Download Exp. 4: Measurement of Hardness of water

Exp. 4: Measurement of Hardness of water
Theory:
The hardness of water is mainly due to the presence of carbonates, bi-carbonates, chlorides and
sulphates of calcium and magnesium in dissolved form. These salts cause excessive consumption of
soap used for cleaning purpose.
The formation of solid calcium carbonate is an endothermic process. Thus, when water containing
both carbonate and calcium ions is heated, calcium carbonate can precipitate out onto the walls of
pipes, boilers, and household items such as tea pots. This can shorten the life-time of some of these
items.
The World Health Organization (WHO) says that "there does not appear to be any convincing
evidence that water hardness causes adverse health effects in humans.
Total Hardness is composed of two components, temporary and permanent hardness.
The temporary hardness is due to the presence of carbonates and bi-carbonates of calcium and
magnesium. It can be easily removed by boiling the water or by adding lime to water.
Both calcium bi-carbonate and magnesium bi-carbonate decompose when heated. The original
insoluble carbonate is reformed. This happens when water is boiled. The precipitation reactions are
as follows:
As you can see boiling the water causes the precipitation of solid calcium carbonate or solid
magnesium carbonate. This removes the calcium ions or magnesium ions from the water, and so
removes the hardness. Therefore, hardness due to bi- carbonates is said to be temporary.
The permanent hardness i.e non-carbonate hardness is due to presence of sulphates, chlorides and
nitrates of calcium and magnesium. It requires special methods of water softening.
Hardness is expressed in part per million as calcium carbonate or commonly known as ppm as
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calcium carbonate.
Environmental Measurements Laboratory | Islamic University of Gaza
Exp. 4: Measurement of Hardness of water
Hard water classification:
Description
Hardness rang ( mg/l as CaCO3 )
o Soft water
Water with hardness up to 50 ppm
o Medium
50 to 150 ppm
o Moderately hard water
150 to 300 ppm
o Hard water
If the hardness is more than 300 ppm
Total hardness is commonly found by determining the amount of calcium and magnesium by a
gravimetric analysis and by calculating their equivalent values in terms of CaCO3.
The most common testing method for hardness is the EDTA titrimetric method.
Disodium ethylenediamine tetra acetate (Na2EDTA) forms stable complex ions with Ca+2, Mg+2, and
other divalent cations causing hardness, and remove them from solution. When a small amount of
Erichrome black T dye is added to the water containing hardness ions at pH 10, the solution becomes
wine red and if there is no hardness the colour is blue. With the addition of EDTA the water sample
having indicator dye starts forming stable complexes until all ions have been removed from solution
and the water colour changes from wine red to blue indicating the end point.
Ca+2 + Mg+2 + EDAT
Wine red colour
PH=10
Ca.EDAT +Mg.EDATA
Blue Colour
Calcium hardness can be determined by increasing the pH value of water to 12, at which magnesium
ions get precipitated and EDTA forms stable complex while reacting with calcium ions, resulting in
change of colour from pink to purple when murexide is used as an indicator.
Apparatus
o Burette.
o Two Conical flasks
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o Pipette
o Graduated cylinder
o Funnel
Environmental Measurements Laboratory | Islamic University of Gaza
Exp. 4: Measurement of Hardness of water
o Beaker
o Hot plate stirrer
Reagents
1) Erichrome Black-T indicator.
a. Dissolve 0.2 gram of the dyestuff in 15 ml of Triethanolamine and 5 ml ethanol or
dissolve 0.5 gm dyestuff in 100 ml of rectified spirit.
b. Its chemical formula can be written as HOC10H6N=NC10H4(OH)(NO2)SO3Na.
2) Ammonia buffer.
a. Dissolve 16.9 gram of Ammonium Chloride (NH4Cl) in 143 ml of concentrated
ammonium hydroxide (NH4OH). Add 1.25 gram of magnesium salt of EDTA to
obtain sharp change in colour of indicator and dilute to 250 ml with distilled water.
One or two ml of this solution is required for raising the pH value of sample to 10.
3) Standard Ethylene diamine tetra acetic acid (E.D.T.A.)solution 0.01M.
Dissolve 3.723 gram EDTA sodium salt and dilute to 1000 ml.
Procedure:
(A) Total Hardness
1. Pipette 25-ml of the tap water sample into a a conical flask (Erlenmeyer flask).
2. Add at least one ml of Ammonia buffer solution. The pH should be 10. To check pH,
standardize pH meter.
3. Place the magnetic stirrer in the beaker and turn on the stirrer slowly.
4. Add a few drops Eriochrome Black T indicator to the Erlenmeyer.
5. Fill the burette with standardized EDTA. Record the initial burette reading.
6. Immediately begin to titrate the sample two drops at a time. Be careful to titrate slowly near
the endpoint, as the color will take about 5 seconds to develop. Thus, add the last few drops
at 3-5 second intervals. The endpoint color is blue.
7. Record the initial and final burette reading to the nearest 0.1 ml.
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Environmental Measurements Laboratory | Islamic University of Gaza
Exp. 4: Measurement of Hardness of water
(B) Calcium Hardness
1. Pipette 30-ml of the tap water sample into a a conical flask (Erlenmeyer flask).
2. Add at least one ml of NaOH solution. The pH should be 12. To check pH, standardize pH
meter.
3. Place the magnetic stirrer in the beaker and turn on the stirrer slowly.
4. Add a few drops a pinch of murexide indicator to the Erlenmeyer.
5. Fill the burette with standardized EDTA. Record the initial burette reading.
6. Immediately begin to titrate the sample two drops at a time. Be careful to titrate slowly near
the endpoint, as the color will take about 5 seconds to develop. Thus, add the last few drops
at 3-5 second intervals. The endpoint color is blue.
7. Record the initial and final burette reading to the nearest 0.1 ml.
Calculations
Total Hardness ( mg/L) as CaCO3 =
𝑉𝐸𝐷𝑇𝐴 × 1000
𝑉𝑠𝑎𝑚𝑝𝑙𝑒
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Environmental Measurements Laboratory | Islamic University of Gaza