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A student followed the procedure of this experiment to determine the percent NaOCl in a commercial bleaching solution that was found in the basement of an abandoned house. The student diluted 50.00 mL of commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL aliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na2S2O3 solution. A faded price label on the gallon bottle read $0.79. The density of the bleaching solution was 1.10 g/mL Calculate the number of moles of S2O32- ion required for the titration
How many grams of carbon dioxide would be obtained from the burning of 92g of ethanol in oxygen?
if you dissolve the weighed mass of zinc in water which had not been deionized, how would the volume of EDTA required to reach the indicator end-point
When 25.0 mL of 0.750 M CdCl2 is mixed with 40.0 mL of 0.120 M (NH4)2S, CdS precipitates from the solution. How many moles of CdS is formed.
Rubidium-87 decays by beta decay with a half-life of 4.9 x 10^10 yr. How many 87Rb atoms are in a moon rock sample that has a rubidium decay rate of 3500 disintegrations per hour
1. Using average bond enthalpies, predict which of the following reactions will be most exothermic:
Sodium lauryl sulfate can be prepared by replacing chlorosulfonic acid with another reagent. What could be used? Show the equations.
Based on the data for step 2 of the experiment, predict what would happen if you performed step 3 of the experiment (how many sets of three drops of each of the HCl and NaOH would be needed until the buffering capacity is lost for the two solution..
Calculate the solubility of copper (II) iodate in 0.56 M copper (II) nitrate. Ksp* is 7.4x10-8 M3.
One mole of N2, one mole of O2, and 0.5 mol of H2 are at 25 oC and 1 atm. The final total pressure of the mixture is 1 atm. Calculate delta_S on forming the mixture.
Calculate the molarity of a hydrochloric acid solution that is 18.25% HCl by mass and has a density of 1.20 g/mL.
The mass of the water in the inner bath is 1.60×10^3 g . The temperature of the calorimeter and its contents rises 2.84K as a result of this reaction. 1)Calculate the calorimeter constant.
Suppose that for the precipitation of the stock solution of borzac, the solid borax reagent is contaminated with a water-souble substance that does not eact with HCl.
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