3. Describe the preparation of 750mL of 6.00M H3PO4 (98g/mol) from a commercial reagent containing 85% (w/w) H3PO4 and having a specific gravity of 1.69.
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- 4. What volume of dilute nitric acid of density 1.11g/mL and 19% nitric acid by weight contains in 10g nitric acid. 5. Given 200cm3 of pure water at 40C, what volume of a solution of hydrochloric acid whose density is 1.175g/cm3 and containing 344.4% HCl by weight, could be prepared?6. How many grams of Na2CO3 are needed to prepare 500cm3 of a solution containing 10.0mg of CO32- per cm3?7. What volume of 0.300M H2SO4 is required to exactly neutralize 200mL of 0.500M NaOH?2NaOH + H2SO4 Na2SO4 + 2H2O(1a) Pure benzophenane freezes at 66.6 °C. A solution of 7.75 g of biphenyl (C12H10; molar mass = 154.2g/mol) plus 200.08 g of benzophenane froze at 59.9 °C. Calculate the Kf of benzophenane in °C*kg/mol. (b) An unknown solution with possible cations (Ag+, Hg22+, Pb2+) is treated with 6M HCl and a white precipitate forms. Hot water is added to the precipitate, and a white solid remains after filtration. The white solid is treated with aqueous NH3, and the precipitate turns grey or black. The resulting solution is treated with HNO3 and no precipitate forms. What cations can you determine to be present, absent or maybe present? Explain your reasonDescribe the preparation of 100 mL of 8.0 M H2SO4 from a concentrated solution that has a specific gravity of 1.84 and is 40% (w/w) H2SO4 (98.06g/mol).
- Stock phosphoric acid solution is 85% H3PO4 and has a specific gravity of 1.70 . Hence, the molarity of H3PO4 solution that is prepared by diluting 15.0 mL aliquot of H3PO4 stock solution to 135 mL H2O is?Perform the necessary calculations for the preparation of: d) 100 mL of sulfuric acid (98.08 g / mol) 0.1 N, whose label says 97.5% by weight and density 1.84 g/mL e) 300 mL of barium chloride at 5% p/V f) 150 mL of a 0.02 M NaCl solution, starting from a 0.1 M NaCl solutionExample: Calculation the weight of barium iodate Ba(IO3)2 if it dissolved in 500mL of distilled water (D.W) at 25 °C if M.wt of ppt = 487 g/mole and %3D Ksp= 1.57x10.
- How many moles of solute particles are present in 1.64 mL of 0.458 M K2SO4? (the answer is 2.25E-3 but i would appreciate some insight on what steps to take!)A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the osmotic pressure in atm.
- Assume you dissolve 30.0 g of cobalt sulfate heptahydrate (CoSO4.7H2O) in 500 ml of a 1.0 MH2SO4 solution. Calculate the following for CoSO4.7H2O in this solution:(The Specific Gravity of 1.0 M H2SO4 @ 20°C is 1.0814 g/ml.) Molality, Mole fraction and Weight percentagePrepare 0.1 M solutions of NaOH and 0.1 M ethyl acetate using high-purity distilled water. So, weight desired amount of NaOH and ethyl acetate and dissolved in dH2O to prepare stock solution in equal molarity. Mw (NaOH) = 40.0 g/mol , Mw (EtOAc)= 88.1 g/mol, Density(EtOAc): 0.898 g/cm3What weight of HCl is present in 30mL of hydrochloric acid of specific gravity 1.19 and contains 37.5% by weight of HCl?