Experiment no:1 Date:17.09.06Name of the experiment:

Determination of pH of the supplied sample.

Principle: The electrode of pH meter in contact with hydrogen ions of

the sample under test, acquires an electrical potential which depends on the concentration of H+ ions. A measure of the electrical potential is; therefore, give H+ ion concentration or pH of the sample because the negative logarithm of hydrogen concentration is called pH.

pH = -log [H+]

The pH scale value is from 0 to 14. The 7 is neutral; below 7 is acidic and above 7 is basic in nature.

Materials:1. Supplied soil sample2. pH meter3. Beaker4. Buffer solution

Procedure:a. The pH meter was calibrated before use with buffer

solution of known pH values.b. Then the electrode of pH meter was submerged into

the sample that was taken in a beaker and pH of the sample was recorded.

Result:The pH of the sample was 4.4

Name of the experiment:

Determination of total Electrical conductivity (EC) by EC meter.

Principle:Pure water is a very poor conductor of electric current,

whereas water containing dissolved salts ordinarily found in soils conducts current approximately in proportion to the amount of salt present. Based on this principle, electrical conductance, which is reciprocal of resistance, is measured for salinity appraisal. Electrical conductivity, which is commonly represented by the symbol “EC” increase with salt content and therefore, interpretation of reading, is simple. EC is expressed as m mhos/cm, i.e. reciprocal of ohms.

Materials:5. Beaker6. Water sample7. EC meter

Procedure:a. water sample was taken in a beakerb. Then EC reading was taken by a EC meter.

Result:The EC reading of the supplied water sample was 0.6

ms/cm

Exp no: 2 Date: 19.09.06

Name of the experiment : Determination of CO3²‾ and HCO3‾ of the supplied soil sample.The CO3²‾ of the supplied soil sample is absent.Data for HCO3‾

Burette reading of H2SO4

Observation IBR FBR DIFFERENCESAMPLE 3.0 3.2 0.2BLANK 0 0 0

Calculation : Meq/L of HCO3‾ = (z-2y) × normality of H2SO4 × 1000

ml of aliquotHere,

Z= 0.2Y= 0

Normality of H2SO4 = 0.01 NAmount of aliquot taken =5mlMeq/L of HCO3 = (0.2-2×0) × 0.01×1000

5= 0.4

Result:The amount of HCO3ˉ present in the supplied sample was 0.4

meq /L.

Exp no: 3 Date: 19.09.06

Name of the experiment : Determination of chloride in the supplied soil sample.Data:

Burette reading of silver nitrateObservation IBR FBR Difference

Sample 10.4 11.6 1.2Blank 3.2 4.2 1.0

Calculation:Meq/L of Clˉ= (T-B) ×N ×1000

ml of aliquot taken

= (1.2-1) × 0.005 ×10005

= 0.2

Result:The amount of chloride present in the supplied soil sample was

0.2 meq/L.

Exp no: 4 Date: 19.09.06

Name of the experiment : Determination of water soluble calcium of the supplied sample.

Data:Burette reading of EDTA

Observation IBR FBR DifferenceSample 2.6 3.3 0.7Blank 6.6 6.7 0.1

Calculation:Meq/L of Ca = (ml of versenate solution used × normality of

versenate solution ×1000)/(ml of aliquot taken)Here, ml of versenate solution used = (T-B)

= (0.7-0.1) ml = 0.6 ml

Normality of versanate solution = 0.01ml of aliquot taken = mlSo, meq/L Ca = 0.06×0.01×1000

5= 1.2

Result:The amount of water soluble calcium present in supplied sample was

1.2 meq/L.

Exp no: 5 Date: 19.09.06

Name of the experiment : Determination of water soluble magnesium present in the supplied soil sample.

Data:Burette reading of EDTA

Observation IBR FBR DifferenceSample 3.8 4.6 0.8Blank 22.1 22.2 0.1

Calculation:Meq/L of (Mg+Ca) = (ml of versenate solution used ×

normality of versenate solution ×1000)/(ml of aliquot taken)Here, ml of versenate solution used = (T-B)

= (0.8-0.1) ml = 0.7 ml

Normality of versanate solution = 0.01Nml of aliquot taken =5 mlSo, meq/L (Ca+Mg) = 0.7×0.01×1000

5 = 1.4

So, meq/L mg = meq/L of (Ca+Mg) – meq/L of Ca = 1.4-1.2 = 0.2

Result:The amount of Mg present in the supplied sample as water soluble

was 0.2 meq/L.

Exp no: 6 Date: 20.09.06

Name of the experiment : Determination of exchangeable calcium present in supplied sample.

Data:Burette reading of EDTA

Observation IBR FBR DifferenceSample 0.4 1.8 1.4Blank 31.9 32.1 0.2

Calculation:Meq/L of Ca = (ml of versenate solution used × normality of

versenate solution ×1000)/(ml of aliquot taken)Here, ml of versenate solution used = (T-B)

= (1.4-0.2) ml = 1.2 ml

Normality of versanate solution = 0.01ml of aliquot taken =5 mlSo, meq/L Ca = 1.2×0.01×1000

5= 2.4

Result:The amount of exchangeable calcium present in supplied soil sample

was 2.4 meq/L.

Exp no: 7 Date: 24.09.06

Name of the experiment : Determination of exchangeable magnesium present in supplied soil sample.

Data:Burette reading of EDTA

Observation IBR FBR DifferenceSample 1.2 2.9 1.7Blank 47.5 47.7 0.2

Calculation:Meq/L of (Mg+Ca) = (ml of versenate solution used ×

normality of versenate solution ×1000)/(ml of aliquot taken)Here, ml of versenate solution used = (T-B)

= (1.7-0.2) ml = 1.5 ml

Normality of versanate solution = 0.01Nml of aliquot taken =5 mlSo, meq/L Ca = 1.5×0.01×1000

5= 3

So, meq/L of Mg= meq/L of (Ca+Mg)- meq/L of Ca = (3-2.4) = 0.6

Result:The amount of exchangeable magnesium present in supplied soil

sample was 0.6 meq/L.

Exp no: 8 Date: 20.09.06

Name of the experiment : Determination of exchangeable Potassium (K) present in supplied sample by flame photometry method.

Data & calculation:Reading =3.3ppm

Factor from standard curve=1Dilution factor= 10

ppm K in soil = Reading × factor from standard curve × dilution factor = 3.3×1×10

= 33 ppmK, meq/100 gm = ppm

390

= 33 390

= 0.0846

Result:The amount of exchangeable Potassium (K) present in supplied soil

sample 0.0846 meq/100gm.

Exp no: 9 Date: 20.09.06

Name of the experiment : Determination of exchangeable Sodium (Na) present in supplied sample by flame photometry method.

Data & calculation:Reading =14.5

Factor from standard curve=1Dilution factor= 10

ppm K in soil = Reading × factor from standard curve × dilution factor = 14.5×1×10

= 145 ppmNa, meq/100 gm = ppm

230

= 145 230

= 0.6304

Result:The amount of exchangeable Sodium (Na) present in supplied soil

sample 0.6304 meq/100gm.

Exp no: 10 Date: 20.09.06

Name of the experiment : Determination of water soluble Sodium (Na) present in supplied sample by flame photometry method.

Data & calculation:Reading =5ppm

Factor from standard curve=1Dilution factor= 10

ppm K in soil = Reading × factor from standard curve × dilution factor = 5×1×10

= 50 ppmK, meq/100 gm = ppm

230

= 50 230

= 0.2174 meq/100 gm soil

Result:The amount of water soluble Sodium (Na) present in supplied soil

sample 0.2174 meq/100gm soil.

Exp no: 11 Date: 20.09.06

Name of the experiment : Determination of water soluble Potassium (K) presents in supplied sample by flame photometry method.

Data & calculation:Reading =0.9ppm

Factor from standard curve=1Dilution factor= 10

ppm K in soil = Reading × factor from standard curve × dilution factor = 0.9×1×10

= 9 ppmK, meq/100 gm = ppm

390

= 09 390

= 0.02307

Result:The amount of water soluble Potassium (K) present in supplied soil

sample 0.2307 meq/100gm.