1. Determination of ksp of slightly soluble salt(CaCO3) before and after the addition of common ion (CaCL2) DONE BY : Hiba Sabah , Zeina Dawood , Sura Zuhair

2. Experimental work
1.Add 0.5 gm of CaCO3 into 5 conical flasks then pour 20ml of different molarities (DW. , 0.02 M CaCL2 , 0.04 M CaCL2 , 0.06M CaCL2 and 0.08M CaCL2) to 1st , 2nd ,3rd .4th and 5th conical flasks respectively 2.Shake for 10 min. ,leave 10 min. for equilibration. 3. filter, take 10ml of the filtrate, titrate against 0.01N NaOH using phenolphthalein indicator and calculate the solubility product of CaCO3. 3.There is 0.1M CaCL2 in the laboratory , prepare the required concentration using dilution method C1*V1=C2*V2

3. 1ST Conical flask ksp=[Ca +2] [CO3 -2]
In other flasks ksp =[CO3 -2] [Ca+2 + Ca+2 from CaCL2]
CaCO Ca CO3 -2
CaCL Ca CL -1
neglected

4. Calculation In titration CO3 -2 +2NaOH Na2CO3 + 2H2O
1 eq.wt of CO * 1eq.wt of NaOH
60 \ L 1N NaOH
30 \1000 * ml N NaOH
ml N NaOH

5. For the 1st conical flask EP1 * 0.0003 = gm \10ml
convert it to mole \ liter = molar conc.of CO3 -2 = molar conc. of Ca+2
Ksp 1st flask = [ CO3-2] [ Ca+2]
Ksp 2nd flask = [CO3-2] [0.02 ]
Ksp 3rd flask =[CO3-2] [ 0.04]
Ksp 4th flask = [ CO3-2] [ 0.06]
Ksp 5th flask = [ CO3-2] [ 0.08]