Trials 1 2 Volume of aliquot of standard CaCO, solution 25.00 25.00 25.00 (ml) Volume of titrant, EDTA (ml) 23.20 23.50 23.34 Titer (mg CaCO̟ImL EDTA) Trial 1 Trial 2 Trial 3
Q: Ag* 0.0000133038 Cr 0.0000133038
A: Concentration of Ag+ = 0.0000133M Concentration of Cl- = 0.0000133M
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
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Q: (b) 50 mL of 0.005 M Pb2* solution buffered at pH 10 is to be titrated with 0.01 M EDTA solution.…
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Q: Kide solution. Trial 1 Trial 2 Trial 3 ,4 28.01 49,6041.10 28.0123,3O to'9 Ĉ 2.89x1041,963.0 21.6…
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Q: A foot powder sample containing Zn was dissolved on 50.00 ml water and was titrated to the end point…
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Q: Hd 14 12 10 00 5 4 2 0 0 Titration Data 0.5ml Volume (ml) 1.0ml 2ml
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Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
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Q: solution is mixed with 40.00 mL of 1.2% (w/v, g/mL) Na2CO3 solution. What volume of 0.087 M HCl will…
A: The question is based on the concept of titrations. we are titrating a mixture of bases with a…
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
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Q: concentration
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Q: What is the result of the Analytical Method Validation of 0.1 N H2SO4 Standardization? Given: 50…
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Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
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Q: Part Il: Determination of Standard Solutions mL of 0.200 mL H20 added Tube # M Cuso, M CusO4-5 H20…
A: In the given question, the molarity of CuSO4 solution needs to be determined from the given data.
Q: Concentration EDTA (M): 1.94e-3 Trial #1 Trial #2 Trial #3 Volume of Water Sample titrated…
A: Given,Concentration of EDTA = 1.94 × 10-3 M = 1.94 × 10-3 mol/LVolume of water sample titrated (mL)…
Q: With the attached data, how do I calculate the number of moles of HC2H3O2 in 5.00mL of vinegar?
A: Given:Molarity of NaOH = 0.2012Volume of NaOH = 21.20 mLVolume of HC2H3O2 = 5.00 mLChemical reaction…
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
A: Correct option is (b) .
Q: What is the type of titration is involved this method? Direct Indirect Residual Blank 2. What is…
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Q: A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient…
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Q: 4. (review: multi-point standard addition method) Calcium is determined in river water sample using…
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Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
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Q: Titration Heating Volume of DCIP (ml) Average Amt of Conc of #3 time vol of Vit C in Vit C Sample…
A: Ascorbic acid in Vitamin C reacts with DCIP in 1:1 fashion.
Q: A 50.00-mL aliquot of solution containing 0.310 of MgSO4 (FM 120.37) in 0.500 L required 37.77 mL of…
A: Given, 50.00-mL aliquot of solution containing 0.310 g of MgSO4 (FM 120.37) in 0.500 L required…
Q: A foot powder sample containing Zn was dissolved on 200.00 mL water and was titrated to the end…
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Q: Calculate Average Molarity of EDTA and Relative Average Deviation (R.A.D.)
A: According to Law of Chemical Equivalence M1V1 = M2V2 M1 = molarity of EDTA = M2V2/V1 Trial…
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl,…
A:
Q: Compute for the molar concentration of EDTA standardized using 50.00 mL of the CaCO3 primary…
A: EDTA complexometric titration is based on the fact that many metallic ions form stable complexes…
Q: 1. How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW:…
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Q: What would your main concern be if you accidentally used wash buffer (10mM imidazole) instead of…
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A: Given:Al with ICP-AES = 2 ppb = 2 µg/L = 2×10-6 g/L.Mass of Al with GF-AAS = 5 picogram = 5×10-12…
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Q: With the attached data, how do I calculate the mass percent of vinegar?
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Q: Standardization of EDTA Solution Weight of pure CaCO3: 0.2517 g % Purity of CaCO3: 98.0% Total…
A: The experiment data given is, Trial 1 2 3 The volume of standard CaCO3 solution (ml) 25.00…
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
A:
Q: In the next part of the experiment, you used the standard solution of sodium oxalate to standardize…
A: The data given is,
Q: Volume HCl (mL) 25.00 а. 0.00 b. Initial buret reading (mL) 25.40 c. Final buret reading (mL) 25.40…
A: Equation NaOH(aq) + HCl (aq) ——> NaCl (aq) + H2O(l) Molarity = no. of moles / volume (Lt)
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
A: Given, 0.3045 g of CaCO3 dissolved in concentrated HCl and dilute to mark 250 mL Molar mass of…
Q: Chosen wavelength : 400 nm EDTA Volume (mL) Absorbance O mL 0.445 1 mL 0.439 2 ml 0.434 3 ml 0.428 4…
A: Answer
Q: II. A saturated solution of Ca(lO3)2 was prepared by dissolving pure Ca(IO3)2 in D.I. water; after…
A: #(i): IO3-(aq) reacts with S2O32-(aq) according to the reaction below: IO3-(aq) + 6S2O32-(aq) +…
Q: A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient…
A:
Q: [Standardization] A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCI,…
A:
Q: A foot powder sample containing Zn was dissolved on 100.00 mL water and was titrated to the end…
A: The question is based on the concept of complexometric titrations. We have to calculate P value of…
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Q: Data & Results: Complete the table. TRIAL 1 TRIAL 2 TRIAL 3 Wt. of vinegar sample Vol. of vinegar…
A: % CH3COOH = Normality of NaOH * Volume of NaOH * Eq wt of CH3COOH * 100 / Weight of sample
Q: solubility
A: Borax : Na2B Na2B <-------> 2Na+(aq) + B^2-(aq) At Equilibrium : [Na+] = 2s and [B^2-] = s…
Q: Assuming that the concentration of EDTA for the experiment was 0.01 M in 20 ml tap water and the…
A: 1. For total Mg2+ and Ca2+ Volume of EDTA added during titrations are as follows: 1st titration:…
Q: Trials 1 2 3 Volume of aliquot of standard CaCO, solution 25.00 (ml) 25.00 25.00 Volume of titrant,…
A: Titer for trial 1 is determined as shown below.
Q: Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100…
A:
Q: Formula: ml base x N x meq. wt. x 100 %w/w = Sample weight A 4.59 ml sample of HCI, specific gravity…
A: 50.5ml of 0.9544N NaOH is required. HCl and NaOH reacts in 1:1 ratio. 4.59ml of sample was used…
Calculate for titer: (in mgCaCO3/mL EDTA)
Molarity of Trials:
Trial #1:
.01083 M EDTA
#2: .01069 M EDTA
#3: .01077 M EDTA
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- M 23 (H) Inorganic Analytical Chemistry pard My courses CHEM 23 (H) FS-AY:20-21 Week 4-5: Quantitative Analysis by Gravimetry and Titration Quiz 4 Qu 10 The 500.0-mg sample of impure Na2 CO3 (FM: 105.96) required 22.00 mL of the HCI standard solution (the obtained concentration of HCI from the previous question, problem 5: Titrimetry short answer type) for complete neutralization. ut of 1. Give the balanced chemical equation between the sample, Na2CO3 and the standard, HCI. 2. What is the mass (g) of Na, CO3 in the sample? 3. Calculate the % (w/w) purity of a 500.0-mg sample of impure Na2 CO3 Note: Type your solution here or upload its pic in Jpeg or pdf format. Another option is to send it to me via email (subject: Fam name-Quiz 4) or messenger, privately. Do not forget to box the final answer and write your name. В I 1.Table A: Standard NaCl used to make primary standard solution Mass of weighing bottle + NaC1 (g) 21.8720 Mass of weighing bottle after transfer (g) 21.772 Mass of NaCl used in solution (g) 0.6948 Purity of NaCl (%) 100.03 Table A: unknow used to make primary standard solution Mass of weighing bottle + unknow (g) 16.8777 Mass of weighing bottle after transfer (g) 16.20010 Mass of unknow used in solution (g) 0.6776 Purity of unknow (%) Table C: Titration of 25.00 mL aliquots of NaCl with AGNO3 Trial 1 Trial 2 Trial 3 Final Burette Reading (mL) 28.29 24.79 25.11 Initial Burette Reading (mL) 4.99 1.49 1.69 Volume Added (mL) 23.30 23.30 23.42 Table C: Titration of 25.00 mL aliquots of unknow with AGNO3 Trial 1 Trial 2 Trial 3 Final Burette Reading (mL) Initial Burette Reading (mL) 23.99 22.45 26.91 2.89 1.25 5.61 Volume Added (mL) 21.10 21.20 21.30MAX OF 15 MINUTES A solution contains NaOH (FM = 40), NaHCO3 (FM = 84), and NazCO; (FM = 106), either alone or in a permissible combination. Titration of a 50 mL portion to a phenolphthalein end point requires 16.3 mL of 0.100 M HCI. A second 50.0-mL aliquot requires 38.2 mL of the HCI when titrated to a bromocresol green end point. %3D %3D What is the % w/w composition of the following? Express answers in two decimal places. If the component is not present, write 0.00 in the answer box. NAOH: NazCO3: NaHCO3: 96
- Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration = 23.50mL Volume of 0.5N HCl consumed in blank titration = 44.50mL Percent purity (USP/NF) = Aspirin tablets contain NLT 90.0% and NMT 110.0% of the labeled amount of aspirin (C9H8O4) What is the calculated weight (in grams) of pure aspirin?..Given the following data Dissolved Oxygen Titration Data Trial 1 Preparation of titrant 0.4455 g NazS203•5H20 in 50.0 mL water Mass of water sample used (g) 5.21 g Initial mass of Na2S203 soln and Beral pipet(g) 12.40 g Final mass of Na2S203 soln and Beral pipet(g) 12.20 g MW of Na2S203•5H2O 248.11 g/mol MW of NazS203 158.11 g/mol MW of O2 32 g/mol Calculate the following: a) Concentration of Na2S203•5H20 in mol/g c) DO of sample (ppm) Final answer: 3 significant figuresConcentration 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
- 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 MinimizeIn this double titration experiment determining composition of soda ash, you are given the following data: M HCl titrant: 0.0501 M +/- 0.0507 Mass of soda ash sample, g: 0.2505 ± 2.0e-4 (Analytical Balance) Total volume of Sample Stock, mL: 75 ± 0.05 (100mL graduated cylinder) Volume of Sample Stock Aliquot, mL: 25 ± 0.3 Find the missing information. Show solutions3. sample of pure CaCO3 (MW 100.09) weighing 0.4148 g is dissolved in 1: 1 hydrochloric acid and the solution is diluted to 500 mL in a volumetric flask. A 50.0 –mL aliquot is withdrawn with a pipet and placed in an Erlenmeyer flask. The solution is titrated with 40.34 mL of an EDTA solution using Erichrome Black T indicator. Calculate the molarity of the EDTA solution.
- Data Table 3: Complexometric Titration of Soft Water 6ml of water used (1ml of buffer and 5ml of soft water) 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):The mass percent of Fe in an unknown salt sample was determined using both volumetric and gra vimetric titration. Ten determinations using both methods were performed. Volumetric(% of Fe): 24.22, 23.86, 24.07, 24.49, 24.69, 23.71, 24.28, 24.11, 24.26, 24.10 Gravimetric (% of Fe): 24.35, 24.26, 24.10,24.19, 24.18, 24.32, 24.11, 24.33, 24.17, 24.12 a. Do the two methods give similar standard deviations? b. Do the two methods give similar results for the mass percent of Fe at the 95% confidence level?The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…