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Q: 0.00247
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0.7682 g MgCO3 is dissolved in 1000 mL of water, 50 mL of this solution is taken and titrated with EDTA. In titration, calculate the molar concentration of EDTA since 42.35 mL of EDTA is spent. (MgCO3: 84 g/mol).
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.The molarity of an EDTA solution is 0.0114 M. A 25.0 mL sample of water with unknown Ca+2 concentration is titrated with this EDTA solution and requires an average volume of 22.60 mL of EDTA. How many grams of CaCO3 is present per liter of water sample?
- For the determination of Ca in blood serum, 5 mL of a serum sample is taken and the Ca2 + in it is precipitated as CaC2O4. The precipitate is filtered, dissolved in acid and titrated with 0.001 M KMnO4 by heating. Calculate the Ca concentration in the sample since 4.94 mL of KMnO4 was used. A. 0.00135 B. 0.00247 C. 0.1135 D. 0.00563An EDTA solution was prepared by dissolving approximately 3 grams of Na2H2Y•H2O in sufficient water to give 1 liter of solution. This solution was then standardized against 50.00 mL aliquots of 0.004517 molar Mg2+. An average titration volume of 32.22 mL was required. Determine the molar concentration of EDTA.A 15.00 mL sample of hard water was titrated with a 0.0150 M EDTA solution. The titration required 26.72 mL of EDTA to reach the end point. What is the total hardness concentration of the water sample in ppm?
- Titration of 0.2342 g of pure Na,C,O, (134.0 g/mol) required 33.45 ml of KMNO, solution according to the chemical reaction: 4. 2MNO, +5C,0 +16 H* 2MN2+ + 10CO, +8H,O The Molarity of KMNO, solution would be: a. 0.01609 M b. 0.04020 M c. 0.02090 M d. 0.20140 M e. 0.12450 M Please fill in the space with one of the following characters ( a or b or c or d or e)0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate the percentage of 38.5 mL of 0.161 M titrant consumed in the titration (Fe: 56 g/mol). 25.4150.82C.76,23D.32,45A student wanted to determine the amount of NaOCI in a commercial bleaching solution. He diluted 2 g of bleach in a 100 ml volumetric flask. A 50 ml sample of the diluted bleach was mixed with excess acidified potassium iodide KI and a few drops of an indicator. The resulting solution was titrated with Na-S.O, solution. The titration required 17 mL of 0.05M Na,S,O, solution. The series of reactions that take place during this experiment: 21+OCI+ 2H1₂ + Cl + H₂O 1₂+28,0,³ →21+S,0,² a) Calculate the number of moles of OCI- in 50 mL diluted bleach and in 100 mL.
- 0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). At what volume (in mL) of EDTA added will the equivalence point be reached?To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.If 10.00 mL sample of 0.01 M standard Ca2+ solution is titrated with 9.8 mL of EDTA solution, what is the molarity of EDTA? (Ca: 40 g/mol)