580340 Determination of Water Hardness by Titration Q
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Determination of Water Hardness by Titration
Jerret Jarvis
November 2, 2023
1
Data
Activity 1
Data Table 1: Complexometric Titration of Hard Water
Hard Water
Trial 1
Hard Water Trial 2
Hard Water
Trial 3
Initial
Syringe
Reading (mL)
1.0 mL
1.0 mL
1.0 mL
Final Syringe
Reading (mL)
0.6 mL
0.5 mL
0.2 mL
Volume of
EDTA
Consumed
(mL)
0.4 mL
0.5 mL
0.8 mL
Water
Hardness
ppm CaCO
3
(mg/L)
400.4 ppm
500.5 ppm
800.9 ppm
Average ppm CaCO
3
(mg/L):
567.23 ppm
© 2016 Carolina Biological Supply Company
2
Data Table 2: Complexometric Titration of Tap Water
Hard Water
Trial 1
Hard Water Trial 2
Hard Water
Trial 3
Initial
Syringe
Reading
(mL)
1.0 mL
1.0 mL
1.0 mL
Final
Syringe
Reading
(mL)
0.3 mL
0.5 mL
0.3 mL
Volume of
EDTA
Consumed
(mL)
0.7 mL
0.5 mL
0.7 mL
Water
Hardness
ppm CaCO
3
(mg/L)
700.7 ppm
500.5 ppm
700.7 ppm
Average ppm CaCO
3
(mg/L): 633.97 ppm
© 2016 Carolina Biological Supply Company
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3
Activity 2
Data Table 3: Complexometric Titration of Soft Water
Hard Water
Trial 1
Hard Water Trial 2
Hard Water
Trial 3
Initial
Syringe
Reading (mL)
1.0 mL
1.0 mL
1.0 mL
Final Syringe
Reading (mL)
0.7 mL
0.9 mL
0.7 mL
Volume of
EDTA
Consumed
(mL)
0.3 mL
0.1 mL
0.3 mL
Water
Hardness
ppm CaCO
3
(mg/L)
300.3 ppm
100.1 ppm
300.3 ppm
Average ppm CaCO
3
(mg/L): 233.57 ppm
1.
The calmagite indicator changes from a pink to a blue color during the
titration. Describe why the color change occurs.
It shows a chemical reaction occurred.
2.
Based on the results of your experiment, do you have hard or soft water?
Briefly explain your answer.
I have Hard water. The flask color turned pink and not purple.
3.
EDTA is added to some soaps and cleaning products to improve their
performance. Based on the results of your experiment, explain why it
would be beneficial.
The EDTA attracts the metal particles out of the hard water making
the water soft. It would be better for your skin.
© 2016 Carolina Biological Supply Company
4
4.
How could this experiment be modified to determine temporary or
permanent hardness of water?
Could use filtration and boiling methods to find temporary
hardness.
5.
A complexometric titration can also be used to determine the amount of
calcium in milk. The calcium concentration in milk is typically 1,200 mg/L.
How would you alter the procedure used in this experiment to determine
milk’s calcium content?
Photos
Photo 1
Photo 2
© 2016 Carolina Biological Supply Company
5
Photo 3
© 2016 Carolina Biological Supply Company
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Related Documents
Related Questions
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact
concentration of the standard NaOH solution to calculate the moles of NaOH.
Quantity
Еxample
Trial 1
Trial 2
Trial 3
M NaOH (exact
concentration)
0.992 M
0.953 M
0.953 M
0.953 M
V initial buret
reading = V,
0.20 mL
1.20 mL
0.52 mL
0.15 mL
V final buret
reading = V,
12.90 mL
14.22 mL
13.71 mL
13.31 mL
%3D
Vep = VNAOH
added = V; - V,
12.70 mL
13.02 mL
13.19 mL
13.16 mL
Vep = VNAOH in L
0.01270 L
0.01302 L
0.01319 L
0.01316 L
moles NaOH =
0.0126 mol
0.0124 mol
0.0126 mol
0.0125 mol
MNAOH X VNAOH
moles AA =
0.0126 mol
0.0124 mol
0.0126 mol
0.0125 mol
moles NaOH
V sample = V
acid
0.0150 L
0.0150 L
0.0150 L
0.0150 L
(15.00 mL)
(15.00 mL)
(15.00 mL)
Actual molarity
0.840 M
0.827 M
0.840 M
0.833 M
of AA
Average molarity for 3 trials =>
of AA
0.833 M
1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M).
2. Use your average AA concentration to calculate the mass…
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Data Table 3: Complexometric Titration of Soft Water
5 ml of water
1ml of buffer
Hard Water Trial 1
Hard Water Trial 2
Hard Water Trial 3
Initial Syringe Reading (mL)
1ml
1ml
1ml
Final Syringe Reading (mL)
77ml
79ml
75ml
Volume of EDTA Consumed (mL)
.23ml
.21ml
.25ml
Water Hardness
ppm CaCO3 (mg/L)
Average ppm CaCO3 (mg/L):
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Concentration sodium thiosulfate solution used:
0.056 mol L-1
ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED
Volume titration 1, (ml)
Volume titration 2, (ml)
Your Group
15.80
15.75
Group 1
16.05
15.70
Group 2
16.30
16.25
ANALYSIS
Average volume used, (mL)
Standard deviation
Number of moles sodium thiosulfate used, (mol)
Number of moles calcium iodate in solution, (mol)
Volume of calcium iodate used, (mL)
Concentration of saturated calcium iodate solution (mol L-¹)
Unrounded value
15.9750
0.26220
Rounded value
15.97
0.262
10.0
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Concentration sodium thiosulfate solution used:
0.056 mol L-1
ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED
Volume titration 1, (mL)
Volume titration 2, (mL)
Your Group
15.80
15.75
Group 1
16.05
15.70
Group 2
16.30
16.25
ANALYSIS
Average volume used, (ml)
Standard deviation
Number of moles sodium thiosulfate used, (mol)
Number of moles calcium iodate in solution, (mol)
Volume of calcium iodate used, (mL)
Concentration of saturated calcium iodate solution (mol L-¹)
Unrounded value
15.9750
0.26220
0.00089400
0.00036700 A
Rounded value
15.97
0.262
8.94 x 10-4
10.0
Minimize
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Calculate the total volume of HCl titrant delivered to the equivalence point for each trial
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How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations.
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Concentration sodium thiosulfate solution used:
0.056 mol L-1
ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED
Volume titration 1, (ml)
Volume titration 2, (mL)
Your Group
15.80
15.75
Group 1
16.05
15.70
Group 2
16.30
16.25
ANALYSIS
Average volume used, (mL)
Standard deviation
Unrounded value
Rounded value
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Preparation and Standardization of KMnO4 solution
Experimental data
Complete the table below.
Trial 1
0.2001 g
Trial 2
0.2065 g
Trial 3
Weight of sodium oxalate
(Na2C2O4, MM= 134 g/mol)
Titration data
0.2050 g
Final reading
Initial reading
29.86 mL
0.00 mL
30.66 mL
30.52 mL
0.00 mL
0.00 mL
Total vol. of KMNO4 used
Computed Molarity of KMNO4
solution
Mean Molarity
Computed Normality of KMNO4
Mean Normality of KMNO4
solution
Reaction Involved:
Calculations:
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Table 2. Titration data
Trial 1
Trial 2
Trial 3
Initial burette reading (mL)
1.19
2.26
2.39
Molarity of NaOH (M)
0.100
0.100
0.100
Volume of vinegar sample (mL)
5.00
5.00
5.00
Final burette reading (mL)
48.55
49.43
49.99
Expected color at end point
Volume of NaOH used (mL)
Average Volume of NaOH used in liters
Average moles of NaOH used (mol)
Average moles of acetic acid (mol)
Average molarity of acetic acid (M)
Average mass of acetic acid (g)
Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL)
Average mass % of acetic acid in vinegar
Known mass % of acetic acid in vinegar is 5.45%
Percent Error
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Determine the concentration of acetic acid and vinegar
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Sample #
1
2
0.2425
0.2160
0.2274
Weighed mass of ascorbic acid (g)
volume of KIO3 (mL)
18.86
17.91
17.37
0.02459
0.02462
0.02432
[KIO3] (mol L-1)
Mean [KIO3] (based on titration)
0.02451
mol L-1
Standard deviation in the mean [KIO3]
mol L-1
Confidence limit for the [KI03]
mol L-1
Relative confidence limit for the [KIO3]
ppt
=
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Part A: Standardization of a Sodium Hydroxide Solution
Titration 1
Titration 2
Titration 3
Mass of 125 mL flask
45.849g
46.715g
44.953g
Mass of flask and KHP
46.849g
47.745g
46.003g
Initial buret reading (mL)
0.5 ml
0.5 ml
0.5 ml
Final buret reading (mL)
27.8 ml
26.5 ml
26.7 ml
Volume of NaOH used (mL)
45.11 ml
45.06 ml
45.14 ml
Calculations
Titration 1
Titration 2
Titration 3
Moles of KHP
Moles of NaOH
Molarity of NaOH
Average Molarity of NaOH: _______________
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Data Table 1: Complexometric Titration of Hard Water
6ml of water used (5ml of hard water and 1ml of buffer)
Hard Water Trial 1
Hard Water Trial 2
Hard Water Trial 3
Initial Syringe Reading (mL)
1ml
1ml
1ml
Final Syringe Reading (mL)
0.55ml
.50ml
.33ml
Volume of EDTA Consumed (mL)
0.45ml
.50ml
.77ml
Water Hardness
ppm CaCO3 (mg/L)
Average ppm CaCO3 (mg/L):
photo shows equation that needs to be used to solve
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20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments.
14.0
12.0
10.0
HO
8.0
6.0
4.0
2.0
0.0
0.0
10.0
20.0
30.0
Volume of titrant (mL)
40.0
444444
50.0
(a) Is the species being titrated an acid or a base?
(b) Is the species being titrated strong or weak?
(c) What is the value of Ka (if a weak acid) or K (if a weak base) for the species being titrated?
If the species is strong (100% dissociated), enter 999.
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Hi, I just need to know the correct answer for these. Thank you
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Data:
Table 1: Titration of 1.00 mL H2O2 with KMNO4
0.1134M
Concentration of KMNO4
Trial #
Initial KMNO4 Volume (mL)
Final KMNO4 Volume (mL)
Volume KMnO4 Used (mL)
1
10
2
10
19.7
19.7
29.6
Pre-lab:
1.
What is a titrant? What is the titrant in this lab?
2. What is an analyte? What is the analyte in this lab?
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A student performed three aqueous layer titrations in Part 1 and they reported the
following measurements:
Final Burette
Reading
Initial Burette
Reading
Volume of Aqueous
Aliquot
Final Burette
Reading
Initial Burette
Reading
Volume of Sodium
Thiosulfate
Determination #1
16.33 mL
6.50 mL
9.83 m
31.98 mL
0.76 mL
31.22 mL
Determination #2 Determination #3
26.76 mL
16.33 mL
10.43 mL
33.62 mL
0.88 mL
32.74 mL
36.95 mL
26.76 mL
10.19 mL
32.22 mL
0.41 mL
31.81 mL
Which determinations were the student's 'best two'? Calculate the percent
difference for the 'best two' and show the complete calculation. Note that the
concentration of standard sodium thiosulfate, which the student used, is unknown.
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A drug is ordered to be administered IV at the initial rate of 4 mU/min, and may increase by 2 mu/min q 15 min to a max of 10 mU/min. The IV strength is 5 mU/mL.
Construct the first two lines of the titration table for this order.
O A. Dose Rate (mU/min) IV rate (mL/h)
4 mU/min (initial)
8 mU/min
36 mL/h
48 mL/h
O B. Dose Rate (mU/min)
4 mU/min (initial)
6 mU/min
Oc. Dose Rate (mU/min)
4 mU/min (initial)
6 mU/min
O D. Dose Rate (mu/min)
4 mU/min (initial)
6 mu/min
IV rate (mL/h)
24 mL/h
48 mL/h
IV rate (mL/h)
48 mL/h
72 mL/h
IV rate (mL/h)
36 mL/h
36 mL/h
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Understanding of food analysis methods. Principles of method described compared to other techniques.
1 The MOHR Titration, AOAC Method? What is it and how does it work? How can it be used to quantify salt in a sample.
2 Are there any advantages and/or disadvantages of this method?3 Are there any alternate methods better than the Mohr Titration toquantitatively determine salt in a sample?
4. Diseases with recent statistics? Refer to World Health Organisation?
5. Why analayse salt?
6. Consumption?
7. Main aims of study?
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Titration Experiment 1: Acid-Base Titration: Unknown HCl
Write chemical equation
*+ HClcags N s
→ Naclceg) + H,O
Write NIE
OH c) + HEogs → H2OC)
Enter the data into the table and choose three titrations to find the molarity of the unknown HCI.
Unknown # HCI
Titration 1 Titration 2 Titration 3 Titration 4 Titration 5
Volume NaOH used to titrate
unknown HCI solution
17.43ml 16.5O ml662 mll16.57ml16.6dmL
Molarity of NaOH used for
each titration
0.2564
0.1787/01692/0.1704/oiado1703
Molarity of HCI
Average M HCI (avg ±
standard deviation)
10.1717
1.63
% Precision
Calculations
1. Provide one representative calculation that you used to determine the molarity of HCI. Be
sure to show all units and use proper sig figs!
V HCI-25mL
MHCI =?
VN2OH = 16.6lmL
MNAOH=0.2564
MHCI VHCI=MNAOH VAa OH
MHCI 25=O. 1564 16.61
MHCI= 0.2564.16.61
25
MHCI=0.1703
2. Average molarity of three titrations.
6.1787+0.1692+0.1704+0.1619+ O.1703
MACI= 0.117
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Xanthurenic acid stock solution
Absorbance
25
0.052
50
0.128
75
0.202
100
0.310
150
0.448
200
0.621
Plot a graph, from graph, y=mx (force the trend line to pass through origin since the blank with no xanthurenic acid was set to be zero absorbance) in which, y: Absorbance, x concentration
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30
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Calculate the average concentration of Vitamin C in each sample
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Acid-Base titration:
Standardization of 0.1 M NAOH
Trial 1
Mass KHP used, g
0.297 g
Final reading
Volume NaOH, mL
15.59 mL
Initial reading
Volume NaOH, mL
0.23 mL
Volume NaOH
consumed, mL
15.36 mL
Moles KHP used
Moles NaOH used
Molarity of NaOH
solution
arrow_forward
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Related Questions
- Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…arrow_forwardData Table 3: Complexometric Titration of Soft Water 5 ml of water 1ml of buffer Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):arrow_forwardConcentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (ml) Volume titration 2, (ml) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (mL) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 Rounded value 15.97 0.262 10.0arrow_forward
- Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (mL) Volume titration 2, (mL) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (ml) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 0.00089400 0.00036700 A Rounded value 15.97 0.262 8.94 x 10-4 10.0 Minimizearrow_forwardCalculate the total volume of HCl titrant delivered to the equivalence point for each trialarrow_forwardHow much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations.arrow_forward
- Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (ml) Volume titration 2, (mL) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (mL) Standard deviation Unrounded value Rounded valuearrow_forwardPreparation and Standardization of KMnO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 Weight of sodium oxalate (Na2C2O4, MM= 134 g/mol) Titration data 0.2050 g Final reading Initial reading 29.86 mL 0.00 mL 30.66 mL 30.52 mL 0.00 mL 0.00 mL Total vol. of KMNO4 used Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:arrow_forwardTable 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.55 49.43 49.99 Expected color at end point Volume of NaOH used (mL) Average Volume of NaOH used in liters Average moles of NaOH used (mol) Average moles of acetic acid (mol) Average molarity of acetic acid (M) Average mass of acetic acid (g) Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL) Average mass % of acetic acid in vinegar Known mass % of acetic acid in vinegar is 5.45% Percent Errorarrow_forward
- Determine the concentration of acetic acid and vinegararrow_forwardSample # 1 2 0.2425 0.2160 0.2274 Weighed mass of ascorbic acid (g) volume of KIO3 (mL) 18.86 17.91 17.37 0.02459 0.02462 0.02432 [KIO3] (mol L-1) Mean [KIO3] (based on titration) 0.02451 mol L-1 Standard deviation in the mean [KIO3] mol L-1 Confidence limit for the [KI03] mol L-1 Relative confidence limit for the [KIO3] ppt =arrow_forwardPart A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________arrow_forward
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