{"id":5998,"date":"2020-10-13T12:16:48","date_gmt":"2020-10-13T06:46:48","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=5998"},"modified":"2020-10-13T12:16:36","modified_gmt":"2020-10-13T06:46:36","slug":"qualitative-analysis-anions","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/qualitative-analysis-anions\/","title":{"rendered":"Qualitative analysis – Anions"},"content":{"rendered":"

<\/h4>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
CHEMICAL TEST FOR<\/span><\/b><\/td>\nTEST METHOD<\/span><\/b><\/td>\nOBSERVATIONS<\/span><\/b><\/td>\nTEST CHEMISTRY<\/span><\/b><\/td>\n<\/tr>\n
Chemical test for Carbonate ion CO3<\/sub>2\u2013<\/sup> or hydrogencarbonate HCO3<\/sub>\u2013<\/sup> ion<\/span><\/b>\"test<\/span><\/p>\n

Acid is added to the solid carbonate in a test tube. You could also collect a sample of gas from a heated carbonate, i.e. the solid is where the liquid is in the left hand test tube.<\/span><\/p>\n

 <\/td>\n

(i)<\/b> Add any dilute strong acid<\/b> to the suspected solid carbonate \u2013 if colourless gas <\/b>given off, test with limewater<\/b>.<\/span>(ii)<\/b> Effect of fairly strong heating and testing for any carbon dioxide given off.<\/span><\/p>\n

Test (ii) will distinguish<\/b> sodium hydrogencarbonate (NaHCO3<\/sub><\/b> readily decomposes \u2013 ‘baking powder’) from anhydrous sodium carbonate (Na2<\/sub>CO3<\/sub><\/b>, thermally very stable).<\/span><\/td>\n

(i)<\/b> Fizzing \u2013 colourless gas<\/b>which turns limewater milky \u2013 cloudy fine white precipitate<\/b>\u00a0<\/span>(ii)<\/b> There might be colour changes in the solid, but you need to collect a sample of gas from just above the heated solid to see it gives a white precipitate with limewater.<\/span><\/p>\n

Apart from hydrated sodium carbonate, sodium hydrogencarbonate is one of the few common carbonates to give off water on heating and condenses on side of test tube, but basic carbonates will also give off H2<\/sub>O as well as CO2<\/sub>.<\/span><\/td>\n

(i)<\/b> To identify any carbonate\/hydrogencarbonate + acid <\/b>==> salt + water + carbon dioxide<\/b>, then white precipitate with limewater. The ionic equations are for carbonate …<\/span><\/span>CO3<\/sub>2\u2013<\/sup><\/b>(s)<\/sub> + 2H+<\/sup>(aq)<\/sub> ==> H2<\/sub>O(l)<\/sub> + CO<\/b>2<\/b>(g)<\/sub><\/span><\/p>\n

and for the hydrogencarbonate …<\/span><\/p>\n

HCO3<\/sub>\u2013<\/sup><\/b>(s)<\/sub> + H+<\/sup>(aq)<\/sub> ==> H2<\/sub>O(l)<\/sub> + CO<\/b>2<\/b>(g)<\/sub><\/span><\/p>\n

(ii)<\/b> The thermal decomposition equations are for carbonates<\/span><\/p>\n

MCO<\/b>3<\/b>(s)<\/sub> ==>MO(s) + CO<\/b>2<\/b>(g)<\/sub><\/span><\/p>\n

e.g. M = Mg, Zn, CuO and note that some give clear colour changes in the solid which might be useful to identify the metal\u00a0<\/span><\/p>\n

and for sodium hydrogencarbonate …<\/span><\/p>\n

2NaHCO<\/b>3<\/b>(s)<\/sub> ==> Na2<\/sub>CO3(s)<\/sub> + H2<\/sub>O(l)<\/sub> + CO<\/b>2<\/b>(g)<\/sub><\/span><\/td>\n<\/tr>\n

Sulphate ion\u00a0or sulphate(VI) ion SO4<\/sub>2\u2013<\/sup><\/b>[sulfate, sulfate(VI)] chemical test<\/span>If the solution also contains the chloride ion, you test with barium ions 1st, filter off any barium sulphate precipitate and then test for chloride ion. This is because silver sulphate is also ~insoluble.<\/span><\/td>\n(i) <\/b>To a solution of the suspected sulfate add dilute hydrochloric and a few drops of barium chloride\/ nitrate <\/b>solution.<\/span>(ii)<\/b> Add lead(II) nitrate solution.<\/span><\/td>\n(i)<\/b> A white precipitateof barium sulfate.<\/span>(ii)<\/b> A white precipitate of lead(II) sulphate.<\/span><\/p>\n

 <\/td>\n

(i)<\/b> Ba2+<\/sup>(aq)<\/sub> + SO4<\/sub>2\u2013<\/sup>(aq)<\/sub> <\/b>==> BaSO4(s)<\/sub><\/b><\/span>A<\/span>ny soluble barium salt + any soluble sulphate forms a white dense barium sulphate precipitate.<\/span><\/p>\n

(ii)<\/b> Pb2+<\/sup>(aq)<\/sub> + SO4<\/sub>2\u2013<\/sup>(aq)<\/sub> <\/b>==> PbSO4(s)<\/sub><\/b><\/span><\/p>\n

Neither white precipitate is soluble in excess hydrochloric acid.<\/span><\/td>\n<\/tr>\n

Sulphite ion or sulphate(IV) ion SO3<\/sub>2\u2013<\/sup><\/b>[sulfite, sulfate(IV)] chemical test<\/span>Test (iii) is easily unreliable, the sulphite ion is oxidised by air (dissolved oxygen) to give the sulphate ion, so you will lucky to obtain a clear solution after adding excess acid.<\/span><\/td>\n(i) <\/b>Add dilute hydrochloric acid to the suspected sulfite.<\/span>(ii)<\/b> Test any gas evolved with fresh potassium dichromate(VI) paper.<\/span><\/p>\n

(iii)<\/b> Add barium chloride or barium nitrate solution.<\/span><\/td>\n

<\/b>(i)<\/b> Acrid choking sulfur dioxide gas formed.<\/span>(ii)<\/b> The dichromate paper turns fromorange<\/b> to green<\/b>.<\/span><\/p>\n

(iii)<\/b> A white ppt.<\/b> of barium sulphite which dissolves in excess hydrochloric acid to give a clear colourless solution.<\/span><\/td>\n

(i)<\/b> <\/span>To identify any sulphite salt + hydrochloric acid <\/b>==> chloride salt + <\/b><\/span>sulphur dioxide<\/b>.<\/span>(ii)<\/b> The sulphur dioxide reduces the dichromate(VI) to chromium(III). Note:<\/span> sulphites do\u00a0 not give ppt. with acidified barium chloride\/nitrate because sulphites dissolve in acids.<\/span><\/p>\n

(iii)<\/b> Ba2+<\/sup>(aq)<\/sub> + SO3<\/sub>2\u2013<\/sup>(aq)<\/sub> <\/b>==> BaSO3(s)<\/sub><\/b><\/span><\/p>\n

BaSO3(s)<\/sub> + 2HCl(aq)<\/sub> <\/b>==> BaCl2(aq)<\/sub> + H2<\/sub>O(l)<\/sub> + SO2(aq)<\/sub><\/b><\/span><\/td>\n<\/tr>\n

Sulphide<\/span> ion S2\u2013<\/sup> (sulfide)<\/span><\/b> chemical test<\/span>In test (ii) dangerous hydrogen sulphide<\/b> (hydrogen sulfide) is formed.<\/b><\/span><\/td>\n(i)<\/b> If soluble, add a few drops lead(II) ethanoate solution.<\/span>(ii)<\/b> If solid, add dil. HCl(aq) acid, test smelly gas with damp lead(II) ethanoate paper (old name lead acetate<\/i>).<\/span><\/td>\n(i) Black precipitate<\/span><\/b>of lead sulphide.<\/span>(ii)<\/b> Rotten egg smell of hydrogen sulphide and the H2<\/sub>S gas turns lead(II) ethanoate paper black.<\/span><\/td>\n(i)<\/b> Pb2+<\/sup>(aq)<\/sub> + S2\u2013<\/sup><\/b>(aq)<\/sub> => PbS<\/b>(s)<\/sub>\u00a0<\/span>(ii)<\/b> MS<\/b>(s)<\/sub> + 2H+<\/sup>(aq)<\/sub> => M2+<\/sup>(aq)<\/sub> + H2<\/sub>S<\/b>(g)<\/sub> (e.g. M = Pb, Fe, Cu, Ni etc.) Then reaction (i) above occurs on the lead(II) ethanoate paper (old name lead acetate<\/i><\/b>).<\/span><\/td>\n<\/tr>\n
Chloride ion<\/span><\/b> chemical test<\/span>Cl\u2013<\/sup><\/span><\/b><\/p>\n

If the solution also contains the sulphate ion, you test with barium ions 1st, filter off any barium sulphate precipitate and then test for chloride ion. This is because silver sulphate is also ~insoluble, so the two precipitates of silver sulfate and silver chloride could not be distinguished<\/span><\/td>\n

(i)<\/b> If the chloride is soluble, add dilute nitric acid and silver nitrate solution. The silver nitrate is acidified with dilute nitric acid to prevent the precipitation of other non\u2013halide silver salts.<\/span>(ii)<\/b> If insoluble salt, add conc. sulphuric acid, warm if necessary then test gas as for HCl<\/b>.<\/span><\/p>\n

(iii)<\/b> Add lead(II) nitrate solution. Not a very specific test \u2013 test (i) is best.<\/span><\/td>\n

(i)<\/b> <\/span>white precipitate<\/b>of silver chloride soluble in dilute ammonia.<\/span>(ii)<\/b> You get nasty fumes of hydrogen chloride which turn blue litmus red<\/b> and give a white precipitate<\/b> with silver nitrate solution.<\/span><\/p>\n

(iii)<\/b> A white ppt.<\/b> of lead(II) chloride is formed.<\/span><\/td>\n

(i)<\/b> <\/span>Ag+<\/sup>(aq)<\/sub> + Cl\u2013<\/sup>(aq)<\/sub><\/b> ==> AgCl(s)<\/sub><\/b><\/span>A<\/span>ny soluble silver salt + any soluble chloride\u00a0 gives a white silver chloride precipitate<\/b>, that darkens in light.<\/span><\/p>\n

(ii)<\/span><\/b> Cl\u2013<\/sup>(s)<\/sub> + H2<\/sub>SO4(l) <\/sub>==> HSO4<\/sub>\u2013<\/sup>(s)<\/sub> + HCl(g)<\/sub> ,<\/span><\/p>\n

then Ag+<\/sup>(aq)<\/sub> + Cl\u2013<\/sup>(aq)<\/sub><\/b> ==> AgCl(s)<\/sub><\/b><\/span><\/p>\n

(iii)<\/b> Pb2+<\/sup>(aq)<\/sub> + 2Cl\u2013<\/sup><\/b>(aq)<\/sub> ==> PbCl<\/b>2<\/b>(s)<\/sub><\/span><\/td>\n<\/tr>\n

Bromide <\/span>ion <\/span><\/b>\u00a0chemical test<\/span>Br\u2013<\/sup><\/span><\/b><\/td>\n(i)<\/b> If bromide soluble, add dilute nitric acid and silver nitrate solution. The silver nitrate is acidified with dilute nitric acid to prevent the precipitation of other non\u2013halide silver salts.<\/span>(ii)<\/b> If insoluble salt, add conc. sulphuric acid, warm if necessary.<\/span><\/p>\n

(iii)<\/b> Add lead(II) nitrate solution. Not a very specific test \u2013 test (i) is best.<\/span><\/td>\n

(i)<\/b> C<\/b><\/span>ream precipitate<\/b> of silver bromide, only soluble in concentrated ammonia.<\/span>(ii)<\/b> O<\/b>range vapour<\/b> of bromine and pungent fumes of SO2<\/sub>, test for sulphur dioxide<\/b>.<\/span><\/span><\/p>\n

(iii)<\/b> A white ppt.<\/b> of lead(II) bromide is formed.<\/span><\/td>\n

(i)<\/b> <\/span>Ag+<\/sup>(aq)<\/sub> + Br\u2013<\/sup>(aq)<\/sub><\/b> ==> AgBr(s)<\/sub><\/b><\/span>Any soluble silver salt + any soluble bromide\u00a0gives a cream silver bromide<\/b> precipitate<\/span>.<\/span><\/p>\n

(ii)<\/b>\u00a0The<\/span> bromide ion is oxidised to bromine and the sulphuric acid is reduced to sulphur dioxide.<\/span><\/p>\n

(iii)<\/b> Pb2+<\/sup>(aq)<\/sub> + 2Br\u2013<\/sup><\/b>(aq)<\/sub> ==> PbBr2<\/sub><\/b>(s)<\/sub><\/span><\/td>\n<\/tr>\n

Fluoride Ion<\/span><\/b> chemical test<\/span>F\u2013<\/sup><\/span><\/b><\/p>\n

<\/b>Fluoride and hydrogen fluoride gas are harmful, irritating and corrosive substances.<\/span><\/td>\n

(i)<\/b> If the suspected fluoride is soluble add dilute nitric acid and silver nitrate solution.<\/span>(ii)<\/b> You can warm a solid fluoride with conc. sulphuric acid and hold in the fumes (ONLY!) a glass rod with a drop of water on the end.<\/span><\/td>\n(i)<\/b> There is NO precipitate<\/b>!<\/span>(ii)<\/b> Look for etching effects<\/b> on the surface of the glass rod.<\/span><\/td>\n(i)<\/b> Silver fluoride, AgF, is moderately soluble so this test proves little except that it isn’t chloride, bromide and iodide!<\/span>(ii)<\/b> Hydrogen fluoride gas is produced by displacement<\/span><\/p>\n

F\u2013<\/sup> + H2<\/sub>SO4<\/sub> ==> HSO4<\/sub>\u2013<\/sup> + HF <\/b>which reacts with the glass silica to form silicic acid, silicon oxyfluoride, silicon fluoride. The chemistry is messy and complex BUT the glass rod is clearly etched<\/b>.<\/span><\/td>\n<\/tr>\n

\n

Iodide<\/span> ion<\/span><\/b> chemical test<\/span><\/p>\n

I\u2013<\/sup>\u00a0<\/span><\/b><\/p>\n<\/td>\n

(i)<\/b> If iodide soluble, add dilute nitric acid and silver nitrate solution. The silver nitrate is acidified with dilute nitric acid to prevent the precipitation of other non\u2013halide silver salts.<\/span>(ii)<\/b> If insoluble salt can heat with conc. sulphuric acid, (ii) get purple fumes of iodine and very smelly hydrogen sulphide.<\/span><\/p>\n

(iii)<\/b> If iodide soluble, add lead(II) nitrate solution.<\/span><\/td>\n

(i)<\/b> <\/span>Yellow precipitate<\/b> of silver iodide insoluble in concentrated ammonia.<\/span>(ii)<\/b> purple vapour<\/b>and rotten egg smell!<\/span><\/p>\n

(iii)<\/b> <\/span>Yellow precipitate of lead(II) iodide. Not too definitive \u2013Test (i) best.<\/span><\/td>\n

(i)<\/b> <\/span>Ag+<\/sup>(aq)<\/sub> + I\u2013<\/sup>(aq)<\/sub><\/b> ==> AgI(s)<\/sub><\/b><\/span>any soluble silver salt + any soluble iodide\u00a0 ==> yellow silver iodide precipitate,<\/span><\/p>\n

(ii)<\/b> <\/span>iodide ion is oxidised to iodine and the sulphuric acid is reduced to ‘rotten eggs’ smelly hydrogen sulphide,<\/span><\/p>\n

(iii)<\/b> insoluble lead(II) iodide formed<\/span><\/p>\n

Pb2+<\/sup>(aq)<\/sub> + 2I\u2013<\/sup>(aq)<\/sub> ==> PbI<\/b>2<\/b>(s)<\/sub><\/span><\/td>\n<\/tr>\n

Nitrate ion or nitrate(V) ion NO3<\/sub>\u2013<\/sup><\/span><\/b>chemical test<\/span><\/td>\n(i)<\/b> Boil the suspected nitrate with sodium hydroxide solution and fine aluminium powder (Devarda’s Alloy) or aluminium foil.<\/span>(ii)<\/b> Add iron(ii) sulphate solution and then conc. sulphuric acid (the ‘brown ring<\/span>‘<\/b>test)<\/span><\/p>\n

(iii)<\/b> Strongly heating nitrates of M2+<\/sup> salts.<\/span><\/td>\n

(i)<\/b> the fumes contain ammonia, which turns redlitmus blue<\/b>,\u00a0<\/span>(ii)<\/b> Where the liquids meet a brown ringforms<\/span><\/p>\n

(iii)<\/b> Nasty brown gas<\/b> (beware!) ofnitrogen (IV) oxide<\/b> (nitrogen dioxide)<\/span><\/td>\n

(i)<\/b> The aluminium powder is a powerful reducing agent and converts the nitrate ion, NO3<\/sub>\u2013<\/sup><\/b>, into ammonia gas, NH3<\/sub><\/b><\/span>(ii)<\/b> NO complex of iron(II) formed<\/span><\/p>\n

(iii)<\/b> a general thermal decomposition equation for this reaction is<\/span><\/p>\n

2M(NO3<\/sub>)2(s)<\/sub> ==> 2MO(s)<\/sub> + 4NO<\/span>2<\/span>(g)<\/sub><\/b> + O<\/span>2(g)<\/span><\/sub><\/p>\n

where M = Pb, Zn, Mg, Cu etc.<\/span><\/td>\n<\/tr>\n

Nitrite ion or nitrate(III) ion NO2<\/sub>\u2013<\/sup><\/span><\/b>chemical test<\/span><\/td>\n(i) in acid solution it decomposes to give colourless NO gas which rapidly oxidises to nasty brown fumes of NO2<\/sub>, (ii) it decolourises (purple ==> colourless) acidified potassium manganate(VII), (iii) it liberates iodine from acidified potassium iodide solution, (iv) forms ammonia with hot Al powder\u2013foil\/NaOH(aq)<\/sub>\u00a0 and gives ‘brown ring’ test\u00a0<\/span><\/td>\n<\/tr>\n
Alkali:<\/span><\/b><\/b>Hydroxide ion<\/span><\/b> chemical test<\/span> i.e. a soluble base (alkali) which forms the OH\u2013 <\/sup>ion in water (note: to completely identify alkalis you need to test for the cation e.g. sodium for NaOH etc.)<\/span><\/b><\/td>\n(i)<\/b>Litmus or universal indicator or pH meter.<\/span>(ii)<\/b> Add a little of an ammonium salt.<\/span><\/td>\n(i)<\/b> It turns litmus<\/b><\/b>blue<\/b>, variety of colours univ. ind. dark green \u2013 violet for weak \u2013 strong.<\/span>(ii) If strongly alkaline ammonia should be released,<\/span><\/td>\n(i)<\/b>\u00a0A pH meter gives a value of more than 7, the higher the pH number the stronger the alkali, the higher the OH\u2013<\/sup>concentration, (ii) ammonia gas is evolved:<\/span>(ii)<\/b> Ammonia released from the salt.<\/span><\/p>\n

NH4<\/sub>+<\/sup>(aq)<\/sub> + OH\u2013<\/sup>(aq)<\/sub> ==> NH3(g)<\/sub> + H2<\/sub>O(l)<\/sub><\/span><\/td>\n<\/tr>\n

Chromate(VI) ion<\/span><\/b> chemical test<\/span>CrO4<\/sub>2\u2013<\/sup><\/b> (yellow)<\/span><\/p>\n

These tests are not very definitive, but collectively they are a good ‘pointer’!<\/span><\/td>\n

(i) Add dilute sulphuric acid.<\/span>(ii) Add barium chloride\/nitrate solution.<\/span><\/p>\n

(iii) Add lead(II) nitrate solution.<\/span><\/td>\n

(i) The yellow<\/b>solution turns orangeas the dichromate(VI) ion is formed.<\/span>(ii) A yellow precipitate<\/b> of barium chromate(VI) is formed.<\/span><\/p>\n

(iii) A yellow precipitate<\/b> of lead(II) chromate(VI) is formed. ‘lead chromate<\/i>‘<\/span><\/td>\n

(i) CrO4<\/sub>2\u2013<\/sup>(aq)<\/sub> + 2H+<\/sup>(aq)<\/sub> ==> Cr2<\/sub>O7<\/sub>2\u2013<\/sup>(aq)<\/sub><\/span>(ii) Ba2+<\/sup>(aq)<\/sub> + CrO4<\/sub>2\u2013<\/sup>(aq)<\/sub> ==> BaCrO4(s<\/sub>)<\/span><\/p>\n

(iii) Pb2+<\/sup>(aq)<\/sub> + CrO4<\/sub>2\u2013<\/sup>(aq)<\/sub> ==> PbCrO4(s<\/sub>)<\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

<\/h4>\n

Tests for S2<\/sub>O3<\/sub>2-<\/sup><\/h4>\n

S2<\/sub>O3<\/sub>2-<\/sup>(aq) + dil.HCl\u00a0\u2192 SO2<\/sub>(g) + S(s)<\/p>\n

S2<\/sub>O3<\/sub>2-<\/sup>(aq) +AgNO3<\/sub>(aq)<\/span>\u00a0\u2192 \u00a0Ag2<\/sub>S2<\/sub>O3<\/sub>\u00a0(aq) \u00a0\u2192\u0394 \u00a0<\/sub>Ag2<\/sub>S (black precipitate)<\/p>\n

S2<\/sub>O3<\/sub>2-<\/sup>(aq) +Pb(NO3<\/sub>)2<\/sub>(aq)<\/span>\u00a0\u2192 \u00a0PbS2<\/sub>O3<\/sub>\u00a0(aq)(white) \u00a0\u00a0\u2192\u0394 \u00a0Ag2S(black)<\/sub><\/p>\n

<\/h4>\n

Test for PO4<\/sub>3-<\/sup><\/h4>\n

\u2022 To a solution of add conc. HNO3<\/sub>, excess of ammonium molybdate and warm. A yellow precipitate will be formed.<\/p>\n","protected":false},"excerpt":{"rendered":"

CHEMICAL TEST FOR TEST METHOD OBSERVATIONS TEST CHEMISTRY Chemical test for Carbonate ion CO32\u2013 or hydrogencarbonate HCO3\u2013 ion Acid is added to the solid carbonate in a test tube. You could also collect a sample of gas from a heated carbonate, i.e. the solid is where the liquid is in the left hand test tube. […]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1662],"tags":[],"class_list":["post-5998","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-06"],"acf":[],"yoast_head":"\nQualitative analysis - Anions - Learning & Education Portal<\/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:\/\/astan.lk\/al_virtualclassroom\/qualitative-analysis-anions\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Qualitative analysis - Anions - Learning & Education Portal\" \/>\n<meta property=\"og:description\" content=\"CHEMICAL TEST FOR TEST METHOD OBSERVATIONS TEST CHEMISTRY Chemical test for Carbonate ion CO32\u2013 or hydrogencarbonate HCO3\u2013 ion Acid is added to the solid carbonate in a test tube. You could also collect a sample of gas from a heated carbonate, i.e. the solid is where the liquid is in the left hand test tube. 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You could also collect a sample of gas from a heated carbonate, i.e. the solid is where the liquid is in the left hand test tube. 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