precipitimetry - psau · precipitimetry it is a type of quantitative analysis in which the compound...

Precipitimetry

Dr .Elsadig H.Kh.Adam

Pharmaceutical Analytical Chemistry- Preciptimetry Dr.Elsadig Adam

Precipitimetry

It is a type of quantitative analysis in which the compoundto be analyzed is able to form insoluble product precipitate

(ppt) when treated with certain reagents known as precipitating agents.

The precipitate must be sparingly soluble and formed quickly.

-To understand precipitation reactions, the following topics should be studied:

Solubility product (Ksp).Precipitate formation.Fractional Precipitation.Common ion effect.

Solubility ProductSolubility product (sp) is the product of the molar concentrations of the

ions, each concentration being raised to a power equal to the number of ions derived from the ionization of one molecule of the original substance.

-Examples: AgCl = Ag+ + Cl-

Solubility product constant,Ksp (AgCl ) = [Ag+] [Cl-] Ag2CrO4 = 2Ag+ + CrO4

(Ksp) Ag2CrO4 = [Ag+] 2 [CrO4-2]

-Calculate the Ksp of AgCl if you know that the solubility of it in water is 0.0015 g/l and its M.wt. = 143.5 g/mol

Molar concentration = 0.0015 / 143.5 = 1.05 x 10-5 mol/l

(Ksp) AgCl = [Ag+] [Cl-] = (1.05 x 10-5 ) (1.05 x 10-5 )= 1.1 x 10-10 mol L -1

*ion product is greater than Ksp, thus a precipitate will form

• Calculate the solubility of Ag2CrO4. (Ksp = 2.4 x 10-12 M, M.wt. 331.8 g/ mol).

Ag2CrO4 2Ag+ + CrO42-

• if A is the molar solubility [Ag2CrO4 ]• A 2A + A• Ksp = [2A]2 [A] • Ksp = [2A]2 [A] = 2.4 x 10-12

• = 4A3 = 2.4 x 10-12

• A = = 8.4 x 10-5 mol/L

• The solubility = 8.4 x 10-5 x 331.8 = 0.0279 gm/L

Solubility Product

10x4.2

• Calculate the Ksp of pb3(PO4)2 if you know that the solubility = 0.00014 g/l (M.wt. = 811.7 g/mol)

• Calculate the solubility of AgI (Ksp = 0.9x10-16, M.wt.=235 g/mol).

Solubility Product

Precipitate Formation

The ppt. is formed when the product of ions concentrations exceed the solubility product at given temperature.

-Dissolving the formed ppt.:The ppt. is dissolved by making the product of ions concentration below the solubility product of the precipitate.

Fractional Precipitation-When a precipitating agent is added slowly to a solution containing two ions capable of being precipitated by the agent, the substance with the lower Ksp will precipitate first followed by the one having higher Ksp.Example:Solution of Ba+2 and Sr+2 ions, upon the addition of H2SO4, BaSO4 of (lower Ksp) will precipitate first, then SrSO4 (higher ksp)

Common Ion

When NaCl and KCl are dissolved in the same solution, the Cl− ions are common to both salts. In a system containing NaCl and KCl, the Cl− ions are common ions.

NaCl ⇌ Na+ + Cl−

KCl ⇌ K+ + Cl−

CaCl2 ⇌ Ca2+ + 2Cl−

AlCl3 ⇌ Al3+ + 3Cl−

AgCl ⇌ Ag+ + Cl−

For example, when AgCl is dissolved into a solution already containing NaCl (actually Na+

and Cl− ions), the Cl− ions come from the ionization of both AgCl and NaCl. Thus, [Cl−]differs from [Ag+]. The following examples show how the concentration of the common ion is calculated.

Example 1

What are [Na+], [Cl−], [Ca2+ ], and [H+] in a solution containing 0.10 M each of NaCl, CaCl2, and HCl?

SOLUTIONDue to the conservation of ions, we have

[Na+] = [Ca2+ ] = [H+] = 0.10Mbut

[Cl−] = 0.10 (due to NaCl)+ 0.20(due to CaCl2)+0.10(due to HCl)= 0.40M

How to calculate the common ion

Exercise

Ahmed poured 10.0 mL of 0.10 M NaCl, 10.0 mL of 0.10 M KOH, and 5.0 mL of 0.20 M

HCl solutions together and then he made the total volume to be 100.0 mL. What is [Cl−]

in the final solution?

Common Ion Effect- Common ion has a pronounced effect on the weak electrolytes.

A -Effect on ionization:Ionization of weak electrolyte may be strongly reduced by the presence of a common ion.

-Example:CH3COOH = H+ + CH3COO-

HCl → H+ + Cl-

Ionization of CH3COOH decreases by adding H+ or CH3COO- and the equilibrium shifted to left.

B -Effect on Precipitation:It is clear that the addition of common ion will decrease the solubility of the salt and increase its precipitation.

e.g. Addition of Ag+ or Cl- to a saturated solution of AgClAgCl = Ag+ + Cl-

ppt ions (soluble) -The presence of Ag+ or Cl- in the solution as common ion will shift the reaction to left and accordingly the concentration of ionized part of AgCl decreased.

Detection of End Point in Precipitimetry

I. No indicator method:

A- Disappearance of ppt.

Principle :-

The ppt. formed during titration is redissolved by the titrant.

The end point is detected by disappearance of turbidity.

Example:

Det. of Ag+ by standard CN-

The first drop of addition of st. CN- titrant AgCN is formed.

Precipitation is continued until all Ag+ is ppted. as AgCN.

Adding more CN- will form the soluble argento cyanide complex.

Ag+ + CN - AgCN

AgCN + CN - = [Ag(CN)2] -

The process is continued until all AgCN is dissolved as soluble complex.

The end point is the disappearance of last trace of turbidity.

B- Appearance of ppt. (Liebeg’s method)Principle :-This method depends on formation of complex. The end

point is detected by the appearance of the first turbidity.Example:Det. of CN- by st. Ag+

1) st. Ag+ titrant is added to CN- soln. AgCN ppt.2) The ppt. then redissolve as soluble complex.3) Titration is continued till all CN- form soluble

argentocyanide.AgCN + KCN = K[Ag(CN)2]

4) The first xss. of Ag+ added will form silver argentocyanide.K[Ag(CN)2] + Ag+ = Ag [Ag(CN)2] + K+

Insoluble or 2 AgCN

KCN + AgNO3 AgCN + KNO3

AgCN + KCN = K[Ag(CN)2]--------------------------------------------------------2 KCN + AgNO3 = K[Ag(CN)2]+ KNO3

K[Ag(CN)2 ]+ AgNO3 2 AgCN (indicator reaction) + KNO3

5) The end point is detected by the appearance of the first turbidity.

To make end point more clear we add I- which forms with precipitating agent more insoluble salt. This modification is known as Denige’s Modification.

Add I- in ammoniacal medium to detect the end point as yellow turbidity of AgI because AgI is insoluble in ammonia and has lower Ksp than AgCN i.e. AgI is ppted. at the end point in place of AgCN

Liebeg's Method

II –Using indicator methods:

-Formation of colored ppt.: e.g. Mohr’s method

-Formation of colored soln.: e.g. Volhard's method

-Using Adsorption Indicators.: e.g. Fajan’s method

Pharmaceutical Analytical Chemistry- Preciptimetry - Dr.Elsadig Adam

-It is a direct method used for determination of soluble chloride and bromide salts by

titration with standard solution of AgNO3 , in neutral or slightly alkaline medium at pH 7-9,

using K2CrO4 solution as indicator.

-End point

After complete precipitation of halide with AgNO3, the first excess drop of AgNo3 will

precipitate CrO4-as brick red ppt. of Ag2CrO4

NaCl + AgNO3 → AgCl (ppt.) +NaNO3

K2CrO4 + 2AgNO3 → Ag2CrO4 +NaNO3

brick red ppt

Mohr’s method

Mohr's MethodThe medium must be neutral or slightly alkaline (pH 7-9).

• In acidic medium: formation of soluble acid chromate and dichromate

• 2 CrO42- + 2 H+ 2 HCrO4

- = Cr2O72- + H2O

• In strongly alkaline medium: silver ppted. as its oxide

• 2 Ag+ + 2 OH- 2 AgOH = Ag2O + H2O

• It is not used for I- & CNS- which adsorb CrO42- (no

Ag2CrO4 is formed at E.p.), and yellow colour of AgIrender the end point difficult.

• It is not used for det. of halides in presence of CO32- ,

PO43- & oxalate which are ppted. in neutral medium.

• Titration should be carried out at room temp. because Ag2CrO4 is more soluble in hot water.

Volhard’s methodIt is an indirect method for determination of halides in an

acidic medium (HNO3 ).A known excess of standard AgNO3 solution is added to the

soluble halides, filter and acidify the filtrate with HNO3 .Residual AgNO3 is back titrated with standard SCN- in presence

of (Fe+3) ferric alum as indicator.End point is detected by the appearance of red color of

Fe(SCN)3 or [Fe(SCN)6]-3

NaCl + AgNO3 → AgCl (ppt.) + NaNO3

AgNO3 (xss) + KSCN → AgSCN (ppt.) + KNO3

• At end point : Fe+3 + 6 SCN- → [Fe(SCN)6]-3 (red color)• The method can be used for direct determination of Ag+ by

SCN- and SCN- by Ag+ in an acidic medium.

Volhard's Method The titration must be carried out in acidic medium (HNO3)• (i) the formed ppt. is insoluble in HNO3.• (ii) prevent pptn. of Ag+ and Fe3+ as AgOH or Fe(OH)3 in

alkaline medium.• Filtration is very necessary to prevent attacking the formed

AgCl ppt. by CNS- due to the Ksp of AgCNS (Ksp = 7x10-13) is less than that of AgCl (Ksp = 1.2x10-10). Therefore after the CNS- reacts with all Ag+, it will displace the Cl- from AgCl to form the more insoluble AgCNS.

• AgCl + CNS AgCNS + Cl-

• This problem can also be avoided by adding nitrobenzene which surround the particles of ppt. by a thin film which protect the ppt. from attacking by CNS-

• Volhard method was used for the det. of Ag+ by direct titration with CNS- in the presence of HNO3 using ferric alum as indicator.

Adsorption Indicators(Fajan Method)Fajan in 1889 discovered that, certain dyes change

their color when adsorbed to precipitate. Such compounds are called adsorption indicators.-They are either weak acids e.g. Fluorescein and Eosin or weak bases e.g. Rhodamine 6G-Examples of Adsorption Indicators

-Fluorescein: used for determination of Cl- and Br-, color change form yellowish green to pink.

-Eosin: used for determination of Cl-, Br- and I-, color change form orange red to bluish red.-Rhodamine: used for determination of Ag+, the color change from orange red to violet.

Fajan's MethodIt is a direct method used for determination of

soluble Cl-, Br- , I- and SCN- in neutral medium by titration with standard solution of AgNo3 , in presence of an adsorption indicator as fluorescein.

-The method is used for determination of Br-

and I- in an acidic medium, using eosin as indicator.

-The method is used for determination of Ag+ by titration with standard solution of Br- in an acidic medium using Rhodamine as indicator

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