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A 5.00-mL aqueous suspension of elemental selenium was treated with 25.00 mL of ammoniacal 0.0360 M AgNO3. After the reaction was complete, nitric acid was added to dissolve the AgSO3 but not the AgSe. The Ag+ from the dissolved Ag2SeO3 and the excess reagent required 16.74mL of 0.01370 M KSCN in a Volhard titration. How many milligrms of Se were contained in each milliliter of sample?
The absorbance of solutions containing Cr as dichromate Cr2O7-2 in 1.0M H2SO4 were measured in a 5cm cell. The following results were obtained
Calculate the osmotic pressure (in torr) of 5.48 L of an aqueous 0.136 M solution at 25 celsius if the solute concerned is totally ionized into three ions (for example, it could be Na2SO4 or MgCI2).
The mass of a cube of iron is 392 g. Iron has a density of 7.87 g/cm3. What is the mass of a cube of lead that has the same dimensions?
State what are the most common agents in polymer degradation
Dibutyl ether and 1 -butene can be formed as by products in this reaction. explain how they are removed by sulfuric acid.
Which of the following is a neutralization reaction?
C12H22O11(aq) + 3 O2(g) 2 H3C6H5O7(aq) + 3 H2O(l) Determine the mass of citric acid produced when 4.60 mol C12H22O11 is used.
The radioisotope iodine-131, used to image the thyroid, has a half-life of 8.0 days What fraction of iodine-131 remains in the body after 3.0 days?
What happens to the solubility of an ionic compound as ionic strength of the solution increases up to ~0.5 M)? Why is there a correlation between the solubility of an ionic compound and the ionic strength of the solution?
1.50 mol of helium gas in a cylinder is held at a volume of 22.4 L by a piston at 273K and 1.00 atm. Heat is supplied to the system to double the volume and temperature of the gas while maintaining the internal pressure at 1.00 atm.
A groundwater sample is taken from a geologic formation containing various carbonate minerals (e.g., CaCO3, MgCO3, CaCO3•MgCO3, etc.) without exposing the water sample to the atmosphere.
empirical formula for 2.80 g nitrogen and 8.00 g oxygen. what is the molecular formula empirical formula of NH2Cl, molar mass = 51.5 g/mol
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