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Calculate the volume of 0.0500 M EDTA needed to titrate 29.13 mL of 0.0598 M Mg(NO3 )2. Use a MW value in 4 decimal places.
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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 ___________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?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?
- A student titrated a 25.00 mL sample of water with 0.0200 M EDTA. The titration required 20.40 mL of EDTA. Calculate the ppm hardness in the water sampleMolarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?
- Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Mass of NaOCl in the diluted bleach titrated. ?In the titration of 25.00 mL of a water sample, it took 19.990 mL of 3.480x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures) Calculate the number of grams of…Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?
- Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. Calculate the molar concentration of the KMnO4 solution.Determine the molarity of the 10.00 mL standard EDTA solution titrated using 1.000 g zinc sulfate in 100 mL solution. (ZnSO4 = 161.47 g/mol ) 0.006193 M 0.6193 M 6.193 M 0.06193 MTitration of 0.2121 g of primary standard Naz2C204 (133.999 g/mol) required 21.66 mL of KMnO4 (153.034 g/mol) to reach the end point. 2- Calculate the molar concentration of KMNO4? 2 MnO, +5 C204² +16 H+ → 2 Mn2 10 CO2 +S H,0 1. O0.0146 2. 00.0292 3. O0.00731 4. 00.1462 Previous Next 4) へ hp 112 insert VAA f9 f8 f6 43 JOI & $4 % 7 80 LC %24