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If I have a concentrated stock chemical at 4.4 Molar, and I need 350mL at 1.5 Molar, how do I make this?
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- Prepare the following solutions: 100.0 mL 0.0500 M stock Ca2+ solution 50.0 mL 0.0050 M working standard Ca2+ solution from 0.0500 M Ca2+Mass solute needed to prepare 0.500L of 0.2 M NaCO3 from a solid NaCO3 with a purity of 92.0wt%The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
- Consider the following scenario: After the first compound elutes off of the column, you collect multiple fractions without seeing the next compound begin to elute. What change might you want to make before you continue taking fractions?A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Show the clear and complete solutionWhat volume (in cm3) of 30 mass/mass%, ammonium solution is needed (with a density of0.892 g/cm3 ) to produce 1.0 dm3 of pH 11.0 solution?Kb = 1.8 x 10-5
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