A. TITLE

: Identification Reaction of Cation and Anion

B. PURPOSE:1. To know special reagents for each cation and anion in a group

2. To show identification reaction of cation and anion

3. To write the chemical reaction

C. BASIC THEORY :

CATION

Cation analysis requires a systematic approach. This is generally done in two ways, namely separation and identification. The separation is done by dissolving a group cation out of the solution. Cation group precipitate separated from the solution by centrifuge and the filtrate poured into another test tube. Solution which still contains most of the cation is dissolve once more to form a new group of cations. If the group of cation that is dissolve still contains some cations, so cations are then separated again into smaller groups of cations, and so on so that ultimately exacerbate the specific test for the cation. The type and concentration of the reactants and the pH adjustment is done to separate the cation into several groups.

Qualitative analysis is a method used for identification of ions or compounds in a sample. In many cases, qualitative analysis will also involve the separation of ions or compounds in a mixture. Examples of qualitative tests would include ion precipitation reactions (solubility tests) or chemical reactivity tests. The separation of ions is easily achieved by taking advantage of their solubility properties

Having become familiar with the characteristic reactions of cations, one may be able to identify an unknown material using simple chemical tests and separations. In this process, called inorganic qualitative analysis, one deals with the detection and identification of the elements that are present in a sample of material. Frequently this is accomplished by making an aqueous solution of the sample and then determining which cations and anions are present on the basis of chemical and physical properties.

If a sample contains only a single cation, their identification is a fairly simple and straightforward process, although to distinguish between two cations (or anions) that have similar chemical properties is not easy and in this instance additional confirmatory tests are required. The detection of a particular ion in a sample that contains several ions is somewhat more difficult, because the presence o the other ions may interfere with the test. This problem can be circumvented by precipitating, thereby removing, the disturbing ions from solution prior to testing for the particular ion. The successful analysis of a mixture containing large number of ions centres upon the systematic separation of the ions into groups containing only a few ion. It is much simpler task to work with 2 or 3 ions than with 10 or more. Ultimately, the separation of cations depends upon the difference in their tendencies to form precipitates, or to form complex ions.

One of the best and well known separation scheme, outlined below, was first described by R. Fresenius in 1841, though in the course of time modifications were introduced. In this system cations are classified into five groups on the basis of their behavior against some reagents, called group-reagents. By the systematic use of these reagents one can decide about the presence or absence of groups of cations, and can also separate these groups for further examination. The group reagents used for the classification of most common cations are hydrochloric acid, hydrogen sulfide, ammonium sulfide, and ammonium carbonate. Classification is based on whether a cation reacts with these reagents by the formation of precipitates or not. It can therefore be said that classification of the most common cations is based on the differences of solubility of their chlorides, sulfides, and carbonates. The five groups of cations and the characteristics of these groups are as follows:

Group 1

Cations of this group form precipitates with dilute hydrochloric acid. Ions of this group are lead (II), mercury (I), and silver (I). Rationale: Softest acids react strongly enough with a borderline base to precipitate in acid solution

Group 2

The cations of this group do not react with hydrochloric acid, but form precipitates with hydrogen sulfide in dilute mineral acid medium. Ions of this group are mercury (II), copper (II), bismuth (III), cadmium (II), tin(II), tin(IV), arsenic(III), arsenic(V), antimony(III), and antimony(V). The first four form the sub-group 2/a and the last six the sub-group 2/b. While sulfides of cations in Group 2/a are insoluble in ammonium polysulfide, those of cations in Group 2/b are soluble. Rationale: Soft acids react with a very soft base. Group 3

Cations of this group do not react either with dilute hydrochloric acid, or with hydrogen sulfide in dilute mineral acid medium. However they form precipitates with ammonium sulfide in neutral or ammoniacal medium. Cations of this group are iron (II), iron (III), cobalt (II), nickel (II), manganese (II), chromium (III), aluminum (III), and zinc (II). Rationale (1): ZnS, NiS, FeS as sulfides, i.e. borderline acids bind to a very soft base, when the pH is adjusted so as to weaken the M(OH2)nm+ hydrated cation. Rationale (2): Fe(OH)3, Cr(OH)3, Al(OH)3 precipitate because these are hard acids reacting with the hard base OH-. As acidic cations, they will tend to precipitate when the pH is equal to the pKa. These are all hard cations, and therefore prefer the hard base OH

Group 4

Cations of this group do not react with the reagents of Groups 1, 2, and 3. They form precipitates with ammonium carbonate in the presence of ammonium chloride in neutral medium. Cations of this group are calcium (II), strontium (II), and barium (II). Rationale: These are weakly acidic (Bronsted definition) cations. The carbonates are insoluble because of the favorable lattice energy when the weakly basic carbonate ion reacts with these cations, since the cation and anion are both doubly charged and similar in size.

Group 5

Common cations, which do not react with reagents of the previous groups, form the last group of cations, which includes magnesium(II), lithium(I), sodium(I), potassium(I), and ammonium(I) ions. Rationale: These are weakly acidic (Bronsted definition) cations. The carbonates are insoluble because of the favorable lattice energy when the weakly basic carbonate ion reacts with these cations, since the cation and anion are both doubly charged and similar in size.

ANION :

Qualitative analysis is a method used for identification of ions or compounds in a sample. In many cases, qualitative analysis will also involve the separation of ions or compounds in a mixture. Examples of qualitative tests would include ion precipitation reactions (solubility tests) or chemical reactivity tests. The separation of ions is easily achieved by taking advantage of their solubility properties

To facilitate the analysis process, it is often useful to put ions that react in similar ways and follow similar chemical reaction patterns into groups. For example, it may be useful to group ions based on their solubility properties. Some anions such as halides and sulfates are insoluble in lead containing solutions while remaining soluble in iron or copper containing solutions. Therefore, anions can be roughly classified into groups according to their solubility in a particular solution. The reactions used to form groups of anions are referred to in this lab protocol as classification reactions. The individual anions in each group are then separated and identified using different reactions often referred to as confirmatory reactions.

Having become familiar with the characteristic reactions of anions, one may be able to identify an unknown material using simple chemical tests and separations. In this process, called inorganic qualitative analysis, one deals with the detection and identification of the elements that are present in a sample of material. Frequently this is accomplished by making an aqueous solution of the sample and then determining which anions and anions are present on the basis of chemical and physical properties. If a sample contains only a single anion, their identification is a fairly simple and straightforward process, although to distinguish between two anions that have similar chemical properties is not easy and in this instance additional confirmatory tests are required. The detection of a particular ion in a sample that contains several ions is somewhat more difficult, because the presence o the other ions may interfere with the test. This problem can be circumvented by precipitating, thereby removing, the disturbing ions from solution prior to testing for the particular ion. The successful analysis of a mixture containing large number of ions centres upon the systematic separation of the ions into groups containing only a few ion. It is much simpler task to work with 2 or 3 ions than with 10 or more. Ultimately, the separation of anions depends upon the difference in their tendencies to form precipitates, or to form complex ions.

The methods available for the detection of anions are not as systematic as those which have been described above for cations. No really satisfactory scheme has yet been proposed which permits the separation of the common anions into major groups, and the subsequent unequivocal separation of each group into its independent constituents; however, it is possible to detect anions individually in most cases, after perhaps a 1-2 stage separation. It is advantageous to remove all heavy metals from the sample by extracting the anions through boiling with sodium carbonate solution; heavy metal ions are precipitated out in the form of carbonates, while the anions remain in solution accompanied by sodium ions.

The following scheme of classification of anions has been found to work well in practice; anions are divided into four groups on the basis of their reactions with dilute hydrochloric acid and of the differences of solubility of their barium and silver salts.

The four groups of anions and the characteristics of these groups are as follows:

Group 1

Visible change, gas evolution and/or formation of a precipitate, with dilute hydrochloric acid. Ions of this group are carbonate, silicate, sulfide, sulfite, and thiosulfate.

The first group of anions to be separated will be those that precipitate in the presence of calcium ions, Ca+2. Sulfate ions, SO4-2, and carbonate ions, CO3-2, precipitate, that is they form a solid, when mixed with an aqueous solution containing Ca2+ ions. The net ionic equations representing the reactions occurring are shown below:

Ca+2(aq) + SO4-2(aq) CaSO4(s)

Equation 1

Ca+2(aq) + CO3-2(aq) CaCO3(s)Equation 2

A confirmatory reaction that distinguishes between sulfate ion and carbonate ion utilizes the fact that calcium carbonate will undergo a reaction with a strong acid to form carbon dioxide gas and water while calcium sulfate will not (see equations 3 and 4).

CaCO3(s) + 2H+(aq) Ca+2(aq) + CO2(g) + H2O(l)

Equation 3

CaSO4(s) + H+(aq) No Reaction (precipitate remains) Equation 4

Group 2

The anions of this group do not react with hydrochloric acid, but form precipitates with barium ions in neutral medium. Ions of this group are sulfate, phosfate, fluoride, and borate.

When mixed with dilute sulfuric acid, and heated, the nitrite ion, NO2-, forms red-brown nitrogen dioxide gas and nitrate ion. This is a confirmatory reaction, since only one ion is involved.

2NO2-(aq) NO(aq) + NO3-(aq)

Equation 5

2NO(g) (colorless) + O2(g) 2NO2(g) (red-brown)

Equation 6

Equation 5 is a simplified representation of a multi-step process involving hydrolysis and auto-redox reactions of nitrite ion (that is, NO2- is acting as both the oxidizing agent and the reducing agent).

Note that carbonate ion could also be listed in this group (gas forming anions), since it does produce a gas, carbon dioxide, in its reaction with acid. However, the presence of carbonate ion was be confirmed earlier in Group I.

Group 3Anions of this group do not react either with dilute hydrochloric acid, or with barium ions in neutral medium. However, they form precipitates with silver ions in dilute nitric acid medium. Anions of this group are chloride, bromide, iodide, and thiocyanate.

Precipitation is also the main reaction type in the classification of halides, but with a different precipitating agent than for Group I above. Cl-, Br-, and I- ions, when mixed with an aqueous solution containing Ag+ ion, form precipitates that are insoluble in water. As opposed to other solid silver salts, silver halides are also insoluble in strong acid (nitric acid will be used here). Therefore, once the precipitate is formed, it will not dissolve on addition of acid. The Ag+ ion solution used in this experiment is aqueous silver nitrate solution, the only silver salt that is soluble in water. Net ionic equations:

Ag+(aq) + Cl-(aq) AgCl(s)

Equation 7

Ag+(aq) + Br-(aq) AgBr(s)

Equation 8

Ag+(aq) + I-(aq) AgI(s)

Equation 9

Confirmatory reactions that distinguish between the three halide ions and identify each are based on a redox process. All three halides can act as reducing agents and in the process are oxidized to their diatomic elemental forms. Their relative reducing strength is as follows: I- >Br- > Cl-. When coupled with a strong oxidizing agent such as aqueous Cl2 (chlorine water), bromide and iodide ions will undergo oxidation. If chloride reacts with chlorine it will produce chloride and chlorine. While this may happen, it is easier to say that no reaction occurs

Cl2(aq) (colorless) + Cl- (aq) (colorless) No Reaction Equation 10

Cl2(aq) (colorless) + Br-(aq) (colorless) Br2(aq) (yellow to brown ) + Cl-(aq) (colorless)

Equation 11

Cl2(aq) (colorless) + I- (aq) (colorless) I2(aq) (yellow to brown) + Cl-(aq) (colorless)

Equation 12

If Cl- ion is present in the solution, without any other halide, the chlorine water will remain colorless. Therefore, this test verifies the presence of Cl- ion only if the classification test produced a silver precipitate that did not dissolve in acid. After addition of colorless chlorine water to a colorless solution of either bromide or iodide, the solution will change color to yellow-brown, since elemental iodine and bromine impart such color to water. This test, however, does not distinguish between the two ions. One more step is necessary. It is not a reaction, but a physical process of extraction with hexane of the solution obtained upon addition of chlorine water. A small volume of hexane is added to the yellow-brown halide solution. A pink or purple hexane layer (the top layer) after extraction indicates that the initial solution contained I- ion. A yellow to brown-orange hexane layer indicates that the initial solution contained Br- ion. The actual shade of the hexane layer depends on the concentration of the halogen (a higher concentration of the halogen produces a darker shade).

Group 4

Common anions, which do not react with reagents of the previous groups, form the last group of anions, which includes nitrite, nitrate and chlorate ions.

Nitrate ion does not directly produce any precipitates (remember the solubility rules?) nor does it produce any gaseous products in an acidic environment. However, upon reduction by Fe2+ ion it forms a characteristic brown gas, nitrogen dioxide. As with nitrite, the reaction is considered a confirmatory one. The equations for the reactions involved are as follows:

NO3-(aq) + 4H+(aq) + 3Fe2+(aq) NO(aq) + 3Fe3+(aq) + 2H2O(l) Equation 13

2NO(g) (colorless) + O2(g) 2NO2(g) (red-brown)

Equation 14

A specific test reagent, ideally, possesses a specific reaction with each type of anion. The reagent might react with one anion to provide a distinguishing product, but not with the other anions in the mixture. The color of precipitate formed and the reaction of the precipitate formed with dilute acid or identity of gas liberated gives us definitive proof of the unknown anion in the solution.There are three main solution tests and these are also confirmatory tests for specific anions:Test reagentsSpecific Anions Identified

Silver nitrate solution followed by dilute nitric acidChloride, Cl-Iodide, I-Carbonate, CO32-

Barium nitrate solution followed by dilute nitric acid orBarium chloride solution followed by dilute hydrochloric acid.Sulfate, SO42-Sulfite, SO32-Carbonate, CO32-

Lead(II) nitrate solutionChloride, Cl-Iodide, I-Sulfate, SO42-Carbonate, CO32-

Addition of NaOH, aluminum foil / powder or Devarda's alloy. HeatNitrate, NO3-

The principles that are employed in the identification of cations can also be applied to the analysis of anions. The qualitative detection of anions in a sample depends on the distinctive solubility properties of particular salts of the ions and specific chemical reactions that are (ideally) unique to a particular ion.

D. TOOLS AND MATERIALS:

a. Cation

MaterialsTools

Sample Beaker Glass

AquadesTest Tube

HCl 6 MRack

H2O2 3%Tripot

HCl 2 MBurner

NH4Cl 2 MSpatula

NH4OHKassa

Ammonium OxalateClamp

b. Anion

MaterialsTools

Unknown SolutionTest tube

Na2CO3 concentrateBurner

AgNO3Tripot

Kassa

Clamp

E. PROCEDURE a. General Procedure of Cation

b. Analysis Procedure of Cation Ca2+

Thinned with aquades

Added 5 drops of solution into test tube

Added 5 drops of water

Added 2 drops of HCl 6 M

Stirred

Washed substances that stick on the wall with water

Added 6 drops of H2O2 3%

Added 2 drops of HCl 2 M

Boiled until reach volume 1-2 drops

Cooled dawn

Added 6 drops of HCl 6 M

Evaporated

Added 4 drops of NH4Cl 2 M

Mixed it well

Added 15 drops of NH4OH, drop by drop

Stirred

Added 2 drops of NH4OH

Added 2 drops of Ammonium Oxalate

c. Analysis Procedure of Anion Cl-1. Making Preparation Solution

Heated with Na2CO3 concentrate

2. Proving Theres Cl-

- Added AgNO3

F. EXPERIMENT RESULT

a. Cation Ca2+No.Procedure of ExperimentExperiment

ResultHypothesis / ReactionConclusion

Thinned with aquades

Added 5 drops of solution into test tube

Added 5 drops of water

Added 2 drops of HCl 6 M

Stirred

Washed substances that stick on the wall with water

Added 6 drops of H2O2 3%

Added 2 drops of HCl 2 M

Boiled until reach volume 1-2 drops

Cooled dawn

Added 6 drops of HCl 6 M

Evaporated

Added 4 drops of NH4Cl 2 M

Mixed it well

Added 15 drops of NH4OH, drop by drop

Stirred

Added 2 drops of NH4OH

Added 2 drops of Ammonium OxalateBefore:- Sample: colorless

- Water : colorless

- HCl : colorless

- H2O2 : colorless

- NH4Cl : colorless

- NH4OH : colorless

- Ammonium Oxalate (NH4)2S : yellow

After:

- Sample + aquades: colorless solution (sample solution)

- Sample solution + water: colorless solution

- Sample solution + water + HCl: colorless solution (filtrate for procedure II)

- Filtrate 2 + H2O2: colorless solution

- Filtrate 2 + H2O2 + HCl: colorless solution

- After boiled and cooled dawn and drop HCl and evaporated: colorless solution

First, we made a hypo-thesis that the sample which is given contain of cation Mg2+, Ba2+, and Ca2+. When we add 1-2 drops of ammonium oxalate, it forms white precipitate. Because calcium oxalate (CaC2O4) will be form after adding of ammonium oxalate.

CaCO3(s)+ H2O(l) Ca(OH)2(aq) + CO2(g)Ca(OH)2(aq) + 2HCl(aq) CaCl2(aq)+2H2O

Ca2+ + (COO)22- Ca(COO)2 Ca2+ + C2O4 ( CaC2O4(s)Separation of calcium with other cation based on the solubility of CaC2O4 salt which cant dissolve on the water, hence the other cation is easy to dissolve. If theres white precipitate in calcium, CaC2O4 will be form when adding (NH4)2C2O4. Solution made in base condition to prevent the solubility of oxalate salt.

b. Anion Cl-NoProcedure of ExperimentExperiment ResultHypothesis / ReactionConclusion

.

2. Making Preparation Solution

Proving Theres Cl-

Before:

- Unknown solution: colorless

- Na2CO3 concentrate: colorless

- AgNO3: colorless

After:- Unknown solution + Na2CO3: colorless filtrate and white precipitate

- Supply Solution + AgNO3: White precipitate

Unknown solution +AgNO3: white precipitate

Ag+ + Cl- ( AgCl(white)Na2CO3 + CaCl2 CaCO3 + 2NaClNa2CO3 + 2 AgNO3 2 NaNO3 + Ag2CO3NaCl + AgNO3 AgCl white + NaNO3 AgCl + 2NH3 [Ag(NH3)2]+ + Cl-

There is white precipitate after adding AgNO3 so the anion of Cl- is proven.

G. ANALYSIS AND DISCUSSION ANALYSIS OF CATION

In this experiment, the sample is colorless and the shape is like jelly. sample is dissolved in a test tube by using aquades, this is done to simplify the analysis of anions and cations. Then the samples were dissolved according with the procedures analyzed cation analysis in general. The first sample of 6 M HCl added three drops, precipitate containing group 1, the filtrate containing group 2, 3, 4 or 5 after the H2S gas flowed and added with HCL. Precipitation in the form group 2 and the filtrate containing group 3, 4 or 5. Added (NH4) 2S precipitate containing group 3 and filtrate containing group 4 or 5. Added (NH4)2CO3 precipitate containing group 4 and filtrate containing group 5. First we suppose that the samples containing cations Mg2+, Ba2+ and Ca2+. When the sample solution, added 5 drops of water then there is the compound Ca(OH)2, a solution of white and added 2 drops of HCl solution contained CaCl2 compound, white solution (filtrate to procedure 2)

CaCO3(s) + H2O(l) Ca(OH)2(aq) + CO2(g)Ca(OH)2(aq) + 2 HCl(aq) CaCl2(aq) + 2 H2O

The addition 6 drops of H2O2 in the filtrate group 2 reduce white solution. Similarly, while the addition HCl and boiled and cooled and added with HCl obtain the same results. Then evaporated to obtain a perfect result and produce white solution (filtrate for group 3).

The addition a few drops of NH4Cl and NH4OH in the filtrate group 3 produces white solution containing cations Ca2+ or Ag2+. 2NH4Cl + Ca(OH)2 CaCl2+ H2O + 2NH3After the addition, HH4OH produces white solution but when the the addition ammonium oxalate occur white precipitate because there is precipitate of calcium oxalate compounds. The function of ammonium oxalate for precipitate Ca. Therefore, we conclude that the sample contains cations Ca2+Ca2+ + (COO)22- Ca(COO)2 Ca2+ + C2O4 ( CaC2O4(s)ANALYSIS OF ANION Analyte is colorless and the shape is like jelly. To know there is anion on analyte, the first step that we have done is adding saturated Na2CO3 to the reaction tube which contain of analyte so it formed colorless solution. The purpose of adding Na2CO3 is to dissolve the anion on the analyte , with analyte CaCl2 (Ca is our cation) that have been found so the equation that will be happen is :

Na2CO3 + CaCl2 CaCO3 + 2NaCl

The next step is heating the reaction tube, it purpose to faster the reaction that occur or in other case it can give the activation energy to the solution, so the reaction which didnt take place in the beginning because less of activation energy, through of heating the reaction can be occur.

The third step is separation between precipitate and filtrate, it purpose to remove the other substance which may be react with reagent to be added later. And the fourth steps is adding AgNO3 and filtrate, it purpose to difference between Cl- and Br-.

Na2CO3 + 2 AgNO3 2 NaNO3 + Ag2CO3CO32- ion is precipitated when ionic displacement occurs..

In this experiment Cl- ion would be formed white precipitate and Br- ion would be formed yellow precipitate.NaCl + AgNO3 AgCl white + NaNO3

The last step is dissolve the precipitate into NH3 it purpose to keep the possibility of a substance that formed isnt AgCl, because AgCN has white precipitate too, so that if the substance is reacted with NH3, AgCl will react while AgCN not react, so that when the precipitate dissolved in NH3 it can be concluded that of the analyte anion is Cl-. The reaction is:

AgCl + 2NH3 [Ag(NH3)2]+ + Cl-H. CONCLUSION

Based on experiment that we have done, we can conclude that :1. Cation that contain in our analyte is Ca2+2. Anion that contain in our analyte is Cl- 3. Compound that our observe is CaCl2I. ANSWER AND QUESTION 1. Write the general reaction for each group!Group I : M+ + Cl- ( MCl ( M+ + 2Cl- ( MCl2 (

with M+ = As+ dan Hg22+ ; M2+ = Pb+Group II : M2+ + S2- ( MS (

3M3+ + 2S2- ( M2S3 (

M4+ + 2S2- ( MS2 (

with M2+ = Cu2+, Cd2+, Pb2+ ; M3+ = B3=, As3+, Sb3+ ; M4+ = Sn4+ The color of sediment depends on each cation, ie HgS, Bi2S3, CuS the black, CdS, As2S3, SnS2 yellow, and Sb2S3, Sb2S5 is red. The precipitation carried out in acid solution with the atmosphere (H2S containing dilute HCl).

Group III : M3+ + NH3 + H2O ( M(OH)3(s) +

M2+ + 2OH- ( M(OH)2

with M3+ = Fe3+, Al3+, Cr3+ ; M2+ = Mn2+ Group IIIA : The color of the precipitate depends on the respective cations, namely Fe(OH)3, Al(OH)3, which is white, Cr(OH)3 greenish gray Group IIIB : The color of the precipitate depends on each cation, the NIS, CoS, black, MNS color pink, and white ZnS. The precipitation occurs in

the atmosphere alkaline solution (solution containing H2S, NH3 and NH4Cl)Group IV: M2+ + S2- ( MS (

with M2+ = Zn2+, Co2+, Ni2+ Group V: M2+ + CO32- ( MCO3

With M2+ = Ba2+, Sr2+, Ca2+

In group V, there is no common reagents, so that a special

reaction test used to identify dry ions. Dry test, among

others, test the inflatable tube, staining test, flame test, and so forth2. Why oxidizer used in the analysis of cations in the system H2S is H2O2 or bromine, and instead of HNO3?

Oxidizer used in the analysis of cations in the system H2S is H2O2 or bromine because H2O2 is volatile when added to water in order to get salt deposits of sulfide H2S. And instead of using an oxidizing acid HNO3 because all the salt must be removed so that the sulfite deposits will not be formed, because the H2S gas is passed in the analyte in acidic conditions.3. How do we know that H2S, H2O2, or Br2 is not contained in the solution?

To determine the H2S is not present in the solution, we can boiled to remove the H2S and to know that the H2S was gone, entry the filter paper to the Pbacetate, than clamp the filtrate paper after that directed to the Erlenmeyer mouth, if the filter paper was black it signify that H2S still exist, but if the filtrate paper didnt change into black it signify that the H2S was gone.

To determine H2O2 was not present in the solution, dipped the filter paper into HCl, then faced with the hose holes which are distributed to H2O2. If theres no black spot in the filter paper it show that theres no H2O2. To know Br2 was not present in the solution, through evaporate the solution. Smoke coming out placed on a wet starch paper. If the wet starch paper become reddish-orange, the Br2 is still there, but if the orange, Br2 is not there.4. Why to determine the presence of NH4 + cations should be used its analyte directly?

Because the reagent that we use to analyse the cathion of group I until group IV contain NH4+, for example NH4OH, NH4Cl, etc. So if we use this filtrate the NH4+ exactly present.

5. How is the general reaction to the making of the solution preparation to determine the presence of anion?

Na2CO3 + 2HX 2NaX + H2CO3

6. Precipitation of Sulfide salt on the analysing cations of group II and group IIIB do in the difference condition of solution. Explain?

Because in group II, the precipitation of the salt sulfide reacted under acidic conditions, ie in H2S-containing dilute HCl. This is because the filtrate which used to get the precipitate of salt sulfide from group I filtrate which contaion dilute HCl. In group III B, precipitation of salts sulfide reacted under base condition ie in H2S-containing solution of NH3 and NH4Cl. This is because the filtrate which is used to get the precipitate of salt sulfide from the filtrate of group III A, which still contains NH3 and NH4Cl.

7. Why is the precipitation of group IV must be in the base properties?

The deposition of group IV had under base properties because the ammonium , NH4OH, can prevent the loss of acids which volatile so it will produce carbonate salts derived from a solution of ammonium carbonate.

J. REFERENCE

http://www.inc.bme.hu/en/subjects/inchem/sillabus/129-145.pdf Accessed on Monday, December 2nd 2013 at 15:05

http://classes.uleth.ca/201201/chem20001/6_2012%202000Expt1_Qual1643.pdf Accessed on Monday, December 2nd 2013 at 15:38

http://www2.ucdsb.on.ca/tiss/stretton/chem3/lab_24_intro_qa_theory.html Accessed on Monday, December 2nd 2013 at 16:15

http://chemist-try.blogspot.com/2013/01/analisa-kualitatif-reaksi-identifikasi.html Accessed on Monday, December 2nd 2013 at 17:55

http://www.crescent.edu.sg/crezlab/Webpages/AnionLabManual01.htm Accessed on Monday, December 2nd 2013 at 17:58

http://www.inc.bme.hu/en/subjects/inchem/sillabus/129-145.pdf Accessed on Monday, December 2nd 2013 at 15:05

http://sunny.moorparkcollege.edu/~chemistry/chemistry_1B_labs/experiment_twelve.pdf Accessed on Monday, December 2nd 2013 at 18:01

http://www.slcc-science.org/chem/labs/chem1225/1225experiment07.pdf Accessed on Monday, December 2nd 2013 at 18:15Svela, G. 1985. VOGEL Buku Teks Analisis Anorganik Kualitatif Makro dan Semimakro. Edisi ke 5. Jakarta: PT. Havery Indah.

Achmad, Hiskia. 2012. Kimia Analitik Kualitatif. Bandung:PT. Citra Aditya Bakti. Tim.2013.Panduan Praktikum Kimia Analitik I Dasar-Dasar Kimia Analitik. Surabaya:Jurusan Kimia FMIPA UNESAATTACHMENT

PICTUREEXPLANATION

Unkown solution (clear like gel)

Unknown solution contain cation of Ca (CaC2O4)

Sample of anion solution

White precipitate shown anion of Cl-

Sample

Analyte

Filtrate for Group II

Analyte for Procedure III

White Precipitate

Ca2+ Present

Analyte Contain of Ca2+ or Ag2+

Unknown Solution

Filtrate

Precipitate

Used for next analysis (supply solution)

Preparation Solution

White Precipitate

Cl- exist

Dissolve

-Added NH3

Sample

Analyte

Filtrate for Group II

Analyte for Procedure III

Analyte Contain of Ca2+ or Ag2+

White Precipitate

Ca2+ Present

Preparation Solution

White Precipitate

Cl- exist

Unknown Solution

Filtrate

Precipitate

Used for next analysis (supply solution)

- Heated with Na2CO3 concentrate

-Added NH3

Dissolve

Analysis Cation And Anion 25

_1447520620.unknown