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A solution of ethanol (C2H5OH) in water is prepared by dissolving 88.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 300.0 mL of solution. What is the molarity of the ethanol in this solution?
The excess I3- was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?
SO3 can be produced in the following two-step process: FeS2 + O2 ---> Fe2O3 + SO2 , SO2 + O2 ----> SO3 Assuming that all the FeS2 reacts, how many grams of SO3 are produced when 20.0 g of the FeS2 reacts with 16.0 g of O2?
What is the molar mass of the unknown compound if the solution has a freezing point of -5 oC?
How many ml of a 2M HCl are required to neutralize 200 ml of a 0.4 M solution of NaOH?
Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO. The Ka for HClO is 2.9 x 10-8
Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa = 4.76) of 5:1? Enter answers with 2 decimal points.
calculate the number of moles of KOH in 5.5mL of a .36 M KOH solution. what is the pOH of the solution?
It takes 47.0 J to raise the temperature of an 9.00 g piece of unknown metal from 13.0rm ^circ C to 25.0^circ{C}. What is the specific heat for the metal?
2H2S (g) + 3O2 (g) → 2H2O (g) + 2SO2 (g) If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams.
A solution consisting of .200 mol of methylbenzene (C6H5CH3) in 250 g of nitrobenzene (C6H5NO2)freezes at .40 degrees celsius
Use the density of copper (8.95 g/cm3) and its molar mass (63.55 g/mol) to calculate an approximate atomic radius for copper.
12.5 g of KCl (MM = 74.55 g/mol) is dissolved in enough water to make 675 mL of solution. Calculate the molarity of the KCl solution.
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