Editing Qualitative inorganic analysis

{{short description|Analytical method used to investigate elemental composition of inorganic compounds}}
Classical '''qualitative inorganic analysis''' is a method of [[analytical chemistry]] which seeks to find the [[chemical element|elemental]] composition of [[inorganic compound]]s. It is mainly focused on detecting [[ion]]s in an [[water|aqueous]] [[Solution (chemistry)|solution]], therefore materials in other forms may need to be brought to this state before using standard methods. The solution is then treated with various [[reagent]]s to test for [[chemical reaction|reactions]] characteristic of certain ions, which may cause color change, [[precipitation (chemistry)|precipitation]] and other visible changes.<ref name=King>{{cite book|first1=Edward J.|last1=King|first2=Larkin H.|last2=Farinholt|url=https://books.google.com/books?id=zikLAAAAIAAJ|title=Qualitative Analysis and Electrolytic Solutions|year=1959|publisher=Harcourt, Brace|oclc=594863676|location=New York}}</ref><ref>{{cite book|last1=Vogel|first1=A. I.|last2=Svehla|first2=G.|url=https://books.google.com/books?id=MpPenWMDPd0C|title=Vogel's Qualitative Inorganic Analysis|date=1996|publisher=Longman|location=Harlow, England (1996); New Delhi, India (2008)|isbn=9788177582321|oclc=792729931}}</ref>

Qualitative inorganic analysis is that branch or method of analytical chemistry which seeks to establish the elemental composition of inorganic compounds through various reagents.

==Physical appearance of some inorganic compounds==
{| class="wikitable" border="1"
|-
!

! Salt
! Colour
|-
| 1
| [[MnO]], [[MnO2|MnO<sub>2</sub>]], [[FeO]], [[CuO]], [[Co3O4|Co<sub>3</sub>O<sub>4</sub>]], [[Ni2O3|Ni<sub>2</sub>O<sub>3</sub>]]; [[sulfide]]s of [[Silver|Ag]]<sup>+</sup>, [[Copper(I)|Cu]]<sup>+</sup>, [[Copper(II)|Cu<sup>2+</sup>]], [[Nickel|Ni]]<sup>2+</sup>, [[Iron(II)|Fe]]<sup>2+</sup>, [[Cobalt|Co]]<sup>2+</sup>, [[Lead|Pb]]<sup>2+</sup>, [[Mercury (element)|Hg<sup>2+</sup>]], [[Bismuth|Bi<sup>3+</sup>]], [[Mercury (element)|Hg]], [[BiI3|BiI<sub>3</sub>]], [[Bismuth|Bi]](s), [[Copper(II) thiocyanate|Cu(SCN)<sub>2</sub>]], [[Antimony|Sb]](s), [[Hg2O|Hg<sub>2</sub>O]](s), Cu[C(=NH)S]<sub>2</sub>(s)
| Black
|-
| 2
| Hydrated Cu<sup>2+</sup> salts, Co[Hg(SCN)<sub>4</sub>](s), 
| Blue
|-
| 3
| [[HgO]], [[HgI2|HgI<sub>2</sub>]], [[Pb3O4|Pb<sub>3</sub>O<sub>4</sub>]], Hg<sub>2</sub>CrO<sub>4</sub>(s), Ag<sub>2</sub>CrO<sub>4</sub>(s), 
| Red
|-
| 4
| [[Chromium|Cr]]<sup>3+</sup>, Ni<sup>2+</sup>, hydrated Fe<sup>2+</sup> salts, Hg<sub>2</sub>I<sub>2</sub>(s), Cu(C<sub>7</sub>H<sub>6</sub>O<sub>2</sub>N)<sub>2</sub>(s), CuH[[Arsenic|As]]O<sub>3</sub>(s), 
| Green
|-
| 5
| Hydrated [[Manganese|Mn]]<sup>2+</sup> salts
| Light Pink 
|-
| 6
| KO<sub>2</sub>, [[Potassium dichromate|K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>]], Sb<sub>2</sub>S<sub>3</sub>, [[Ferrocyanide]], [[HgO]], Sb<sub>2</sub>S<sub>3</sub>(s), Sb<sub>2</sub>S<sub>5</sub>(s)
| Orange
|-
| 7
| Hydrated Co<sup>2+</sup> salts
| Reddish Pink
|-
| 8
| [[Chromates]], AgBr, As<sub>2</sub>S<sub>3</sub>, AgI, [[Lead|Pb]]I<sub>2</sub>, [[Cadmium|Cd]]S, PbCrO<sub>4</sub>(s), Hg<sub>2</sub>CO<sub>3</sub>(s), Ag<sub>3</sub>PO<sub>4</sub>(s), Bi(C<sub>6</sub>H<sub>3</sub>O<sub>3</sub>)(s), Cu(CN)<sub>2</sub>(s), Ag<sub>3</sub>AsO<sub>3</sub>(s), (NH<sub>3</sub>)<sub>3</sub>[As([[Molybdenum|Mo]]<sub>3</sub>O<sub>10</sub>)<sub>4</sub>](s), [SbI<sub>6</sub>]<sup>3-</sup>(aq), 
| Yellow
|-
| 9
| CdO, Fe<sub>2</sub>O<sub>3</sub>, PbO<sub>2</sub>, CuCrO<sub>4</sub>, Ag<sub>2</sub>O(s), Ag<sub>3</sub>AsO<sub>4</sub>(s), 
| Brown
|-
| 10
| PbCl<sub>2</sub>(s), Pb(OH)<sub>2</sub>(s), PbSO<sub>4</sub>(s), PbSO<sub>3</sub>(s), Pb<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub>(s), Pb(CN)<sub>2</sub>(s), Hg<sub>2</sub>Cl<sub>2</sub>(s), Hg<sub>2</sub>HPO<sub>4</sub>(s), Al(OH)<sub>3</sub>(s), AgCl(s), AgCN(s), Ag<sub>2</sub>CO<sub>3</sub>(s), Bi(OH)<sub>2</sub>NO<sub>3</sub>(s), Bi(OH)<sub>3</sub>(s), CuI(s), Cd(OH)<sub>2</sub>(s), Cd(CN)<sub>2</sub>(s), MgNH<sub>4</sub>Also<sub>4</sub>(s), SbO.Cl(s), Sb<sub>2</sub>O<sub>3</sub>(s), 
| White
|}

== Detecting cations ==
According to their properties, [[cation]]s are usually classified into six groups.<ref name=King />  Each group has a common reagent which can be used to separate them from the [[Solution (chemistry)|solution]]. To obtain meaningful results, the separation must be done in the sequence specified below, as some ions of an earlier group may also react with the reagent of a later group, causing ambiguity as to which ions are present. This happens because cationic analysis is based on the [[solubility product]]s of the ions. As the cation gains its optimum concentration needed for precipitation it precipitates and hence allowing us to detect it.  The division and precise details of separating into groups vary slightly from one source to another; given below is one of the commonly used schemes.

=== 1st analytical group of cations ===
The ''1st analytical group of cations'' consists of ions which form insoluble [[chloride]]s. As such, the group reagent to separate them is [[hydrochloric acid]], usually used at a [[concentration]] of 1&ndash;2 [[molar solution|M]]. Concentrated HCl must not be used, because it forms a [[Solubility|soluble]] complex ([PbCl<sub>4</sub>]<sup>2−</sup>) with [[lead|Pb<sup>2+</sup>]]. Consequently, the [[lead|Pb<sup>2+</sup>]] ion would go undetected.

The most important cations in the 1st group are [[silver|Ag<sup>+</sup>]], [[Mercury (element)|Hg{{su|b=2|p=2+}}]], and [[lead|Pb<sup>2+</sup>]].  The chlorides of these [[Chemical element|elements]] cannot be distinguished from each other by their colour - they are all white solid compounds. PbCl<sub>2</sub> is soluble in hot water, and can therefore be differentiated easily.  Ammonia is used as a reagent to distinguish between the other two.  While AgCl dissolves in ammonia (due to the formation of the complex ion [Ag(NH<sub>3</sub>)<sub>2</sub>]<sup>+</sup>), Hg<sub>2</sub>Cl<sub>2</sub> gives a black precipitate consisting of a mixture of chloro-mercuric amide and elemental mercury. Furthermore, AgCl is reduced to silver under light, which gives samples a violet colour.

The silver ammonia complex can react with [[bismuth]] ions and [[iodide]] to generate orange or brown [[Ag2BiI5|Ag<sub>2</sub>BiI<sub>5</sub>]] precipitate.<ref name=":0">{{Cite book |last=李 |first=颖 |title=分析化学实验 |year=2021 |isbn=978-7-04-056004-6 |edition=6th |trans-title=Analytical Chemistry Experiments}}</ref>

PbCl<sub>2</sub> is far more soluble than the chlorides of the other two ions, especially in hot water. Therefore, HCl in concentrations which completely precipitate Hg{{su|b=2|p=2+}} and Ag<sup>+</sup> may not be sufficient to do the same to Pb<sup>2+</sup>. Higher concentrations of Cl<sup>&minus;</sup> cannot be used for the before mentioned reasons. Thus, a filtrate obtained after first group analysis of Pb<sup>2+</sup> contains an appreciable concentration of this cation, enough to give the test of the second group, viz. formation of an insoluble sulfide. For this reason, Pb<sup>2+</sup> is usually also included in the 2nd analytical group.

A signature reaction of lead ions involve the formation of a yellow [[Lead(II) chromate|lead chromate]] precipitate upon treatment with [[Chromate and dichromate|chromate]] ions. This precipitate doesn't dissolve in [[ammonia]] (unlike Cu(II) and Ag(I)) or [[acetic acid]] (unlike Cu(II) and Hg(II)).<ref name=":0" />

This group can be determined by adding the salt in water and then adding dilute hydrochloric acid. A white precipitate is formed, to which ammonia is then added. If the precipitate is insoluble, then Pb<sup>2+</sup> is present; if the precipitate is soluble, then Ag<sup>+</sup> is present, and if the white precipitate turns black, then Hg{{su|b=2|p=2+}} is present.

Hg{{su|b=2|p=2+}} ions, after oxidation in the presence of chloride ions to HgCl<sub>4</sub><sup>2-</sup>, can form a characteristic orange-red precipitate of [[Cu2HgI4|Cu<sub>2</sub>HgI<sub>4</sub>]] with the addition of [[Copper|Cu<sup>2+</sup>]] and I<sup>−</sup>.<ref name=":0" />

Confirmation test for Pb<sup>2+</sup>: 
:Pb<sup>2+</sup> + 2 KI → PbI<sub>2</sub> + 2 K<sup>+</sup>
:Pb<sup>2+</sup> + K<sub>2</sub>CrO<sub>4</sub> → PbCrO<sub>4</sub> + 2 K<sup>+</sup>

Confirmation test for Ag<sup>+</sup>:
:Ag<sup>+</sup> + KI → AgI +  K<sup>+</sup>
:2Ag<sup>+</sup> + K<sub>2</sub>CrO<sub>4</sub> → Ag<sub>2</sub>CrO<sub>4</sub> + 2 K<sup>+</sup>

Confirmation test for Hg{{Su|p=2+|b=2}}:
:Hg{{su|b=2|p=2+}} + 2 KI → Hg<sub>2</sub>I<sub>2</sub> + 2 K<sup>+</sup>
:2 Hg{{su|b=2|p=2+}} + 2 NaOH → 2 Hg{{su|b=2}}O + 2 Na<sup>+</sup> + H<sub>2</sub>O

=== 2nd analytical group of cations ===

The ''2nd analytical group of cations'' consists of ions which form acid-insoluble [[sulfide]]s. Cations in the 2nd group include: Cd<sup>2+</sup>, [[bismuth|Bi<sup>3+</sup>]], [[copper|Cu<sup>2+</sup>]], [[arsenic|As<sup>3+</sup>]], As<sup>5+</sup>, [[antimony|Sb<sup>3+</sup>]], Sb<sup>5+</sup>, Sn<sup>2+</sup>, Sn<sup>4+</sup> and Hg<sup>2+</sup>. Pb<sup>2+</sup> is usually also included here in addition to the first group. Although these methods refer to solutions that contain sulfide (S<sup>2−</sup>), these solutions actually only contain H<sub>2</sub>S and [[bisulfide]] (HS<sup>−</sup>).  Sulfide (S<sup>2−</sup>) does not exist in appreciable concentrations in water.

The reagent used can be any substance that gives S<sup>2&minus;</sup> ions in such solutions; most commonly used are [[hydrogen sulfide]] (at 0.2-0.3 M), [[thioacetamide]] (at 0.3-0.6 M), addition of hydrogen sulfide can often prove to be a lumbersome process and therefore sodium sulfide can also serve the purpose.  The test with the sulfide ion must be conducted in the presence of dilute HCl.  Its purpose is to keep the sulfide ion concentration at a required minimum, so as to allow the precipitation of 2nd group cations alone. If dilute acid is not used, the early precipitation of 4th group cations (if present in solution) may occur, thus leading to misleading results. Acids beside HCl are rarely used. Sulfuric acid may lead to the precipitation of the 5th group cations, whereas nitric acid oxidises the sulfide ion in the reagent, forming colloidal sulfur.

The precipitates of these cations are almost indistinguishable, except for [[Cadmium sulfide|CdS]], which is yellow. All the precipitates, except for [[Cinnabar|HgS]], are soluble in dilute nitric acid. HgS is soluble only in [[aqua regia]], which can be used to separate it from the rest. The action of ammonia is also useful in differentiating the cations. CuS dissolves in ammonia forming an intense blue solution, whereas CdS dissolves forming a colourless solution. The sulfides of As<sup>3+</sup>, As<sup>5+</sup>, Sb<sup>3+</sup>, Sb<sup>5+</sup>, Sn<sup>2+</sup>, Sn<sup>4+</sup> are soluble in yellow [[ammonium sulfide]], where they form [[polysulfide]] complexes.

This group is determined by adding the salt in water and then adding dilute hydrochloric acid (to make the medium acidic) followed by hydrogen sulfide gas. Usually it is done by passing hydrogen sulfide over the test tube for detection of  1st group cations. If it forms a reddish-brown or black precipitate then Bi<sup>3+</sup>, Cu<sup>2+</sup>, Hg<sup>2+</sup> or Pb<sup>2+</sup> is present. Otherwise, if it forms a yellow precipitate, then Cd<sup>2+</sup> or Sn<sup>4+</sup> is present; or if it forms a brown precipitate, then Sn<sup>2+</sup> must be present; or if a red orange precipitate is formed, then Sb<sup>3+</sup> is present.

:Pb<sup>2+</sup> + K<sub>2</sub>CrO<sub>4</sub> → PbCrO<sub>4</sub> + 2 K<sup>+</sup>

Confirmation test for copper:

:2 Cu<sup>2+</sup> + K<sub>4</sub>[Fe(CN)<sub>6</sub>] + CH<sub>3</sub>COOH → Cu<sub>2</sub>[Fe(CN)<sub>6</sub>] + 4 K<sup>+</sup>
:Cu<sup>2+</sup> + 2 NaOH → Cu(OH)<sub>2</sub> + 2 Na<sup>+</sup>
:Cu(OH)<sub>2</sub> → CuO + H<sub>2</sub>O (endothermic)
:(Another very sensitive test for copper utilizes the fact that Cu<sup>2+</sup> can serve as a catalyst for the oxidation of [[thiosulfate]] ions by [[Ferric|Fe<sup>3+</sup>]] ions. In the absence of Cu<sup>2+</sup>, Fe<sup>3+</sup> can form the purple complex Fe(S<sub>2</sub>O<sub>3</sub>)<sub>2</sub><sup>−</sup> without undergoing [[redox]]. If the added sample contains Cu<sup>2+</sup>, the solution will rapidly discolor.)<ref name=":0" />

Confirmation test for bismuth:

:Bi<sup>3+</sup> + 3 KI (in excess) → BiI<sub>3</sub> + 3 K<sup>+</sup>
:BiI<sub>3</sub> + KI → K[BiI<sub>4</sub>]
:Bi<sup>3+</sup> + H<sub>2</sub>O (in excess) → BiO{{su|p=+}} + 2 H<sup>+</sup>
:(Bismuth ions can form th bright yellow complex Bi([[Thiourea|tu]])<sub>3</sub><sup>3+</sup> in the presence of [[thiourea]] under acidic conditions, which can be precipitated as the orange-red Bi(tu)<sub>3</sub>I<sub>3</sub>•Cu(tu)<sub>3</sub>I in the presence of Cu<sup>2+</sup> and I<sup>−</sup>, and this can also act as a test for bismuth.)<ref name=":0" />

Confirmation test for mercury:

:Hg<sup>2+</sup> + 2 KI (in excess) → HgI<sub>2</sub> + 2 K<sup>+</sup>
:HgI<sub>2</sub> + 2 KI → K<sub>2</sub>[HgI<sub>4</sub>] (red precipitate dissolves)
:2 Hg<sup>2+</sup> + SnCl<sub>2</sub> →  2 Hg + SnCl<sub>4</sub> (white precipitate turns gray)
:(Hg<sup>2+</sup> may otherwise be detected via Cu<sub>2</sub>HgI<sub>4</sub> formation, see Hg<sub>2</sub><sup>2+</sup> in 1st group cations.)<ref name=":0" />

=== 3rd analytical group of cations ===
The ''3rd analytical group of cations'' includes ions which form hydroxides that are insoluble even at low concentrations.

Cations in the 3rd group are, among others: [[iron|Fe<sup>2+</sup>]], Fe<sup>3+</sup>, [[aluminium|Al<sup>3+</sup>]], and [[Chromium|Cr<sup>3+</sup>]].

The group is determined by making a solution of the salt in water and adding [[ammonium chloride]] and ammonium hydroxide. Ammonium chloride is added to ensure low concentration of hydroxide ions.

The formation of a reddish-brown precipitate indicates Fe<sup>3+</sup>; a gelatinous white precipitate indicates [[aluminium|Al<sup>3+</sup>]]; and a green precipitate indicates Cr<sup>3+</sup> or Fe<sup>2+</sup>. These last two are distinguished by adding sodium hydroxide in excess to the green precipitate. If the precipitate dissolves, Cr<sup>3+</sup> is indicated; otherwise, Fe<sup>2+</sup> is present.

=== 4th analytical group of cations ===
The 4th analytical group of cations includes ions that precipitate as sulfides at pH 9. The reagent used is [[ammonium sulfide]] or Na<sub>2</sub>S 0.1 M added to the ammonia/ammonium chloride solution used to detect group 3 cations. 
It includes: [[zinc|Zn<sup>2+</sup>]], [[nickel|Ni<sup>2+</sup>]], [[cobalt|Co<sup>2+</sup>]], and [[manganese|Mn<sup>2+</sup>]]. [[Zinc]] will form a white precipitate, [[nickel]] and [[cobalt]] a black precipitate and [[manganese]] a brick/flesh colored precipitate. [[Dimethylglyoxime]] can be used to confirm nickel presence, while [[ammonium thiocyanate]] in ether will turn blue in the presence of cobalt. This group is sometimes denoted as IIIB since groups III and IV are tested for at the same time, with the addition of sulfide being the only difference.

This includes ions which form sulfides that are insoluble at high concentrations. The reagents used are H<sub>2</sub>S in the presence of NH<sub>4</sub>OH. NH<sub>4</sub>OH is used to increase the concentration of the sulfide ion, by the common ion effect - hydroxide ions from NH<sub>4</sub>OH combine with H<sup>+</sup> ions from H<sub>2</sub>S, which shifts the equilibrium in favor of the ionized form:

:{{chem|H|2|S}} {{eqmR}} 2{{chem|H|+}} + {{chem|S|2-}}

:{{chem|N|H|4|O|H}} {{eqmR}} {{chem|N|H|4|+}} + {{chem|O|H|-}}

:{{chem|O|H-}} + {{chem|H|+}} {{eqmR}} {{chem|H|2|O}}

They contain [[zinc|Zn<sup>2+</sup>]], [[manganese|Mn<sup>2+</sup>]], [[nickel|Ni<sup>2+</sup>]] and [[cobalt|Co<sup>2+</sup>]]

=== 5th analytical group of cations ===
Ions in 5th analytical group of cations form [[carbonate]]s that are insoluble in water. The reagent usually used is [[ammonium carbonate|(NH<sub>4</sub>)<sub>2</sub>CO<sub>3</sub>]] (at around 0.2 M), with a neutral or slightly basic pH. All the cations in the previous groups are separated beforehand, since many of them also form insoluble carbonates.

The most important ions in the 5th group are [[barium|Ba<sup>2+</sup>]], [[calcium|Ca<sup>2+</sup>]], and [[strontium|Sr<sup>2+</sup>]]. After separation, the easiest way to distinguish between these ions is by testing flame colour: barium gives a yellow-green flame, calcium gives brick red, and strontium, crimson red.

=== 6th analytical group of cations ===
Cations which are left after carefully separating previous groups are considered to be in the sixth analytical group. The most important ones are [[magnesium|Mg<sup>2+</sup>]], [[lithium|Li<sup>+</sup>]], [[Sodium|Na<sup>+</sup>]] and [[potassium|K<sup>+</sup>]]. All the ions are distinguished by flame color: lithium gives a red flame, sodium gives bright yellow (even in trace amounts), potassium gives violet, and magnesium, colorless (although magnesium metal burns with a bright white flame). Magnesium can also be distinguished from other cations in this group by adding sodium hydroxide to drive the pH to 11 or higher, which selectively precipitates Mg(OH)<sub>2</sub>.

==Detecting anions==

=== 1st analytical group of anions ===
The ''1st group of anions'' consist of [[Carbonate|CO{{su|b=3|p=2&minus;}}]], [[Bicarbonate|HCO{{su|b=3|p=&minus;}}]], [[Acetate|CH<sub>3</sub>COO<sup>&minus;</sup>]], [[Sulfide|S<sup>2&minus;</sup>]], [[Sulfite|SO{{su|b=3|p=2&minus;}}]], [[Thiosulfate|{{chem|S|2|O}}{{su|b=3|p=2&minus;}}]] and [[Nitrite|NO{{su|b=2|p=&minus;}}]]. The reagent for Group 1 anions is dilute hydrochloric acid (HCl) or dilute sulfuric acid (H<sub>2</sub>SO<sub>4</sub>).

* Carbonates give a brisk effervescence with dilute H<sub>2</sub>SO<sub>4</sub> due to the release of CO<sub>2</sub>, a colorless gas which turns [[limewater]] milky due to formation of CaCO<sub>3</sub> ([[carbonatation]]). The milkiness disappears on passing an excess of the gas through the lime water, due to formation of Ca(HCO<sub>3</sub>)<sub>2</sub>.
* Acetates give the vinegar-like smell of CH<sub>3</sub>COOH when treated with dilute H<sub>2</sub>SO<sub>4</sub> and heated. A blood red colouration is produced upon addition of yellow FeCl<sub>3</sub>, due to formation of [[iron(III) acetate]].
* Sulfides give the rotten egg smell of H<sub>2</sub>S when treated with dilute H<sub>2</sub>SO<sub>4</sub>. The presence of sulfide is confirmed by adding [[lead(II) acetate]] paper, which turns black due to the formation of PbS. Sulfides also turn solutions of red [[sodium nitroprusside]] purple.
* Sulfites produce SO<sub>2</sub> gas, which smells of burning sulfur, when treated with dilute acid. They turn acidified K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub> from orange to green.
* Thiosulfates produce SO<sub>2</sub> gas when treated with dilute acid. In addition, they form a cloudy precipitate of [[sulfur]].
* Nitrites give reddish-brown fumes of NO<sub>2</sub> when treated with dilute H<sub>2</sub>SO<sub>4</sub>. These fumes cause a solution of [[potassium iodide]] (KI) and [[starch]] to turn blue.

=== 2nd analytical group of anions ===
The ''2nd group of anions'' consist of [[Chloride|Cl<sup>&minus;</sup>]], [[Bromide|Br<sup>&minus;</sup>]], [[Iodide|I<sup>&minus;</sup>]], [[Nitrate|NO{{su|b=3|p=&minus;}}]] and [[Oxalate|C{{su|b=2}}O{{su|b=4|p=2&minus;}}]]. The group reagent for Group 2 anion is concentrated sulfuric acid (H<sub>2</sub>SO<sub>4</sub>).

After addition of the acid, chlorides, bromides and iodides will form precipitates with [[silver nitrate]]. The precipitates are white, pale yellow, and yellow, respectively. The silver halides formed are completely soluble, partially soluble, or not soluble at all, respectively, in aqueous ammonia solution.

Chlorides are confirmed by the ''[[chromyl chloride]] test''. When the salt is heated with K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub> and concentrated H<sub>2</sub>SO<sub>4</sub>, red vapours of chromyl chloride (CrO<sub>2</sub>Cl<sub>2</sub>) are produced. Passing this gas through a solution of NaOH produces a yellow solution of [[sodium chromate|Na<sub>2</sub>CrO<sub>4</sub>]]. The acidified solution of Na<sub>2</sub>CrO<sub>4</sub> gives a yellow precipitate with the addition of [[lead(II) acetate|(CH<sub>3</sub>COO)<sub>2</sub>Pb]].

Bromides and iodides are confirmed by the ''layer test''. A sodium carbonate extract is made from the solution containing bromide or iodide, and [[chloroform|CHCl<sub>3</sub>]] or [[carbon disulfide|{{chem|CS|2}}]] is added to the solution, which separates into two layers: an orange colour in the {{chem|CHCl|3}} or {{chem|CS|2}} layer indicates the presence of Br<sup>&minus;</sup>, and a violet colour indicates the presence of I<sup>&minus;</sup>.

Nitrates give brown fumes with concentrated H<sub>2</sub>SO<sub>4</sub> due to formation of NO<sub>2</sub>. This is intensified upon adding copper turnings. Nitrate ion is confirmed by adding an aqueous solution of the salt to FeSO<sub>4</sub> and pouring concentrated H<sub>2</sub>SO<sub>4</sub> slowly along the sides of the test tube, which produces a brown ring around the walls of the tube, at the junction of the two liquids caused by the formation of {{chem|Fe(NO)|2+}}.<ref>{{cite book
| title = University Chemistry, Volume 1
| author = C. Parameshwara Murthy
| publisher = New Age International
| year = 2008
| isbn = 978-81-224-0742-6
| page = 133
}}</ref>

Upon treatment with concentrated sulfuric acid, oxalates yield colourless CO<sub>2</sub> and CO gases. These gases burn with a bluish flame and turn lime water milky. Oxalates also decolourise KMnO<sub>4</sub> and give a white precipitate with CaCl<sub>2</sub>.

=== 3rd analytical group of anions ===
The ''3rd group of anions'' consist of [[Sulfates|SO{{su|b=4|p=2&minus;}}]], [[Phosphates|PO{{su|b=4|p=3&minus;}}]] and [[Borates|BO{{su|b=3|p=3&minus;}}]]. They react neither with concentrated nor diluted H<sub>2</sub>SO<sub>4</sub>.

* Sulfates give a white precipitate of BaSO<sub>4</sub> with BaCl<sub>2</sub> which is insoluble in any acid or base.
* Phosphates give a yellow crystalline precipitate upon addition of HNO<sub>3</sub> and [[ammonium heptamolybdate|ammonium molybdate]] and heating the solution.
* Borates give a green flame characteristic of [[triethyl borate|ethyl borate]] when ignited with concentrated H<sub>2</sub>SO<sub>4</sub> and ethanol.

==Modern techniques==
Qualitative inorganic analysis is now used only as a [[pedagogical]] tool. Modern techniques such as [[atomic absorption spectroscopy]] and [[ICP-MS]] are able to quickly detect the presence and concentrations of elements using a very small amount of sample.

==Sodium carbonate test==
{{Unreferenced section|date=May 2022}}
The sodium carbonate test (not to be confused with sodium carbonate extract test) is used to distinguish between some common metal ions, which are precipitated as their respective carbonates. The test can distinguish between copper (Cu), iron (Fe), and calcium (Ca), zinc (Zn) or lead (Pb). Sodium carbonate solution is added to the salt of the metal. A blue precipitate indicates Cu<sup>2+</sup> ion. A dirty green precipitate indicates Fe<sup>2+</sup> ion. A yellow-brown precipitate indicates Fe<sup>3+</sup> ion. A white precipitate indicates Ca<sup>2+</sup>, Zn<sup>2+</sup>, or Pb<sup>2+</sup> ion. The compounds formed are, respectively, [[basic copper carbonate]], [[iron(II) carbonate]], [[iron(III) oxide]], [[calcium carbonate]], [[zinc carbonate]], and [[lead(II) carbonate]]. This test is used to precipitate the ion present as almost all carbonates are insoluble. While this test is useful for telling these cations apart, it fails if other ions are present, because most metal carbonates are insoluble and will precipitate. In addition, calcium, zinc, and lead ions all produce white precipitates with carbonate, making it difficult to distinguish between them. Instead of sodium carbonate, [[sodium hydroxide]] may be added, this gives nearly the same colours, except that lead and zinc hydroxides are soluble in excess alkali, and can hence be distinguished from calcium. See qualitative inorganic analysis for the complete sequence of tests used for qualitative cation analysis.

==See also==
* [[Flame test]]
* [[Bead test]]

==References==
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[[Category:Analytical chemistry]]