580340 Determination of Water Hardness by Titration Q

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…

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):

Calculate the total volume of HCl titrant delivered to the equivalence point for each trial

How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations.

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

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:

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

Determine the concentration of acetic acid and vinegar

Titration Titrant Reductant/ Oxidant Analyte Standardizing Indicator Reagent COD BOD INDIRECT TITRATIONKindly identify the blank sections appropriately.

Procedure Preparation of Dilute Solution of Vinegar • Using a 10 mL pipette, transfer 10mL of vinegar into 100 mL volumetric flask.  • Dilute to mark of the volumetric flask using distilled water. B. Titration of Diluted Solution of Vinegar  • Transfer 25 mL of diluted solution to 250 mL Erlenmeyer flask.  • Add 0.5 mL phenolphthalein indicator. Set aside.  • Transfer 50mL of 0.110 M NaOH into a 50 mL burette.  • Titrate the diluted solution until the phenolphthalein endpoint (very faint pink).  • Record volume of NaOH used. Answer the question: What is the experimentally determined concentration of acetic acid in your vinegar solution: (Please give your answer to three significant figures.) ______ M Acetic Acid

Answer if true or false , if false, put the correct answer 1. Molarity of titrant = number of moles analyte / volume of analyte 2. Two general types of titration curves are sigmoidal and linear segment 3. Tritration must occur slowly 4. Primary standard has high purity and is stable 5. Using phenlphthalein indicator, acidic to basic endpoint is usually colorless

Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12 11- 11- 10- 10- 9- 9- 8- 8- 7- 7- 6- 6- 5- 5- 4- 3- 3- 2- 2 1 10 15 20 25 30 35 40 45 50 10 15 20 25 30 35 40 45 50 Titrant.volume Cml). Titrant.volume (mL). Answer Bank This graph does not represent a titration. a basic solution titrated with an acid an acidic solution titrated with a base Hd Hd

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 =

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: _______________

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.

Hi, I just need to know the correct answer for these. Thank you

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?

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

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?

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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Calculate the average concentration of Vitamin C in each sample

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

In the six runs indicated below 1.2 x 105 M stock solution of the crystal violet used. RUN CV + 10.00 mL 6.00 mL 4.00 mL 10.00 mL 6.00 mL B. Only III and IV are correct OC. Only II and III are correct BEAKER 1 D. All of the four statements are correct O E. Only I, II, and III are correct H ₂0 BEAKER 2 1 2 3 4 5 4.00 mL 6 4.00 mL 6.00 mL Which of the following statements is or are correct: I. The initial concentration of NaOH solution in the mixture of runs 1 is 0.025 M, and in runs 4 is 0.015 M II. The initial concentration of crystal violet solution in the mixture of runs 1 is 1.2 x 10-6 M and in runs 3 is 6.0 x 10-6 M III. The used time range of data collection per each run is 5 min. During this period; the temperature is assumed to remain constant. IV. The addition of water will dilute CV +-solution, this dilution will make runs 1 to 3 of different slopes of the inear plots of In A vs. t. OA. Only I and III are correct 4.00 mL 6.00 mL 0.05 M NaOH 10.00 mL 10.00 mL 10.00 mL 6.00 mL…

Data Table 2: Complexometric Titration of Tap Water photo shows equation to find water hardness  6 ml of water used (5 ml of tap water 1ml of buffer)     Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 2ml 2ml 2ml Final Syringe Reading (mL) .61ml .69ml .58ml Volume of EDTA Consumed (mL) 139ml 131ml 142ml Water Hardness ppm CaCO3 (mg/L)         Average ppm CaCO3 (mg/L):

Experiment :CONDUCTOMETRIC TITRATION OF A MIXTURE OF ACIDS WITH A STRONG BASE I want the calculations for this Experiment with the graph note:  M:0.01M

5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.

With the attached data, how do I calculate the mass percent of vinegar?

Question 24 This problem requires a numerical answer. Type your answer into the box provided. Do not include any units. Report the answer to two decimal places. If Canvas rounds to fewer that is ok, but you should not do so independently. 5.00 mL of 0.100o M ammonia (NH3, K, = 1.8x10 5) is titráted with 0.100 M HNO3. Calculate the %3D pH after 1.00 mL of HNO3 is added.