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- A solution of I3- was standardized by titrating freshly dissolved arsenious oxide (As4O6, FM 395.683). The titration of 25.00 mL of a solution prepared by dissolving 0.3663 g of As4O6 in a volume of 100.0 mL required 31.77 mL of I3-. Calculate the molarity of the I3- solution. As4O6(s) + 6H2O ⇌ 4H3AsO3 H3AsO3 + I3- + H2O ⇌ H3AsO4 + 3I- + 2H+ a. 0.01657 M b. 0.02914 M c. 0.1166 M d. 0.0957 MWhat mass (in grams) of Na2S2O3 is needed to dissolve 0.44 g of AgBr in a solution volume of 1.0 L, given that Ksp for AgBr is 3.3×10−13 and Kf for [Ag(S2O3)2]3− is 4.7×1013?The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………
- A sample of impure KI weighing 0.600 g is dissolved in water, the solution acidified, and 25.00 mL of 0.0400 M KIO3 (an excess ) is added. The iodate is reduced to I2 and the iodide is oxidized to I, The I2 is boiled off, the solution cooled, and an excess of pure KI is added to react with the unused KIO3. The I2 produced is titrated with 40.38 mL of 0.1053 N thiosulfate. Write the equations for the reactions which occurred and calculate the percentage of KI in the sample.A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgOWhat is the dominant iron species in water samples ? What environmental factors may have contributed. why is it necesseyy to to investigate Fe3+ concentration and total Fe concentration dpeedtaely ? Why do we need to do the sample to determine total Fe concentration ? And how did then determine Fe2+ concentration?
- Around 15 g of Ba(NO3)2 can be dissolved in water. Calculate from that the Ksp for Ba(NO3)2A 0.7336-g sample of an alloy that contains copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc (At. Mass = 65.38 g/mol) in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and isolated as Zn2P2O7 (FM = 304.70g/mol), yielding 0.1163 g. The copper (At. Mass = 63.55 g/mol) in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN (121.63 g/mol), yielding 0.2383 g. Calculate the %w/w Zn and the %w/w Cu in the sample.What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in water and diluting to 725 mL? A) 0.276 and 0.828 B) 0.828 and 0.276 C) 0.276 and 0.276 D) 0.145 and 0.435
- 28a, solve the problem in the picturesA solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.Why we use ethanol to rinse the crystal instead of distilled water Better yield of crystal can be obtained if the alum solution is placed into refrigerator for a few days. Explain why. Solubility of alum, KAl(SO4)2•12 H2O in an aqueous solution at 0 degree Cecius is 114 g/L. In this experiment, calculate the weight of alum remain in the solution after crystallization completed. (Volume = 40 mL)
