salinity report

– this is a report about Sallinty

– there is a file with the result and tables some tables need to be filled. ( Techniques on Salinity tables)

then I want you to put all the tables in Microsoft Word and Include a paragraph on the accuracy of different techniques of salinity baes on the result.

1. Based on your five experimental Techniques on Salinity
2. construct a Table summarising your results.
3. Include a paragraph on the accuracy of different techniques.

Department of
Biological & Environmental Sciences
MARS 101
Introduction to Marine Science
Instructor: Muhammed Nayeem Mullungal
Laboratory Activity #6
Salinity
MARS 101-LAB 6
Fall 2021
Salinity
Measurement of Salinity by Various
Experimental Methods
Equipment or materials required
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Salt
Beakers
Pipette
Petri dish
Graduated cylinder
Deionized water
Thermometer
Dropper
Burette
burette stand
Aluminium dishes
Stirrer
AgNO3 solution (50 gm of AgNO3 dissolved in 1000mL of deionized water)
K2CrO4 solution (3.5gm of K2CrO4 dissolved in1000mL of deionized water)
Salt water hydrometer
Drying oven
Digital Thermometer
Digital Weighing Balance
Introduction
Salinity is a measure of the total dissolved salts in seawater. This sounds simple enough, but
measuring salinity becomes a problem when we realize that some of the salts do not simply
dissociate into ions but chemically react with water to form complex ions, and some of the ions
include dissolved gases such as CO2 (which converts to carbonic acid, H2CO3, bicarbonate,
HCO3-, and carbonate, CO32-).
Salinity can be defined as:
“The total amount in grams of solid material dissolved in 1 kilogram of seawater when all the
carbonate has been converted to oxide, all of the iodine and bromine have been replaced by
chlorine, and all the organic matter has been completely oxidized”, (Duxbury, 1971).
For this laboratory we will use a simpler definition: The total amount of solid materials in grams
dissolved in 1 kg of seawater.
Normally, salinity is expressed in parts per thousand (ppt), often written as º/ºº. It is also sometimes
abbreviated as per mil, much the same as parts per hundred is abbreviated as percent (%). For
example, if you had 1000 g of seawater that contained 35 grams of dissolved salt, you would
have a 3.5% salt solution or a salinity of 35 parts per 1000 (35º/ºº).
MARS 101-LAB 6
Fall 2021
Salinity
In this laboratory our salt water is not seawater, it is a solution of table salt (NaCI) dissolved
in de-ionized water. We only have two elements of the 11 commonly found in seawater (and the
dozens that are present in trace amounts); however, the methodologies we use here will work for
natural seawater as well as for our artificial seawater.
Pre Lab Question 1:
Why is the sea salty? Why it is important?
Measuring Salinity
In this laboratory we present five analytical methods for determining salinity. The components of
salinity vary in their effects on the different measurement hence different measurements will give
different levels of accuracy and precision. Concentrate in your each methodology so as to produce
repeatable results, but do not expect that each technique will produce exactly the same numbers.
Five Methods of salinity determination:
• Evaporation of seawater
• Conductivity of seawater
• Measurement of water density by hydrometer
• Refraction of light through seawater
• Titration of the chloride ion (CI-)
MARS 101-LAB 6
Fall 2021
Salinity
For each method you will be measuring the salinity of Four samples: Three known sample,
whose salinity is 35º/ºº;10 º/ºº and 50 º/ºº and a sample A whose salinities are to be determined
by you.
A. Determination of salinity by evaporation
As we have defined salinity as the total mass of dissolved salts (measured in grams) in one
kilogram of seawater, the most straightforward way to measure salinity is to measure exactly one
kilogram of seawater, evaporate the water, and weight the salt that precipitates out. Evaporating
a full kilogram of water would take more time than we have today however, so we will shorten
the process by evaporating a small fraction of a kilogram.
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Label four Petri dishes/aluminum dishes ( with the same labels as the sample beakers)
and weigh each to the nearest 0.01 gram. Record the masses of the dishes in Table A
on the answer sheet.
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Using a pipette, transfer about 5 mL of each of the two salt solutions to the
corresponding labeled Petri dishes. Weigh each Petri dish with the water to the nearest
0.01 gram and record the masses on the answer sheet. Determine the mass of the water
samples by subtracting the weight of the dish only, and record the masses.
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Carefully bring the Petri dishes to the back of the room, where your instructor will place
them in the drying oven. Leave them in the oven until dry – this will take the majority of
the lab period. You will be doing exercises B through E while waiting for the samples dry.
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Once the samples are dry allow them to cool for a few minutes, then weigh each Petri
dish and record the results on the answer sheet (dish + salt). Subtract the masses of the
dishes to determine the mass of each of the salt samples and record the results on the
answer sheet.
MARS 101-LAB 6
Fall 2021
Salinity
•
Determine the salinity of each sample using equation 1 (below). Record your
answers on the answer sheet.
10 ppt
35 ppt
50 ppt
Unknown
B. Determination of salinity by electrical conductivity
Take a conductivity meter reading of each sample to compare the relative salinity of each sample.
Conductivity is a measure of the ability of water to pass an electrical current and is affected by the
presence of dissolved solids. As the level of the total dissolved solids (TDS) rises, the
conductivity (electrolytic activity) will also increase.
Sea Sickness: If you drink seawater you will become dehydrated. The sodium concentration in sea
water is several times higher than the concentration in blood. The body has to excrete the extra salt in
the urine and more water is required to get rid of the salt than was in the sea water in the first place.
Therefore, you will literally “dry up” drinking sea water as your neuron- muscular reactions become
erratic. Some sea birds, like penguins, sea gulls and albatross, can drink sea water but they have
special glands in their heads to excrete the excess salt.
(NOTE: It is important to dilute the sample using only deionized water, as tap water contains
ions such as sodium and calcium that will alter the salinity of your sample and skew the results of
the experiment).
Conductivity meters can be made to measure a variety of salinity conditions. Unfortunately
MARS 101-LAB 6
Fall 2021
Salinity
devices that can handle the high salt concentrations found in the world’s oceans (and in today’s
lab) are quite costly. The device we will be using today is only accurate at much lower salinities
so we must dilute our samples by a known amount in order to make our measurements.
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Measure the water’s temperature (allow 30-60 seconds for the thermometer to equilibrate)
and record the temperature in Table B on the answer sheet.
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Measure the electrical conductance of the water (the units of conductance are Siemens/cm
– the reciprocal of electrical resistance). Place the meter into the beaker (be sure that
the probe sensors are completely submerged) and allow at least 30 seconds for the readout
to equilibrate. Record the conductance on your answer sheet.
NOTE: The conductivity meter is a valuable instrument – handle it carefully. Have a small
beaker of deionized water at your station and use it to rinse the probe sensors between
measurements.
NOTE: Since we have only included lines for temperatures at 5 degree increments, you will be
expected to interpolate your results. For example: if your water temperature was 17.5°C, use
your measured conductivity and the graph to determine the salinity if the water were 20°C and if
the water were 15°C. As 17.5°C is halfway between 15°C and 20°C, the salinity value is halfway
between the two values you determined for these temperatures.
MARS 101-LAB 6
Fall 2021
Salinity
Multiple
Name
Symbol Multiple
Name
Symbol
0
10
S
siemens
1
10
decasiemens daS
10–1
decisiemens dS
–2
102
hectosiemens hS
10
centisiemens
cS
103
kilosiemens kS
10–3
millisiemens
mS
6
10
megasiemens MS
10–6
microsiemens
µS
109
gigasiemens GS
10–9
nanosiemens
nS
1012
terasiemens TS
10–12
picosiemens
pS
10 ppt
35 ppt
50 ppt
Unknown
MARS 101-LAB 6
Fall 2021
Salinity
Figure 3: Conductivity as a function of salinity and of temperature. Lines show the relationship
between specific conductivity (Y axis) and salinity at 5 degree increments between 15°C and 25°C..
MARS 101-LAB 6
Fall 2021
Salinity
C. Determination of salinity by density using a hydrometer
.Hydrometer are devices designed to measure fluid density. The hydrometer’s mass is
precisely fixed and it is concentrated at the bottom of the tube (like a buoy) so that the
hydrometer will always float upright. The narrow stem is precisely graduated so that as
the device sinks and displaces its own mass, the level to which it sinks is equal to the
seawater density (Figure 4). As density of the seawater increases, the volume of the
displaced seawater decreases (the hydrometer sinks less in the higher density fluid).
Figure 4: Hydrometer function. As the density of the fluid increases, the hydrometer displaces less water. Since the
upper tube is very narrow this difference in volume corresponds to a significant change in depth. The density of the
fluid can be read from the graduations on the stem.
Figure 5 below shows a close-up view of the hydrometer stem: there are labeled divisions
representing 5/1000 gram/mL (1.010, 1.015, and so on); these are divided into five parts (1/1000
g/mL) by secondary unlabeled divisions; these are divided into halves
g/mL) by tertiary unlabeled divisions. If you are careful using this device you can
determine density to a precision of 5 parts in 10,000 (1/2 milligram/mL).
MARS 101-LAB 6
Fall 2021
Salinity
Figure 5 : Reading density from the hydrometer. The major lines are labeled to 5 parts in 1000, the secondary
unlabeled lines to 1 part in 1000, and the tertiary unlabeled lines to 5 parts in
10,000. This device can be read to the fourth decimal place.
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. Pour approximately 220-240 mL of water from the known (35o/oo) salinity sample
into a 250 mL graduated cylinder.
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. Measure and record the water temperature in Table C on the answer sheet.
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Carefully lower (do not drop) the hydrometer in the graduated cylinder until it floats.
If there is not enough water to allow the hydrometer to float, more water can be added until
the hydrometer rises from the bottom.
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. Read the density of the water from the graduated lines on the hydrometer and
record this value in Table C.
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Rinse and dry the hydrometer and the graduated cylinder with deionized water.
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. Repeat steps 1-5 for the other samples , recording the temperatures and the density
values in Table C.
Figure 6 (below) is a graph relating water density (vertical axis) to salinity (horizontal axis). It
can be read like Figure Three, as it has lines representing the density-salinity relationship at
several fixed temperatures. Determine the salinity of your sample by finding the salinity that
crosses the lines representing your measured density and temperature. As before you may need
to interpolate between the temperature lines. Record your salinity values in the appropriate
space on Table C.
MARS 101-LAB 6
Fall 2021
Salinity
Figure 6: Density as a function of salinity and of temperature. Lines show the relationship between
density and salinity at 5 degree increments between 15°C and 30°C.
10 ppt
35 ppt
50 ppt
Unknown
MARS 101-LAB 6
Fall 2021
Salinity
D. Determination of salinity by refractometer
A refractometer can precisely measure the amount of refraction that is caused by the density.
The instrument that you will be using is temperature compensated. This means that the
temperature effects on refraction can be ignored for these measurements, and you will be able
to read the salinity directly from the refractometer.
The refractometer consists of a blue-tinted glass prism and a beveled, clear plastic cover lens,
each with a known refractive index. When a thin layer of water is placed between these two
lenses it will refract light through an angle that depends upon the salinity of the water sample.
When you look through the eyepiece you will see a calibrated scale with an upper blue- shaded
region and a lower white region. The boundary between these two regions will cross the scale
at a value representing the sample’s salinity (Figure 7).
Figure 7: The refractometer. Place a drop of the water sample between the two lenses and lower
the upper lens into place. Look through the eyepiece and aim the refractometer toward a light
source. The boundary between the upper blue-shaded region of the scale and the lower white
region crosses the calibration scale at a value that represents the salinity of the sample.
MARS 101-LAB 6
Fall 2021
Salinity
Before you begin, carefully rinse the face of the prism and the cover lens of the refractometer
with deionized water, and dry with a cloth towel. Place a drop of deionized water on the lens and
close the cover. Look through the eyepiece. The boundary of the shaded region should cross the
scale at the zero line. If it does not, inform your instructor so that she/he can adjust it or assign
you a different refractometer. If you have a problem reading the scale you can sharpen it using the
focus ring.
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Using an eyedropper, place one or two drops of your known (35o/oo) sample onto the
prism face as shown in Figure 7. Close the prism cover being careful not to trap any air
bubbles in the water on the prism face.
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Holding the prism toward the light, look though the refractometer and note where the
intersection lies between the upper shaded portion and lower clear portions of the scale.
This boundary represents the salinity. Record to the nearest part per thousand (º/ºº) and
enter in Table D on the answer sheet.
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. Rinse the prism and cover plate in deionized water and dry with a cloth towel.
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Repeat steps for the unknowns and record the salinities in Table D.
10 ppt
35 ppt
50 ppt
Unknown
MARS 101-LAB 6
Fall 2021
Salinity
E. Determination of salinity by chemical titration
(Knudson- Mohr Titration)
The final method of salinity determination that we will demonstrate is very precise (that is, it will
replicate well) and accurate (it produces a result that is very close to the true salinity). It is a
bit complicated; however, we introduce it here because for decades it was the standard technique
in oceanography for determining salinity.
In this section we will use a silver nitrate solution to precipitate out all of the chloride in a known
volume of artificial seawater. Although natural seawater contains a much wider array of ions
than a mixture of NaCl and fresh water, the analytical technique is the same. When we add a
solution containing silver nitrate (that is, Ag+ ions and NO3- ions) to a solution containing sodium
chloride (that is, Na+ ions and Cl- ions), the chloride ions in the solution will react with the silver
ions to produce a solid precipitate, silver chloride (and leaving the sodium and nitrate ions in
solution):
Hypothetically we could then dry and weigh the precipitate AgCl, and from the weight determine
the amount of chloride in the sample. But first we have to calculate the mass percentage of chloride
in silver chloride. This is done in the following manner:
From this we can see that AgCl contains 24.7% chloride ions. If we precipitate 100 grams of AgCl
from 1000 grams of seawater that would represent 24.7 grams of Cl-. Chloride represents a majority
of the negative ions present in seawater, but not all. Fortunately the proportion of chloride is
consistent. We know from chemical oceanography that chlorides make up about 55% of the total
salts (salinity) in seawater. Therefore if we know the chlorinity (the mass of chloride present) we
can determine the overall salinity:
Salinity = 100/55 x mass Cl- = 1.8 x mass ClIn the above example we measured 1000 grams of seawater and found 24.7 grams of chloride so
the salinity can be determined:
Salinity = 1.8 x mass Cl- = 1.8 x 24.7g Cl- = 44.5 º/ºº
MARS 101-LAB 6
Fall 2021
Salinity
The problem with drying and weighing the AgCl precipitate is that it takes a lot of time, and the
mass of the precipitate is a function of the oven temperature you use for drying, since the AgCl
can hold onto a significant amount of water even when it has seemingly dried out (similar problems
occur when we determine salinity by evaporation). So rather than drying and weighing the silver
chloride, we can use the same reaction to measure the salinity by knowing exactly how much
AgNO3 was used to precipitate all of the chloride. We can do this by adding another chemical
reagent, potassium chromate (K2CrO4), which acts as an indicator to tell us exactly when all of the
chloride in the seawater has reacted to form AgCl. The potassium chromate indicator remains
colorless as long as there is Cl- present, but the instant the last of the Cl- is bound up as silver
chloride, the solution turns orange. The orange color occurs when the extra chromate ion (CrO42) combines with the silver ion to form a complex ion called silver chromate.
The following two reagents will be made available for the titration analysis: AgN03 solution (50
grams of AgNO3 dissolved into a 1000 mL solution) and the K2Cr04 solution (3.5 grams of K2Cr04
dissolved into a 1000 mL solution).
The experimental setup is shown below in Figure 8.
MARS 101-LAB 6
Fall 2021
Salinity
Figure 8 : Set up for chemical titration. Note that the burette reads from top to
bottom.
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Pour approximately 20 mL of the 35o/oo sample into a 50 mL beaker.
Using a graduated 5 mL pipette, transfer exactly 5 mL of this 35o/oo sample into a beaker
Add 5 drops of the K2CrO4 solution to the same beaker. (Figure8).
Fill the 50 ml burette with the AgNO3 solution, pouring it carefully down a funnel into
the top of the burette. This can be done once for this entire set of four titrations. Record
the starting point in Table E.
MARS 101-LAB 6
Fall 2021
Salinity
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Add the AgN03 solution slowly from the burette and continuously stir it with the help of a
stirrer until you detects an abrupt color change from milky yellow to orange.
Record the new burette reading (the end point) in Table E.
Repeat the analysis for the known sample, again recording the starting and ending points on the
burette in Table E (the starting point for the second analysis should be the same as the ending
point for the first analysis).
Repeat steps to titrate the unknown sample, recording the data in Table E.
Calculate the salinity of unknown sample A using the average amount of AgNO3 required to
titrate the 35o/oo using the equation below:
Rearranging the above equation:
MARS 101-LAB 6
Fall 2021
Salinity