Green solid that insoluble in water<\/li>\n<li>Dissolved in dilute acid with effervescence to form a blue solution<\/li>\n<\/ul>\n<p><strong>Solution:<\/strong><\/p>\n<ul>\n<li>The colour of an aqueous solution of a substance gives a more accurate inference about the nature of the ion present. Blue solution indicates presence of Cu<sup>2+<\/sup> ion.<\/li>\n<li>When a metal reacts with an acid, effervescence due to hydrogen gas liberated is observed. Effervescence due to carbon dioxide gas is seen when an acid reacts with a carbonate salt. Most metals are grey solids. Hence, the green solid X has to be a carbonate salt. X is copper(II) carbonate.<\/li>\n<\/ul>\n<p><strong>Test for gases<\/strong><\/p>\n<ol>\n<li>Gases are often produced from reactions carried out during laboratory tests on salts. Gases can be evolved when<br \/>\n(a) salts are heated.<br \/>\n(b) salts are reacted with acids or alkalis.<\/li>\n<li>For example:<br \/>\n(a) Heating a carbonate salt produces carbon dioxide gas.<br \/>\n(b) Reacting a metal with dilute acids produces hydrogen gas.<\/li>\n<li>By identifying the gases evolved, it is possible to infer the types of cations or anions present in a salt.<\/li>\n<li>A gas can be identified by its colour, smell, effect on litmus paper and reactions with special reagents.<\/li>\n<\/ol>\n<table style=\"height: 3232px;\" border=\"2\" width=\"866\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"288\"><strong>Gas<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"336\"><strong>Characteristic<\/strong><\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Ammonia<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Bring a piece of moist red litmus paper to the mouth of the test tube.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-112086 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-1.png\" alt=\"Qualitative Analysis of Salts 1\" width=\"219\" height=\"186\" \/><\/li>\n<\/ul>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Red litmus paper turns blue.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>Pungent smell<\/li>\n<li>Alkaline gas<\/li>\n<li>Turns moist red litmus paper blue<br \/>\nForms dense white fumes with hydrogen chloride Produced by heating a mixture of ammonium salt and alkali<br \/>\nNH<sub>4<\/sub>Cl(s) + NaOH(aq) \u2192\u00a0NaCl(aq) + NH<sub>3<\/sub>(g) + H<sub>2<\/sub>O(l)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Oxygen<br \/>\nMethod: <\/strong><\/p>\n<ul>\n<li>Lower a glowing wooden splint into the test tube.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-112088 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-2.png\" alt=\"Qualitative Analysis of Salts 2\" width=\"208\" height=\"184\" \/><\/li>\n<\/ul>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Glowing wooden splint is relighted.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>No effect on litmus paper<\/li>\n<li>Supports combustion<\/li>\n<li>Relights a glowing wooden splint<\/li>\n<li>Produced by heating a chlorate(V) or nitrate salt<br \/>\n2KClO<sub>3<\/sub>(s) \u2192\u00a02KCl(s) + 3O<sub>2<\/sub>(g)<br \/>\n2Pb(NO<sub>3<\/sub>)<sub>2<\/sub>(s) \u2192\u00a02PbO(s) + 4NO<sub>2<\/sub>(g) + O<sub>2<\/sub>(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Carbon dioxide<br \/>\nMethod:<\/strong><\/p>\n<ul>\n<li>Bubble the gas through\u00a0limewater.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-112091 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-3.png\" alt=\"Qualitative Analysis of Salts 3\" width=\"253\" height=\"153\" \/><\/li>\n<\/ul>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Limewater turns milky (chalky).<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>Acidic gas<\/li>\n<li>Turns moist blue litmus paper red<\/li>\n<li>Turns limewater milky<\/li>\n<li>Produced by heating a metal carbonate or acid- carbonate reaction<br \/>\nCaCO<sub>3<\/sub>(s) \u2192 CaO(s) + C02(g)<br \/>\nCaCO<sub>3<\/sub>(s) + 2HCl(aq) \u2192\u00a0CaCl<sub>2<\/sub>(aq) + H<sub>2<\/sub>O(l) + CO<sub>2<\/sub>(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Hydrogen<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Bring a lighted wooden splint to the mouth of the test tube.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-112093 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-4.png\" alt=\"Qualitative Analysis of Salts 4\" width=\"218\" height=\"151\" \/><\/li>\n<\/ul>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Gas burns with a \u2018pop\u2019 sound.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>No effect on litmus paper<\/li>\n<li>Forms an explosive mixture with air<\/li>\n<li>Burns with a \u2018pop\u2019 sound<\/li>\n<li>Produced by an acid-metal reaction<br \/>\nMg(s) + 2HCl(aq) \u2192\u00a0MgCl<sub>2<\/sub>(aq) + H<sub>2<\/sub>(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Chlorine<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Bring a piece of moist blue litmus paper to the mouth of the test tube.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"size-full wp-image-112096 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-5.png\" alt=\"Qualitative Analysis of Salts 5\" width=\"211\" height=\"190\" \/><\/li>\n<\/ul>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Blue litmus paper turns red. It is then bleached.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Greenish-yellow gas<\/li>\n<li>Pungent smell Acidic gas<\/li>\n<li>Turns moist blue litmus paper red<\/li>\n<li>Bleaches litmus paper<\/li>\n<li>Produced by heating a mixture of manganese(IV) oxide and concentrated hydrochloric acid<br \/>\nMnO<sub>2<\/sub>(s) + 4HCl(aq) \u2192\u00a0MnCl<sub>2<\/sub>(aq) + Cl<sub>2<\/sub>(g) + 2H<sub>2<\/sub>0(l)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Sulphur dioxide<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Bubble the gas through acidified K2Cr207 solution or acidified KMn04 solution<\/li>\n<\/ul>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-112097 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-6.png\" alt=\"Qualitative Analysis of Salts 6\" width=\"256\" height=\"174\" \/><\/p>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>The orange K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7\u00a0<\/sub>solution turns green or the purple KMnO<sub>4<\/sub> solution turns colourless.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>Pungent smell<\/li>\n<li>Acidic gas<\/li>\n<li>Turns moist blue litmus paper red<\/li>\n<li>Reduces orange acidified dichromate(VI) ion to green chromium(III) ion<\/li>\n<li>Decolourises purple acidified manganate(VII) ion Produced by an acid-sulphite reaction<br \/>\nNa<sub>2<\/sub>SO<sub>3<\/sub>(s) + 2HCl(aq) \u2192\u00a02NaCl(aq) + H<sub>2<\/sub>O(l) + SO<sub>2<\/sub>(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Hydrogen chloride<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Use a glass rod to bring a drop of concentrated ammonia solution to the mouth of the test tube.<\/li>\n<\/ul>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-112118 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-7.png\" alt=\"Qualitative Analysis of Salts 7\" width=\"271\" height=\"193\" \/><\/p>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Dense white fumes are formed.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Colourless gas<\/li>\n<li>Forms fumes in moist air<\/li>\n<li>Acidic gas<\/li>\n<li>Turns moist blue litmus paper red<\/li>\n<li>Forms dense white fumes with ammonia gas<\/li>\n<li>Produced by heating a mixture of common salt and concentrated sulphuric acid<br \/>\nH<sub>2<\/sub>SO<sub>4<\/sub>(aq) + NaCl(s) \u2192\u00a0NaHSO<sub>4<\/sub>(aq) + HCl(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<tr>\n<td width=\"288\"><strong>Nitrogen dioxide<br \/>\n<\/strong><strong>Method:<\/strong><\/p>\n<ul>\n<li>Bring a piece of moist blue litmus paper to the mouth of the test tube.<\/li>\n<li>Observe the colour of gas evolved.<\/li>\n<\/ul>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-112120 aligncenter\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/05\/Qualitative-Analysis-of-Salts-8.png\" alt=\"Qualitative Analysis of Salts 8\" width=\"259\" height=\"188\" \/><\/p>\n<p><strong>Observation:<\/strong><\/p>\n<ul>\n<li>Blue litmus paper turns red.<\/li>\n<li>Brown gas is evolved.<\/li>\n<\/ul>\n<\/td>\n<td width=\"336\">\n<ul>\n<li>Brown gas<\/li>\n<li>Pungent smell<\/li>\n<li>Acidic gas<\/li>\n<li>Turns moist blue litmus paper red<\/li>\n<li>Reacts with water to form colourless solution<\/li>\n<li>Produced by heating a nitrate salt<br \/>\n2Cu(NO<sub>3<\/sub>)O<sub>2<\/sub>(s) \u2192\u00a02CuO(s) + 4NO<sub>2<\/sub>(g) + O<sub>2<\/sub>(g)<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>&nbsp;<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Qualitative Analysis of Salts What is qualitative analysis? Qualitative analysis of a salt Analysis is a chemical technique used to identify the ions present in a salt by analysing its physical and chemical properties and hence determine the identity of the salt. It determines only the presence or absence of a particular ion in a [&hellip;]<\/p>\n","protected":false},"author":3,"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":[4748,4746,4745,4743,4742,157,4747,4744],"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>Qualitative Analysis 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\/qualitative-analysis-salts\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Qualitative Analysis of Salts\" \/>\n<meta property=\"og:description\" content=\"Qualitative Analysis of Salts What is qualitative analysis? Qualitative analysis of a salt Analysis is a chemical technique used to identify the ions present in a salt by analysing its physical and chemical properties and hence determine the identity of the salt. 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