Page 154 - AJWEP-22-6

Yadav, et al.

chloride standard solution. The electrode was cleaned weighing the remaining solid residue. The weight of the
and rinsed with distilled water before and after empty basin (W ) and the final weight after evaporation
1
immersion in the sample. Conductivity readings were (W ) were used to calculate the TDS concentration: 64,71
2
taken once the values stabilized.
Amount of dissolved solids ppm ( W W ) 10
6
1
2
2.3.2.4. Total alkalinity 100
Total alkalinity, indicative of the presence of salts from (IV)
strong bases and weak acids, was determined through
titration. A 100 mL water sample was placed in a conical 2.3.2.7. Free carbon dioxide
flask, and two drops of phenolphthalein indicator were Free carbon dioxide (CO ) was estimated by adding
2
added. If a pink color appeared, it indicated the presence of 5–10 drops of phenolphthalein to a 100 mL water
carbonates, which were titrated with 0.02 N sulfuric acid sample. If the solution did not turn pink, indicating
(H SO ) until the color disappeared. Then, two drops of the presence of free CO , the sample was titrated with
2
4
2
methyl orange indicator were added, and titration continued 0.05N sodium hydroxide (NaOH) until a persistent pink
until the color changed from yellow to red, indicating the color was achieved. The concentration of free CO was
2
presence of HCO . Alkalinity was calculated using the calculated using the following formula: 64,71
−
3
following formulas from Trivedi and Goel. 52,64,71
Volume of NaOH used ×
ANormality of HSO 4 Normality of NaOH 44 1000× ×
×
2
PAasCaCOmgL/ = ×1000×50 (I) Free CO (mg L ) Volume of sample

3 Volume of samplle (V)
BNormality of HSO 2 4 2.3.2.8. Chloride

TAasCaCO mg L 1000 50 (II) Chloride concentration was assessed using the
/
Volume of samplle 3–4 drops of potassium chromate indicator and titrated
3 argentometric method. A 50 mL sample was mixed with
with a standard silver nitrate solution until the yellow
where A = volume of H SO used with phenolphthalein
4
2
only; color changed to red, indicating the formation of silver
B = total volume of H SO used with phenolphthalein chromate. The same procedure was followed for a blank
64,71
4
2
and methyl orange; sample using distilled water.
PA = phenolphthalein alkalinity; and
TA = total alkalinity. 2.3.2.9. Nitrate
Nitrate concentration was measured using a colorimetric
2.3.2.5. TH method. A 10 mL water sample was mixed with 2 mL
TH was measured using direct complexation titration NaOH, followed by the addition of 10 mL H SO and
2
4
with ethylene diamine tetraacetic acid (EDTA), which 0.5 mL brucine solution. The mixture was heated in a
has a high affinity for Ca and magnesium (Mg ) ions. water bath for 20 min, and then cooled. Absorbance
2+
2+
The endpoint of the titration was marked by a color was measured at 410 nm using a spectrophotometer
change from wine red to blue using Eriochrome Black (Spectronic 21; Milton Roy, USA. A standard calibration
−
T indicator, indicating that all Ca and Mg had reacted curve was prepared to quantify NO concentration. 74
2+
2+
3
with EDTA. 64,71
2.3.2.10. Phosphate
Total hardness as CaCO mg /L Phosphate concentration was determined using the

3
Volume of EDT Aused ammonium molybdate–stannous chloride method.
1000 (III) A 50 mL water sample was mixed with 2 mL of
Volume of ssample ammonium molybdate and five drops of stannous
chloride. After 10–15 min, the resulting blue color
2.3.2.6. Total dissolved solids was measured at 690 nm using a spectrophotometer
Total dissolved solids were quantified gravimetrically (Spectronic 21; Milton Roy Company, USA). Distilled
by evaporating a known volume of the water sample and water with the same reagents was used as a blank. 52

Volume 22 Issue 6 (2025) 148 doi: 10.36922/AJWEP025120083