Nephlo Flame
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Transcript of Nephlo Flame
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Expt.No:
Date:
NEPHELOMETRY
Aim: To determine the turbidity of given solution using Nephelometer.
Theory: Turbidity is an expression of the optical property of a sample
which causes the light to be scattered and absorbed rather than
transmitted in straight line through the sample. Scattering is elastic so
that both incident and scattered light have same wave length. Turbidity is
caused by the presence of suspended matter as a dispersant in the liquid.
The intensity of the perpendicularly polarized
component of scattered light and parallel polarized component of
scattered light are functions of the relative refractive index, the size
parameter, the angle of observation as well as the concentration of
dispersant. Light scattering theory is based on tyndall effect also known
as Rayleigh’s scattering.
Principle: At low concentration of a suspension, there is uniform
scattering. Hence the intensity of scattered light is proportional to the
concentration.
Is α [C]
Apparatus Required: Nephelometer
Instrumentation: The main components of nephelometer are
1. Source of light
2. Filters and monochromators
3. Sample cells
4. Detectors
Nephelometer, consists of tungsten lamp as a source of light
and the sample cell is placed on top of light source passing through the
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filter falls on suspended particles. These particles scattered the light. The
light by the particles are collected by the curve mirrors and reflected to
the photo voltaic cell kept at the bottom of the instrument.
Applications Of Nephelometry: Nephelometer is used
1. Control of potable water
2. Monitoring the quality of raw water & products in food industry
3. Assessing suitability of boiler feed & industrial process water
4. Water pollution analysis
5. Measurement of concentration of sediments in waste water
6. Estimation of transparency of beer, alcoholic beverages, fruit juices
and various products of pharmaceutical and chemical industries.
7. Estimation of concentration of insoluble substance in liquid.
Expt.No:
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Date:
ESTIMATION OF SULPHATE
Aim: To estimate the amount of sulphate present in the given sample by
Nephelometry.
Phenomenon In The Dispersant: The turbidity of a dilute BaSo4
suspension is difficult to produce. So, the velocity of precipitation as well
as the concentration of reactants must be controlled by adding pure
BaCl2. The rate of solution of BaCl2 controls the chloric acid solution in
order to inhibit the growth of micro crystals of BaSo4 .Optimum pH
minimizes the effect of variable amounts of other electrolytes present in
the sample. A glycerol alcohol solution stabilizes the turbidity. The
mixture should be shaken gently in order to obtain the uniform particle
size.
Requirements: Nephelometer, test tubes
Reagents:1. STANDARD SULPHATE SOLUTION: Dissolve 1.814g of dry
potassium sulphate in distilled water dilute to 1 litre in a graduated
volumetric flask. This solution contains 1.000 mg of sulphate ion per ml
that gives 1000 ppm.
2. SODIUM CHLORIDE – HYDROCHLORIC ACID REAGENT:
Dissolve 60 g of sodium chloride in 200 ml of distilled water, add 5 ml of
pure concentrated hydrochloric acid and dilute to 250 ml.
3. SOLID BARIUM CHLORIDE: 0.3g (for each tube)
4. GLYCEROL – ETHANOL SOLUTION: Dissolve 1 volume of pure
glycerol in two volumes of absolute ethanol.
Procedure:
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1. Pipette out 0.5, 1.0, 1.5, 2.0, 2.5 and 3.0 ml of standard potassium
sulphate solution into a series of separate 100ml volumetric flask.
2. Test solution was taken into a separate 100 ml volumetric flask.
3. To each flask 10 ml of sodium chloride – hydrochloric acid reagent and
20 ml of the glycerol – ethanol solution were added and diluted to 100ml
with turbidity free distilled water.
4. 0.3 gm of barium chloride was added to each flask and mixed
thoroughly.
5. Allowed each flask to stand for 2 or 3 min and transfer. The contents of
each numbered test tubes.
6. In a separated flask, blank was prepared by adding 3ml of turbidity free
distilled water and performed the steps 2, 3 and 4. Blank was transferred
into a separate marked test tube.
7. The blank filled test tube was kept on the sample compartment and
calibrated to
zero.8. The blank was replaced with the 0.5ml reference standard solution.
9. The same was repeated for 1.0, 1.5, 2.0, 2.5, 3.0ml and unknown test
tubes and readings were noted.
10. A graph was plotted by taking concentration of standards on x-axis
and turbidity (NTU) on y-axis.
Precautions:1. Solutions should have uniform turbidity size of the particles should be
equal to or greater than the wavelength of the incident light.
2. Wavelength of the incident light should not absorb the light but only
scatter the incident light.
3. Refractive index of the particles and the medium should be
different.K 2So4
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Observations:
S.
No
.
Standar
d K 2So4
solution
(ml)
NaCl-HCl
reagent(ml
)
Glycerol
-ethanol
solution
(ml)
Barium
chloride(g
)
Total
volum
e (ml)
Turbidit
y
1 Blank 10 20 0.3 100
2 0.5 10 20 0.3 1003 1.0 10 20 0.3 100
4 1.5 10 20 0.3 100
5 2.0 10 20 0.3 100
6 2.5 10 20 0.3 100
7 3.0 10 20 0.3 100
8 Test 10 20 0.3 100
Calculation:
Unknown concentration = Unknown samples NTU
Standard NTU (mg/ml) x Standard
concentration
Result: The amount of sulphate present in the given sample was
estimated as………NTU
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Expt.No:
Date:
FLAME PHOTOMETRY
Introduction: Flame photometric analysis method is more or less
similar to that of spectrophotometry, with the exception that a flame is
used instead of sample cell. By this technique, the absorption or emission
of specific wavelengths by excited atoms can be measured.
Flame photometry is of 2 types
1. Emission flame photometry
2. Absorption photometry
Principle: Volatilization of molecules in a flame produces free atoms
and then excites them to higher energy levels. The characteristic emission
spectrum of the element is produced when excited atoms return to their
ground state. This is a principle behind the emission flame photometry.
Since the transitions available to the electrons in any given atom are
specified by the available energy levels. The atomic spectra are specific
for the element involved. Moreover, the energy absorbed or emitted is
proportional to the number of atoms in the given path. Thus, flame
photometry provides us identify and quantify of elements present. The
amount of energy depends on temperature and composition of flame. It is
therefore very necessary that the two flame variables must be kept
constant.
Instrumentation: The basic components are of flame photometry are
1. Nebulizers or atomizers
2. Flame
3. Monochronators
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4. Photo cells
Applications:
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1. Food and agriculture: To determine Ca and K content in soils, plant
material, food and beverages.
2. Medicine: Na, K, Li electrolytes in serum.
3. Mining and metallurgy: Alkali and alkaline earth metals.
Expt.No:
Date:
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ESTIMATION OF SODIUM BY FLAME
PHOTOMETER
Aim: To determine the concentration of sodium by using flame
photometry.
Requirements: 1. Flame photometer
2. Sodium filter
Reagents:
1. Stock Standard Solution: The stock standard solution is weighing
accurately 2.542g of quality sodium chloride and transfers it into a 1 liter
volumetric flask. Add double distilled water to the flask, dissolve the
crystals and make up the solution to the mark with double distilled water.
This stock standard contains 1000 ppm of sodium.
2. Working Standard Solution:
The stock standard solution is successively diluted further with
double distilled water to have working standard solution of lower
concentrations of 20, 40, 60, 80 and 100 ppm of sodium.
Principle:
When sodium solution enters the flame chamber, the solution evaporates
and leaves the residue. The Na ions were excited by the thermal energy of
the flame of higher energy levels. These excited Na ions radiate energy,
which were passed through the specific filter designed for Na. These
radiations were detected by the detector to give the digital display of
concentration.
Procedure:
1. Samples of 0, 20, 40, 60, 80 and 100 ppm and an unknown
concentration were taken in test tubes numbered from 1-6. All the test
tubes were made to equal volumes by adding distilled water.
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2. Various samples including the unknown were fed at the capillary tube
of the flame photometer. The solution was sucked into the chamber.
3. The solvent was evaporated and Na ions were excited to higher energy
state and the radiation was detected by the photocell of the detector.
4. The concentration was displayed on the display.
5. A graph was plotted by taking concentration of samples (in ppm) on x-
axis vs. emitted radiation on y- axis and obtained a straight line.
Result:
Precautions: