Present the calculations to determine the% of CaO in an unknown sample using the equation below for each of the replicates. Úse the value of 0.020 M as the average molarity of EDTA: 56.08g Ca0 1mol Cao 1 mol Cao 100.00 mL 11.6 mL (1.86 g)(0.020 M) 1 mol EDTA .46 g %Cao = 10.00 mL x 100
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Q: alculate the amount of manganese (54.94 g/mol) from a processed ore using the following data.
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A: Ppm is equal to mg/L Millimoles = molarity*volume (in ml) Milligrams= molar mass * millimoles
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A: Given data, Q7) Concentration of CoSO4 = 1.569 mg/mL Molar mass of CoSO4 = 155.0 g/mol Concentration…
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Q: 2) In order to determine the hardness of water, 100 mL sample is taken. After neutralizing the…
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Q: How much 0.0500 M EDTA is needed to titrate the Mg and Ca in a 0.2385-g sample that is 92.5%…
A: Given, Molarity of EDTA = 0.0500 M Mass of the sample = 0.2385 g Mass percent of dolomite = 92.5%…
Q: Titration of Ca2+ and Mg2+ in a 50.00 mL sample of hard water required 23.65 mL of 0.01205 M EDTA. A…
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Q: A 25.00 mL aliquot (a portion or part) of the standard Ca (II) solution (prepared by dissolving…
A: First we have to find the moles of Ca2+(aq) ion from 0.3139 g CaCO3. After finding the moles of…
Q: 20. Assume you are using 0.1 M EDTA to titrate a 0.2 M Ca* solution (25 mL) at pH 10.0. V molarity…
A: Calculation of no. of mol of Ca2+: n=Molarity×Volume=0.2 mol/L×25×10-3 L=5×10-3 mol Calculation of…
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Q: You took 25.00 mL of unknown water solution and titrated it with EDTA. The EDTA solution molarity…
A: Interpretation: a) To calculate g of CaCO3 in water if total hardness of water is due to CaCO3. b)…
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Q: The hardness of a water sample may be determined by titrating a 100-mL sample of water with 0.010 M…
A: The above question can be solved using the formula M1V1= M2V2
Q: The total concentration of Ca²+ and Mg²+ in a sample of hard water was determined by titrating a…
A: SOLUTION: Step 1: The concentration of magnesium ion is calculated as follows:
Q: A sample of pure CaCO3 weighing 0.3677g is dissolved in hydrochloric acid and the solution diluted…
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Q: A 50.00-mL sample of water containing Ca2+ and Mg2+ is titrated with 10.28 mL of 0.01001 M EDTA in…
A: Given: Volume of water sample = 50.00 mL Concentration of EDTA = 0.01001 M Volume of EDTA at 1st…
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A: The balanced equation for the titration reaction is: Mg2+(aq) + Y4-(aq) ⇌ MgY2-(aq) ; Keff = 1.7*108…
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Q: In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350x 10−3 M EDTA solution to…
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Q: which of the following is the amount of magnesium in the sample in ppm? (Mg:24 g/mol)
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Q: A water sample was tested for water hardness. A 50.00 mL sample, prepared and buffered to pH 10,…
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Q: A sample of pure CaCO3 weighing 0.2428g is dissolved in HCl and the solution diluted to 250ml in a…
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Q: A standard solution of EDTA (0.08 M) is being used to titrate 50 ml of a 0.04 M Ca 2+ solution.…
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A: Given:Ksp of MgCO3 = 3.5 x 10-8mol2L-2Ksp of Mg(OH)2 = 1.8 x 10-11mol3L-3
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A: The given data contains, weight of CaCO3 =0.4193 g volume of EDTA =23.62 ml
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- A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.A chemist is given a piece of limestone and told that 50.00% of the sample exists as calcium oxide (CaO). To analyze the sample, the chemist wants to dissolve a portion of the sample in 100 mL and then titrate an aliquot (10 mL) using 0.005300 M EDTA. How much sample (in grams) is needed if a titration volume of 25.00 mL EDTA is desired?A 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500 mL. A 25.00 mL aliquot was titrated with 0.0025 M KMnO4 spending a volume of 9.32 mL. Subsequently, a 25.00 mL aliquot was passed through a Walden reducer to later titrate it with the same permanganate solution, using a volume of 14.15 mL for the titration. Determine the percentage of Fe(III) in the sample and report it as % Fe2O3
- What is hardness of water? How can it be determined by using EDTA in a laboratory? Inan experiment to determine the hardness, a sample 100 ml of water required 15 ml of N/50EDTA. 100ml. of water after boiling for 15 minutes and making up to 100 ml again withdistilled water, required 8 ml of EDTA for titration. Calculate total, temporary and permanenthardness of waterMaria wants to determine the concentration of Calcium ions in water from their well. She used a 100.0 mL water sample, and its pH was adjusted to 10 and 3 drops of the indicator were added. She used 2.500 mL of 0.09945 M EDTA to reach the endpoint. What is the concentration (mg/L) of calcium ion in the sample? Identify the classification of water given the reference. Reference: 0 to 60 mg/L Ca is classified as soft, 61 to 120 mg/L as moderately hard; 121 to 180 mg/L as hard; and more than 180 mg/L as very hardA sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930M
- To a 50.00-mL aqueous solution containing Pb2+ is added a total amount of 5.000 mmol EDTA. The pH is made alkaline, and the excess EDTA is back-titrated with 0.0100 M Mg2+, requiring 15.2 mL. Calculate the molar concentration of Pb in the sample. A.0.100 M B. 0.0970 M C. 0.0486 M D. 2.94 x 10-3 MThe SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.
- For complexometric titration of Ca (II) ions in the shell of an egg sample weighing 59,427 g, the necessary processes were applied to the egg shells and a sample of 100 mL was prepared. From the prepared sample, 1 mL was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dripped on it. The prepared solution was titrated with 27.4 mL of EDTA solution set at 0.0097 M. Calculate the amount of calcium in the sample in CaCO3%. (Ca = 40g / mol, CaCO3= 100g / mol)A sample of Na2CO3 is known to contain inert matter and either NaOH or NaHCO3. In the potentiometric titration of a 0.225 gram sample with 0.100 N HCl, using a saturated calomel electrode and a hydrogen electrode, the following data were obtained (photo attached) Plot the titration graph and from it determine the nature and approximate composition of the sample. At what volume does the first equivalence point occur? ____ mL At what volume does the second equivalence point occur? ____ mLCalculate the alkaline strength of pearl ash ( impure potassium carbonate) in terms of percent K2O from the following data: Sample=0.3500 g; HCl used=48.03 m; NaOH used for back titration=2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4·H2O