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Performing a Urinalysis: Physical Examination
There are several steps to performing a urinalysis in the clinical laboratory. This lecture will go over the first step and covers what we will be doing on our first day in urinalysis lab.
The first step in performing a urinalysis is the physical examination. This includes recording the color and clarity of the sample. This may also include a specific gravity
measurement on a refractometer.
Color and Clarity
Before observing the color and clarity, it is important to mix the sample well, as particles sometimes collect in the bottom of the urine cup. If the urine cup is not clear, and color and clarity cannot accurately be determined, it is also good practice
to pour it off into a clear tube to best determine the color and clarity of the sample.
Urine can come in various colors, but there is a standard when determining urine colors, that we must follow in the lab. Unfortunately, we are not allowed to come up with our own descriptions and determine that a urine sample looks to be canary
yellow. Below are the color descriptions that are expected to be used in the laboratory when determining urine color.
Normal Urine Color
Typically, normal urine is represented by some shade of yellow, and this is due to the urochrome pigmentation. Appropriate descriptions are as follows:
Colorless
Pale Yellow (also commonly referred to as Light Yellow, Straw)
Yellow
Dark Yellow
Amber
Abnormal Urine Color
The abnormal urine colors include:
Orange-yellow
Yellow-green
Green
Blue-green
Pink-red
Portwine
Red-brown
Brown-black
Refer to the table in your textbook that describes the different causes for varying colors of urine.
When working in a hospital laboratory, most computer systems will have the tech select a color choice, rather than having them type in a color. This helps to streamline variation in terminology. The terminology above is what is used in our textbook, so when determining color and clarity, we are going to stick with these descriptions.
Shades of pink and red are some of the most common deviations from the normal shades of yellow urine colors. Pink and red urine can have various causes. The flow chart below helps to determine if the source of the red urine is due to
hemoglobinuria, myoglobinuria, or hematuria. Note that if the sample is red and cloudy, this can be indicative of red blood cells being present in the urine. However,
we must rule out the possibility that the cause of the cloudy sample could be due to
white blood cells, mucus, bacteria, etc.
Clarity
Normal freshly voided urine is typically clear. The presence of particles in the urine can create a hazy or cloudy appearance. Fresh urine that exhibits cloudiness is a good indicator that the sample will require a microscopic exam, although not all cloudiness indicates a pathological issue
The following terms are used to describe urine clarity:
Specific Gravity
The specific gravity is also included in the physical examination of urine. Most current test methods will include a specific gravity in their chemistry measurement. However, previous methods included the urinometer and refractometer for determining the specific gravity of urine.
In our college lab, we will learn how to use the refractometer but will utilize reagent strip testing to determine the specific gravity for most of our samples.
Refractometer
A refractometer is a meter that measures the total solids of a solution, usually by measuring the refractive index of the solution.
Refractive Index- the ratio of the velocity of light in air to the velocity of light in solution.
One downside to using the refractometer is that the presence of dense molecules requires a correction. Due to the influence of highly dense molecules such as protein and glucose on specific gravity, certain laboratory procedures necessitate adjustments for elevated concentrations of glucose and protein. This correction involves subtracting 0.003 from the specific gravity reading for every 1g/dL of protein and 0.004 for every 1g/dL of glucose.
Specific Gravity on Reagent Strip
Some reagent dipsticks feature a specific gravity measurement pad based on the dissociation constant of pretreated polyelectrolytes in relation to ionic concentration. This procedure assesses the ionic concentration of urine, correlating
with specific gravity. Polyelectrolytes in the pad have acid groups that dissociate based on the ionic concentration. More ions lead to more dissociation, changing pH. The reagent pad contains a pH indicator to measure this change. Higher urine specific gravity makes the pad more acidic, reflected in color changes from deep
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Related Questions
Consider four distinct physical properties: boiling point, melting point, solubility, and density. Which of these physical properties do you think allows thin layer chromatography (TLC) to work? Choose one then, explain your reasoning.
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STANDARD SAMPLE PREPARATIONS FOR ABSORBANCE & CONCENTRATION DATA
Concentration of stock nickel sulfate hexahydrate solution = .400 Molarity
Sample
Volume
Absorbance
Concentration (In Molarity)
a
5 mL
.179
10 mL
.329
15 mL
.588
20 mL
.760
25 mL
.939
Reference Blank = 0
Please show how to find Molarity, please show
steps. Thank you and stay safe.
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In a test tube, dissolve 10 drops of methanol in 3 ml. of water. Oxidize a copper wire spiral by passing it through a Bunsen burner. Plunge the red-hot wire into the alcohol solution several times, cooling the solution under the tap (faucet) so as not to evaporate too much of it.
Next, add 1 drop of 0.5% resorcinol solution. Measure 2 ml. of concentrated sulfuric acid (CAUTION!) and pour this carefully down the sides of the test tube containing the mixture. Note the color of the zone intermediate between the acid and the solution.
RESULT:
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How to determine the difference between primary , secondary and tertiary alcohol in the laboratory
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Dissolution
Distilled H20
Concentration
0.01 M HCI
Concentration
(mg/ml)
Time
Total amount
A
Total amount
A
(mg/ml)
(mg)
(mg)
5
0.16
0.1
10
0.24
0.18
15
0.35
0.25
20
0.48
0.34
25
0.58
0.4
30
0.67
0.5
1. Plot the given data on an ordinary paper and find the slope for each line then calculate the
IDR constant for aspirin in the two dissolution media, water and HCI.
NOTE: Slope of the calibration curve = 1.0 (mg/ml and saturation solubility of salicylic acid
is equal to 2.0 gm/L.
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Table 2: Absorbance Values of Standards and Unknowns.
Sample
Blank
Standard Solution 1
Standard Solution 2
Standard Solution 3
Standard Solution 4
Standard Solution 5
Water Sample 1
Water Sample 2
Phosphate Concentration
(in ppm)
Y17
0 ppm
0.02 ppm
0.04 ppm
0.08 ppm
0.16 ppm
0.32 ppm
Freeman Lake
0.001
0.325
0.292
0.413
0.315
0.039
0.054
0.049
Absorbance at
2= 690 nm
Calculations:
1. Construct a phosphate standard curve in Excel by plotting concentration (in ppm) on your
x-axis and Absorbance (unitless) on your y-axis for your known solutions. Label the axes
on the graph and provide the curve with a title. Use a linear trendline to generate a best fit
line to your data. Label the graph with the equation and the R" value. Insert your labeled
graph in the space below.
X
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Color BEFORE adding
Color AFTER adding
Intensity of color AFTER
adding FeCl3
Test Tube #
FeCl3
FeCl3
#1 (salicylic acid)
clear
lilac
100%
#2 (commercial aspirin A) clear
slightly pink
50%
#3 (commercial aspirin B) clear
lilac
95%
#4 (aspirin from your
clear
pink
20%
synthesis above)
#5 (control)
clear
clear
0%
Based on this data and the melting point of Aspirin, how pure is the synthesized product?
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Pre-lab question #8: Suppose you were dissolving a metal such as zinc with
hydrochloric acid. How would the particle size of the zinc affect the rate of its
dissolution? As the particle size of the zinc increases, the rate of dissolution
AA (decreases/increases).
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You obtain an Unknown Sample from the Stockroom. You begin testing the solution through the steps outlined in the flowchart of the experiment’s PDF file. You first add HCl and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Addition of the hot water dissolves some of the precipitate, but some white precipitate still remains on the bottom of the test tube. You pour off the supernatant liquid, and add ammonia (NH3) to the remaining precipitate. You now observe the formation of a gray-black precipitate.
Which of the following is a valid conclusion to draw at this point?
Select one:
Hg22+ is definitely present.
Pb2+ is definitely present.
Ag+ could be present, or Hg22+ could be present, or BOTH could be present.
Ag+ is definitely present
arrow_forward
You obtain an Unknown Sample from the Stockroom. You begin testing the solution through the steps outlined in the flowchart of the experiment’s PDF file. You first add HCl and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Addition of the hot water dissolves some of the precipitate, but some white precipitate still remains on the bottom of the test tube.
Which of the following is a valid conclusion to draw at this point?
Pb2+ is definitely present.
Hg22+ is definitely present.
Ag+ could be present, or Hg22+ could be present, or BOTH could be present.
Ag+ is definitely present
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Current Attempt in Progress
From the curves shown in Animated Figure and using the following Equation, determine the rate of recrystallization for pure copper
at the several temperatures. Make a plot of In(rate) versus the reciprocal of temperature (in K-1). (a) Determine the activation
energy for this recrystallization process. (See Section FACTORS THAT INFLUENCE DIFFUSION.) (b) By extrapolation, estimate the
length of time required for 50% recrystallization at room temperature, 20°C (293 K).
(a) i
kJ/mol
(b) i
days
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30
20
10
From the procedure
2. Assemble the simple distillation apparatus as generally shown in Figure SD.1 in the lab manual, ensuring that the thermometer bulb is aligned at, or slightly below, the Y in
the distillation head. Each ground joint is greased by putting three or four stripes of grease lengthwise around the male joint and pressing the joint firmly into the other
without twisting.
3. Attach a water condenser to the distillation head.
4. Remember, water goes in the bottom and out the top. Attach a clamp holder to the end of the drain tube to keep it weighted in the drain. Turn water to a trickle. If it is
slowly draining, it is high enough. Begin a low flow of water through the condenser.
5. Place the set up on a heating/stir plate.
6. Turn on the hot plate to start heating the solution. Monitor the temperature and the boiling of the solution throughout the distillation process.
7. Record the temperature of the distillate when the first drops are recovered.
30.0
8. Adjust…
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Define Extraction in chemistry ?
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1. Solubility Test
Table 1. Results for the solubility test.
OBSERVATION*
INFERENCE
SAMPLE
Ethyl acetate
**
Нехаne
Methanol
Water
Coconut oil
Vitamin E
Beef fat
Miscible (soluble) or immiscible (insoluble)
** polar or nonpolar
Sudan IV Test
Table 2. Results for Sudan IV test.
OBSERVATION*
INFERENCE
SAMPLE
Нехаne
Ethyl acetate
Methanol
Water
**
Coconut oil
Vitamin E
Beef fat
Homogeneous or heterogeneous mixture
** polar or nonpolar
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3. The Maximum Acceptable Concentration (MAC) of Pb in drinking water is 10 ppb. If a sample hasconcentration of 65 nM, what will be the concentration in ppb and does it exceed the MAC?a. 8 ppb, no it didn’t exceed the MACb. 9 ppb, no it didn’t exceed the MACc. 12 ppb, yes it exceeds the MACd. 13 ppb, yes it exceeds the MAC
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50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution.
Information of stock solution -
molar mass- 534.3g/mole
0.587g in MilliQ
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1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data
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What are the types of gravimetric methods? Give an examples where each method is used in an analysis.
What is particulate gravimetry? When do we use this technique?
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A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. You subject it to spectroscopic analysis, in order to get the concentration of amine in this compound. Next, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample, and you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. What is the molecular weight of the compound? (The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.)
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When purifying a sample of aspirin that was produced in the lab, the impure aspirin sample should be dissolved in a very cold solvent, so that solid impurities can be filtered and analyzed the next day or the next week.
True or False?
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Pre Lab Questions: (Each answer is to be written as a complete sentence)
What is the reason for washing the precipitate with water in Step 9?
Define precipitate. Define filtrate.
In Step 2, what is the purpose for rinsing the stirring rod?
read the Procedure to answer the questions
Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker.
Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring.
Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker.
Repeat Step 2 for the solution in the 50 mL beaker.
Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir.
Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel.
Slowly…
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Different type of methods used in household contaminated wastewater purification
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2.
Questions:
1.
CHM-202 Lab 2 Freezing Point Depression Rev2 G6-2022
10/14
From your understanding of colligative properties, how would you design an experiment to
measure the freezing point of a material which freezes at -2 °C using the same apparatus used in
this laboratory and any chemical reagents commonly found in a chemical laboratory. Ice is the
only material you have available to cool the solutions.
If you measured the boiling point of the solution used in Trial 4, would you predict it would have
a boiling point equal to, higher than, or lower than the boiling point of pure cyclohexane?
Explain your answer.
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Which of the following are properties of a good recrystallization solvent? Check all correct answers.
Group of answer choices
boiling point of solvent < melting point of crystals
boiling point of solvent > melting point of crystals
Crystals are soluble in solvent at low temperature and soluble at high temperatures.
Crystals are soluble in solvent at high temperatures but insoluble or slightly soluble at low temperatures.
Solvent boiling point is about room temperature.
Impurities should be either soluble at all temperatures or insoluble at all temperatures.
An abundant amount of crystals must be recoverable from the solvent.
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A student was given a stock ascorbic acid solution of 2.323
mg/L. Following the directions in the lab, the student obtained
the data below. Calculate the concentration of ascorbic acid in
the Standard (in microgram/L,
ug
-). Report your answer with
one place after the decimal.
initial
final
initial volume final volume
volume
volume
color reagent color reagent
stock
stock
solution
solution
solution
solution
Standard 1.35 mL
6.64 mL
5.12 mL
9.32 mL
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PART 3- LABORATORY EQUIPMENT
EQUIPMENT NAME
FUNCTION
To hold test tubes.
Attaches to a retort stand to support glassware being heated.
To pour liquid from a large container into a small container.
To provide a flame during an experiment.
ones
To light the Bunsen burner.
To attach test tubes to a retort stand.
To clean substances out of a test tube.
To hold a hot crucible or flask.
To hold a hot test tube.
To place on the lab bench to prevent burning or to use with ring clamp.
To transfer small amounts of liquid.
To grow bacteria or contain small experiments.
To hold liquids.
To measure liquids.
To contain experiments (a stopper can be used to close the flask).
To hold a hot beaker.
To perform an experiment with a different substance in each well.
To hold chemicals and perform experiments in.
To scoop and transfer small amounts of substances,
To stir during experiments that involve mixing or dissolving.
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The unknown salt you will be identifying is composed of one of the 6 anions and one of the 6 cations studied during previous weeks of lab. However, the list is not endless. An obvious physical property can be used to eliminate some salts. Another physical property can imply or eliminate possibilities as well. During this lab, what are two physical properties that can be used?
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Part C: Determination of the alcohol content of unknown liquor Stretien
Volume (mL)
Sample
ТИШТИНА
0.00% alcohol
10.0% alcohol
20.0% alcohol
40.0% alcohol
50.0% alcohol
Unknown
Mass (g)
1o podina ko
9.8919
9.7899
9.600
9
9.420 д
% Alcohol content of the liquor_
9.2155
9.5089
2VLELA CVOLION EAEK EVI OK DRA
IVBOKY LOBAN
ocen
10.00
10.00
10.00
10.00
10.00
10.00
Density (g/mL)
0.00% alcohol calculation:
ися
→
о
0.99 во
0.99
Ano 7 si dotaW 120.00
supirmbest sdi
na
LANG
411
be: [scpoidas:
0.97
0.94 in oil to notisalarisi
0.92
0.95
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All changes save
7. When two solutions are mixed, a color change occurs. The data tables show the time between mixing and the color change for two sets of conditions. For
Condition One, the solution concentrations were constant and temperature varied. For Condition Two, the temperature was constant and concentrations varied.
Condition One: Concentration
Time for
Temperature
(°C)
Sample
Color to
Change
1
10°
36 sec
22°
14 sec
Condition Two: Temperature
Time for
Concentration
Sample
Color to
%
Change
1.
100%
15 sec
2.
50%
24 sec
Which of these statements is true according to the data?
O The reaction rate is greater at 22°C than at 10°C.
O Reducing the temperature increases the rate of the reaction.
The reaction is affected by changes in temperature
not by changes in concentration.
O Decreasing the concentration increases the reaction rate.
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- Consider four distinct physical properties: boiling point, melting point, solubility, and density. Which of these physical properties do you think allows thin layer chromatography (TLC) to work? Choose one then, explain your reasoning.arrow_forwardSTANDARD SAMPLE PREPARATIONS FOR ABSORBANCE & CONCENTRATION DATA Concentration of stock nickel sulfate hexahydrate solution = .400 Molarity Sample Volume Absorbance Concentration (In Molarity) a 5 mL .179 10 mL .329 15 mL .588 20 mL .760 25 mL .939 Reference Blank = 0 Please show how to find Molarity, please show steps. Thank you and stay safe.arrow_forwardIn a test tube, dissolve 10 drops of methanol in 3 ml. of water. Oxidize a copper wire spiral by passing it through a Bunsen burner. Plunge the red-hot wire into the alcohol solution several times, cooling the solution under the tap (faucet) so as not to evaporate too much of it. Next, add 1 drop of 0.5% resorcinol solution. Measure 2 ml. of concentrated sulfuric acid (CAUTION!) and pour this carefully down the sides of the test tube containing the mixture. Note the color of the zone intermediate between the acid and the solution. RESULT:arrow_forward
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- Color BEFORE adding Color AFTER adding Intensity of color AFTER adding FeCl3 Test Tube # FeCl3 FeCl3 #1 (salicylic acid) clear lilac 100% #2 (commercial aspirin A) clear slightly pink 50% #3 (commercial aspirin B) clear lilac 95% #4 (aspirin from your clear pink 20% synthesis above) #5 (control) clear clear 0% Based on this data and the melting point of Aspirin, how pure is the synthesized product?arrow_forwardPre-lab question #8: Suppose you were dissolving a metal such as zinc with hydrochloric acid. How would the particle size of the zinc affect the rate of its dissolution? As the particle size of the zinc increases, the rate of dissolution AA (decreases/increases).arrow_forwardYou obtain an Unknown Sample from the Stockroom. You begin testing the solution through the steps outlined in the flowchart of the experiment’s PDF file. You first add HCl and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Addition of the hot water dissolves some of the precipitate, but some white precipitate still remains on the bottom of the test tube. You pour off the supernatant liquid, and add ammonia (NH3) to the remaining precipitate. You now observe the formation of a gray-black precipitate. Which of the following is a valid conclusion to draw at this point? Select one: Hg22+ is definitely present. Pb2+ is definitely present. Ag+ could be present, or Hg22+ could be present, or BOTH could be present. Ag+ is definitely presentarrow_forward
- You obtain an Unknown Sample from the Stockroom. You begin testing the solution through the steps outlined in the flowchart of the experiment’s PDF file. You first add HCl and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Addition of the hot water dissolves some of the precipitate, but some white precipitate still remains on the bottom of the test tube. Which of the following is a valid conclusion to draw at this point? Pb2+ is definitely present. Hg22+ is definitely present. Ag+ could be present, or Hg22+ could be present, or BOTH could be present. Ag+ is definitely presentarrow_forwardCurrent Attempt in Progress From the curves shown in Animated Figure and using the following Equation, determine the rate of recrystallization for pure copper at the several temperatures. Make a plot of In(rate) versus the reciprocal of temperature (in K-1). (a) Determine the activation energy for this recrystallization process. (See Section FACTORS THAT INFLUENCE DIFFUSION.) (b) By extrapolation, estimate the length of time required for 50% recrystallization at room temperature, 20°C (293 K). (a) i kJ/mol (b) i daysarrow_forward30 20 10 From the procedure 2. Assemble the simple distillation apparatus as generally shown in Figure SD.1 in the lab manual, ensuring that the thermometer bulb is aligned at, or slightly below, the Y in the distillation head. Each ground joint is greased by putting three or four stripes of grease lengthwise around the male joint and pressing the joint firmly into the other without twisting. 3. Attach a water condenser to the distillation head. 4. Remember, water goes in the bottom and out the top. Attach a clamp holder to the end of the drain tube to keep it weighted in the drain. Turn water to a trickle. If it is slowly draining, it is high enough. Begin a low flow of water through the condenser. 5. Place the set up on a heating/stir plate. 6. Turn on the hot plate to start heating the solution. Monitor the temperature and the boiling of the solution throughout the distillation process. 7. Record the temperature of the distillate when the first drops are recovered. 30.0 8. Adjust…arrow_forward
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