Calculate the final molarity of H2O2H2O2 if 5.1 mL5.1 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.1 mL5.1 mL of a starch-iodide solution.
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Calculate the final molarity of H2O2H2O2 if 5.1 mL5.1 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.1 mL5.1 mL of a starch-iodide solution.
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- Calculate the final molarity of H2O2H2O2 if 5.9 mL5.9 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.9 mL5.9 mL of a starch-iodide solution. final [H2O2]=[H2O2]= MM Calculate the final molarity of H2O2H2O2 if 1.6 mL1.6 mL of the 3.0% w/w H2O23.0% w/w H2O2 solution is diluted with 3.4 mL3.4 mL water, then added to 5.0 mL5.0 mL of a starch-iodide solution. final [H2O2]=[H2O2]= M(a) What is the molarity of a solution made by dissolving 10 moles of sucrose, C12H22O11, in 10L of water? (b) How much boric acid (H3BO3), in grams, is needed to be dissolves in 300.g of water to make a 1.50m aqueous H3BO3 solution? The molar mass of H3BO3 is 61.83g/mol. (c) How much aluminum sulfate (Al2(SO4)3) in moles, is needed to be dissolved in 500g of water to make a 1.0m aqueous Al2(SO4)3 solution?1. Calculate the normality of 0.321 g sodium carbonate (106.0 g/mol) when it is mixed in a 250 mL solution. 2. What is the normality of 0.0521 M H3PO4? 3. A12.5-mL portion of a base solution of an element from group 2A is diluted to 500 mL; the resulting concentration of this solution is determined to be 0.125 M. What is the normality of the original solution. 4. A sample of USP-grade citric acid (H3C6H5O7, three titratable protons) is analyzed by titrating with 0.1087 M NaOH. A 0.2678-g sample requires 38.31 mL of the titrant for titration. A. What is the normality of the titrant? B. What is the stoichiometric relationship between the analyte and the titrant? C. How many moles of the titrant were consumed to react with the analyte? NOTE: please include the given, the unknown, the chemical reaction, the calculation process, and the final answer with the proper number of significant figures.
- Calculate the molar concentration of a thiosulfate solution from the following information:A 40.-mL aliquot of a 0.00653 M KIO3 solution is added to a flask containing 2 g of KI and 10 mL of 0.5 M H2SO4. The resulting solution is titrated to a starch endpoint with 38 mL of the thiosulfate solution.In standardizing a solution of NaOH (40 g/mol) against 1.431 g of KHP (204.22 g/mol) the analyst uses 35.50 mL of the alkali and has to run back with 8.25 mL of acid (1 mL=10.75 mg NaOH). What is the molarity of the NaOH solution?What is the concentration of Cu2+ in a solution that has been prepared by diluting 1 mL of 0.1 M Cu(NO3)2 to 50 mL?
- What volume of 0.00945 M solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a concentration of H2SO4 of 1.23 x 10^-4 M?10 mL of 0.6M NiSO4 is mixed with 20 mL of 0.3 M CuSO4 . calculate the molarity of Ni2+, Cu2+ and SO42- ions present in solutionHow many grams of NaHCO3 (baking soda) would you need to neutralize 675 mL of battery acid (H2SO4, 6.00 M) that has been spilled on your garage floor? Assume that the concentration of the battery acid is 12 molar. 340. g 17.0 g 680. g 170. g 19.0 g
- When 3.5 g of CaF2 (an insoluble salt, Ksp = 3.9 X 10-11) is added to water to make 200. mL of solution, what is the concentration of calcium ions in the resulting solution?A sample of CaCO3 (molar mass=100.1) weighing 0.4856 g is dissolved in HCl and the solution diluted to 500.0 mL in a volumetric flask. A 25.00-mL aliquot requires 21.37 mL of an EDTA solution for titration. How many grams of Na2H2Y.2H2O (molar mass=372.2) are required to prepare 500.0 mL of this solution.what is the molarity of a solution that results from dissolving 5.4 g of a compound with FW 169.51 into a total volume of 853 mL? (Give your answer in units of M, with two places after the decimal point.)