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A student standardized her I2 solution by preparing a solution of 0.0450 g of ascorbic acid (vitamin C) in a 100 mL volumetric flask. She titrated several 10.00 mL samples of the Vitamin C solution and found an average of 24.95 mL of I2 solution was required to get to the end point. Calculate the molarity of the I2 solution
A piston has an external pressure of 8.00 torr How much work has been done if the cylinder goes from a volume of 0.130 liters to 0.450 liters.
The vapor pressure of pure ethyl bromide at this temperature is 400.0 torr. Assuming an ideal solution, what is the molecular mass of the compound?
Acetylene gas (C2H2) is produced as a result of the following reaction. CaC2(s)+2H2O(l) = C2H2(g)+Ca(OH)2(aq) . If 32.0 g of CaC2 are consumed in this reaction, how many moles of H2O are needed?
calculate the percentage of empty space in 1 mol of water at 25C. Obtain the density from the experiment " Some Measurements of Mass and Volume." The volume of a molecule of water can be taken as the sum of the volumes of the two hydrogen atoms.
Calculate the pH of a buffer solution prepared by dissolving 0.200 moles of benzoic acid (C6H5COOH) and 0.450 moles of sodium benzoate (C6H5COONa in enough water to make 1.00 L of solution
Calculate the pH at the equivalence point in titrating 0.120 M solutions of each of the following with 8.0* 10^-2 M NaOH
At 1 atm, how much energy (kJ) is required to heat 65.0 g of H2O(s) at -20.0 degrees C to H2O(g) at 135.0 degrees C?
What are the concentrations of each of the ions in a saturated solution of PbBr2, given the Ksp of PbBr2 is 2.1 x 10^-6?
The specific heats of ice and water are 2.09 and 4.184 J/g.°C, respectively. The heat of fusion for water is 334 J/g.
A sample of nitrogen gas in a 4.7-L container at a temperature of 28°C exerts a pressure of 3.6 atm. Calculate the number of moles of gas in the sample.
A solid block of exactky 100.0 cm 3 has a mass of 153.6g. Determine its density. Will the block sink or float on water?
What was the composition of the mixture of Mg and Zn expressed as percent by mass? If the volume of acid used was 100 mL, what were the final molar concentrations of MgSO4 and ZnSO4?
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