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A 24-hour urine specimen was diluted to 2.000 L. After the solution was buffered to pH 10, a 10.00-mL aliquot was titrated with 27.32 mL of 0.003960 M EDTA. The calcium in a second 10.00-mL aliquot was isolated as CaC2O4(s) redissolved in acid, and titrated with 12.21 mL of the EDTA solution. Assuming that 15 to 300 mg of magnesium and 50 to 400 mg calcium per day are normal, did this specimen fall within these ranges?
What is the total mass of AlCl3 in this sample? b. How many moles of AlCl3 are in this sample?
What would account for the smaller amount of napthalene collected. Mothballs in a closet gradually disappear over time. What happens to this material
A 4.0L sample of air collected at 298 K and then cooled to 278F while held at constant pressure. What is the new volume of the air
Predict the electronic configurations of (a) the benzen anion, (b) the benzene cation. Estimate the pi-electron binding energy in each case within the Huckel Approximation.
Epsom Salts is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for epsom salt can be written as MgSO4* X H2O
In an equilibrium mixture of the three gases, the partial pressures of SO2Cl2 and SO2 are 3.31 atm and 1.59 atm, respectively. What is the partial pressure of Cl2 in the equilibrium mixture?
Determine the oxidation state for the following element in the compounds indicated;sulfur in H2SO4,nitrogen in NO2
If the freezing point depression of water is -1.86 degrees C/M, what would be the freezing point of this solution
Question- What is the density (in g/L) of a sample of nitrogen gas that occupies a volume of 7.04L at a pressure of 4.02 atm and a temperature of 33.6oC
The complex ion Co(H2O)6(2+)(aq) is pink when placed in solution. Addition of chlorine ions creates an equilibrium with CoCl6(4-) in the solution, which is blue in color.
A 500mL solution contains 1.68g NH3 and 4.05g (NH4)2SO4. How many mL of 12M HCl is needed to change the pH to 9.00?
Problem- Identify the neutral element represented by this excited-state electron configuration, then write the ground-state electron configuration for that element.
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