1. lab 1
aldehyde and ketone

2. Reaction and characterization for eliphatic aldehyde &ketone
Aldehydes are the first oxidation product of primary alcohol
[O]
1o alcohol aldehyde
H atom of aldehyde in very weakly acidic
ex.
formaldehyde HCOH
acetaldehyde CH3COH
call carbonyl group
Ketones:-
are the first oxidation product of secondary alcohol
2o alcohol ketone
Ex:- acetone
also call carbonyl group

3. Ex:- acetone
also call carbonyl group
test used to distinguish ald. and ketone
Tollen,s test
is used to identify the aldehyde .
tollen,s reagent
1-(( silver nitrate AgNO3 ))
2-sodium hydroxide (( NaOH )) 3-ammonia NH3

4. Silver ammonia complex
Black ppt.
silveroxide
sodium nitrate
silver nitrate sodium hydroxide
Silver ammonia complex
Tollen ,s reagent

5. To prevent the precipitation of insoluble silver oxide (Ag2O) the complex agent NH3 in added
Tollen,s test
Principle
Silver ammonia complex is reduced by aldehyde to metallic silver with a few min .(one min) in alkaline medium because ald. contain H atom in their structure
Aldehyde
Silver mirror
reducing agent oxidizing agent carboxyl group
NO reaction
ketone
ketone absence of H atom

6. procedure
In two clean test tube put
1- 10 drop of tollen reagent
2-then added to the first one 5 drops of acetaldehyde then added to the second one 5 drops of acetone wait 1 min , silver mirror deposited on the side the test tube in aldehyde (because aldehyde contain H atom ) and no reaction in the 2nd tube because ketone is not contain H atom
Fehling test:
Fehling solution consist of :-
1- fehling solution one : CuSO4 cupper sulfate-blue colour
2- fehling solution two : sodium –pottasium tartarate
principle of fehling test
aldehyde act as reducing agent it can reduce the deep blue colour of fehling solution in to red ppt. of cuprous oxide

7. Ald.
Cupric ion
Carboxyl ion
red ppt.. of cuprous oxide
acetone
Cupric ion

8. procedure
in two clean test tube put
drop of fehling
2- 15 drop of fehling
mixed very well
then added to the first one 10 drops acetaldehyde
and to the second 3 drops acetone
mixed very well , then put the tubes in a boiling water bath for 3-5 min, red ppt. appears in the first tube indicate the presence at aldehyde (because it contain H atom ) ,
In the 2nd no change in colour (remain blue colour ) because it contain ketone (absence of H atom )

9. blue colour (no reaction )
Conclusion
Observation
test
Tollen,s test
Silver mirror
aldehyde
acetaldehyde
No reaction
ketone
acetone
Fehling test
Red ppt.
blue colour (no reaction )

10. Analysis of group and test of the ions within the group
lab 2
Analysis of group and test of the ions within the group

11. Analysis of group and test of the ions within the group
Group -1- consist of Ag+, pb+2, Hg+2, these ions are provided as nitrate ( Hg2(NO3)2 , pb(NO3)2 , AgNO3) and precipitated as chloride .
The chloride salt of these ions are insoluble in water but soluble in excess acid
Soluble complex
   
Soluble complex

12. Procedure
In clean centrifuge tube put drops of mixture ( AgNO3 , Hg2(NO3) , PbCl2 ) then added 4 drops of 4M HCl. To ppt. the ions as chloride AgCl , Hg2Cl2 ,PbCl2
Mixed well, then put in centrifuge for 1 min

13.   decantation
Filtrate ppt.
neglected AgCl , Hg2Cl2 , PbCl2 
add 10 drop of D.W
then heat in a boiling
water bath with stirring
about 5 min
centrifuge
Filtrate Pb ppt.
identify the Pb (Ag+1&Hg+2)
add 1 drop of ammonium added 7drops
acetate and 1 drop of K2CrO of NH4OH , mixed very well
yellow ppt. appear indicate the then centrifuge for 1min presence of Pb+2

14. filtrated ppt
Ag black ppt.
to identify Ag indicate the
added 1 drop of phenonaphthalene solution presence Hg2+2
then added (4M)HCl drop by drop until
white ppt. appear indicate the presence for Ag+1

15. Test
Observation
Conclusion
Silver
White ppt.
Indicate the presence of Ag+ ion
Lead
Yellow ppt
Indicate the presence of Pb+2 ion
Mercurous
Black ppt
Indicate the presence of Hg2+2 ion

16. lab 3
Determination of PH

17. Determination of Ph
Determination of pH = means determination the power of H+ in the solution
pH define as = the negative Log of hydrogen ion conc.
pH = - Log(H+)
Table -1-
pH of some fluid .
1- blood plasma = 7.4
2-pancreatic juice = 8
3-gastric juice = 1.2 – 3
4-urine = 5 – 8
5-pepsine = 2
The fluid of all living organism contain conjugated acid or base which act as buffer
In determination of pH we should know the following .
1- indicator .
means an organic dyes which change their colour with change of the pH

18. pH of some indicators pH 1
phenolphthalein
8.8-10 2
Methyl orange 3
Thymol blue. (acid) 4
Thymol blue. (base)
8-8.4 5
Phenol red 6
Bromophenol blue . 7
Bromothymol blue
6-7.6

19. These indicator may be used in the form of solution or paper .
2- universal indicator
It is a suitable mixture of certain selected indicator which cover the whole pH range from ( 0-14) it is used to determin the approximate pH of the solution .
The different between the universal indicator and the indicator
Universal indicator used in unknown solution , indicator used in known solution
We have two type of universal indicator

20. 1-universal indicator paper
2-universal indicator solution
method used for determination for determined pH value .
1-by litmus paper . only for acid solution or basic solution .
2-by universal indicator . ( paper solution )
3-colorimetric method by ( Lovibond method ) .
4-Electro metric method by ( pH – meter )
**By universal indicator paper and solution
procedure ;
1-clean 5 test tube put 10 drops solution 1,2,3,4,5
2-cut small piece of universal indicator paper then put one of solution to the end of the paper and allow to the dry for 1min ,then compare the color on the chart . record the result .
3-add to each tube 1 drop of universal indicator mixed and compare colour with the colour on the chart then record the result .

21. No. of solution
pH univ. (paper colour )
pH univ. solution 1 2 3 4 5

22. ** Electrometric method.
Is the best method for determine pH . It depend upon the tension set between two electrode . positive and negative or depend upon the measurement of electrometric force between H+ and OH- in the solution .
PH meter consist of :-
1-the + ve electrode called (calomel electrode ) is made by .( Hg / HgCl and saturated solution of KCl ) It is called (reference electrode )
2-the –ve electrode is glass electrode . which filled with 0.1 N HCl .
when there two electrode . placed in the solution a different of potential . develops between the solution inside the electrode and that outside. The value depend upon the conc. of H+ outside the electode because the conc. of H+ inside the electrode remane constant

23. lab 4
Titrimetric analysis

24. Titrimetric analysis :
Means to find the quantity of substance by using titration
Titration :
is the process of addition of standard solution of known concentration to another unknown substance until the reaction complete , this can be obtained by using indicator .
Standard solution :
The reagent exact known concentration used in titration
Equivalent point (end point):
the point at which amount of the standard solution equivalent to the substance that react during titration .
Indicator :-
Chemical compound that charge their colour with change the PH
Primary standard solution :-
High purified chemical compound and stable .
Normality :
Is the unit to measure the concentration . Of the solution .

25. No. of equivalent of solute
N = ……(1)
Volume of solution (liter) Or
No. of miliequivalent of dissolved solute
N = …(2)
weight
No. of equivalent = ……(3)
Equivalent wt
weight × 1000
No. of miliequivalent = …..(4)
Molecular wt
Equivalent wt =
No of charge
wt wt × 1000
N = or N =
equivalent × V (liter) equivalent × V (ml)

26. Procedure :
fill the burette with HCl solution.
Measure (5 ml) of unknown solution Na2CO3 . by pipette and put in conical flask.
Add one drop of methyl orange indicator yellow colour appear
Titrate HCl aqunist Na2CO3 by adding drop by drop till the pink colour appear stopped the titration and calculation .

27. Result calculation
Measure the volume of HCl and find the normality of Na2CO3  
N1×V1 = N2×V2
HCl Na2CO3
×read on burette = ? × 5
N2 = (the normality of Na2CO3 )
2-Find the conc. Of the unknown Na2CO3 in gm/1000ml
weight × 1000
N =
equivalent × V (ml)
molecular wt
equivalent wt of Na2CO3 = , = = 53
wt × 1000
53 × 1000
wt = gm