As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTA b. Calculate the percent brucite (Mg(OH)2) content of rock B if it was titrated with 76.5 mL EDTA

As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTA b. Calculate the percent brucite (Mg(OH)2) content of rock B if it was titrated with 76.5 mL EDTA

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter19: Complex Ions

Section: Chapter Questions

Problem 51QAP: A child eats 10.0 g of paint containing 5.0% Pb. How many grams of the sodium salt of EDTA,...

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As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. Calculate the percent brucite (Mg(OH)2) content of rock B if it was titrated with 76.5 mL EDTA
As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTA
A sample of pure CaCO3 weighing 0.2428g is dissolved in HCl and the solution diluted to 250ml in a volumetric flask. A 50.00ml aliquot requires 42.74ml of an EDTA solution for titration. A 200ml sample of water containing Ca+2 is titrated with 16.38ml of the EDTA solution. Calculate the degree of hardness of water in ppm CaCO3.
Hardness in groundwater is due to the presence of metal ions, primarily Mg2+and Ca2+. Hardness is generally reported asppm (mg/L) CaCO3or mmol/L Ca2+. To measure water hardness, a sample of groundwater is titrated with EDTA, a chelating agent, in the presence of the indicator eriochrome black T, symbolized here as In. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2+and turns blue when Ca2+is removed. A 50.00-mL sample of groundwater is titrated with 0.0850M EDTA. Assume that Ca2+accounts for all of the hardness in the groundwater. If 10.10 mL of EDTA is required to titrate the 50.00-mL sample, what is the hardness of the groundwater in molarity Ca2+and in ppm CaCO3?
Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the volume of standard NaOH that reacted with iron :
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.32,45
Chromium(III) hydroxide, Cr(OH)3, is highly water insoluble. Its molar mass is 103.02 g/mol. a.) Write the chemical equation for dissolving Cr(OH)3 in water. b.) Calculate the mass solubility of Cr(OH)3 in pure water. c.) Calculate the mass solubility of Cr(OH)3 in a solution containing 0.221 M Cr(NO3)3(aq). d.) Calculate the mass solubility of Cr(OH)3 in 0.350 MM NaOH(aq).
0.7682 g MgCO3 is dissolved in 1000 mL water, 50 mL of this solution is taken and titrated with EDTA. Calculate the molar concentration of EDTA since 42.35 mL of EDTA is consumed in the titration. (MgCO3: 84 g / mol). A. 0.0054 B. 0.0216 C. 0.0108 D. 0.0432
From the water sample analysis: 40 mg/L Ca+2, 5 mg/L Mg+2, 10 mg/L K+, 10 mg/L SO4-2, and alkalinity which is equal to 122 mg/L as CaCO3. Calculate the TH, CH, and NCH. Also check the classification of water hardness of the water sample.
Calculate the mass of Na2S2O3•5H2O needed to prepare a 1.00-liter solution of 0.0700 M concentration. Write the net ionic balanced equation for the redox reaction of iodate and iodide in acidic medium forming iodine and water. This is the pre-titration reaction. Write the net ionic balanced equation of iodine and thiosulfate forming iodide and tetrathionate, S4O62-. This is the titration reaction. Write the overall balanced equation for reactions 2 and 3. What is the expected color at this endpoint? Write the balanced net ionic equation when ascorbic acid, C6H8O6, reacts with iodine to form dehydroascorbic acid, C6H6O6 and iodide in acidic medium. This is second pre-titration reaction for the analysis of Vitamin C.
To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.
Calcium in powdered milk is determined by dry ashing a 1.50-g sample and then titrating the calcium with EDTA solution; 12.1 mL is required. The EDTA was standardized by titrating 10.0 mL of a zinc solution prepared by dissolving 0.632 g zinc metal in acid and diluting it to 1 L (10.8 mL EDTA required for titration). What is the concentration of calcium in the powdered milk in parts per million? is the correct answer 2.89 ppm?