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A powder contains FeSO4·7H2O (molar mass = 278.01 g/mol) among other components. A 3.585-g sample of the powder was dissolved in HNO3 and heated to convert all iron to Fe3 . The addition of NH3 precipitated Fe2O3·xH2O which was subsequently ignited to produce 0.350 g of Fe2O3. What was the mass of FeSO4·7H2O in the 3.585-g sample?
0.250 g of a binary unknown acid, HX, requires 31.96 mL of a 0.09668M NaOH solution when titrated. What is the identity of the unknown acid.
Calculate the pH during the titration of 20.00 mL of 0.1000 M hydrazine N2H4(aq), with 0.1000 M HCl after 20.25 mL of the acid have been added. Kb of hydrazine = 1.7 x 10-6
Write down the electron configurations for C2 and F2. What is the bond order for each? Which one is likely to have larger bond dissociation energy.
how many whole drops (.05 mL/drop) of 6 M HCl are required to dissolve the calcium carbonate? b) What is the Ca concentration when this is dissolved and diluted to 100.00mL
Calculate the ratio of the hydronium ion in acid rain to that in normal rain.
Although the aluminum cylinder is a solid (and, therefore, is quite in-compressible), it actually contains quite a bit of empty space.
Using Henry's Law to calculate gas solubility If air contains 78% N2 by volume, what is the solubility of N2 in water of 25oC and 1 atm (Henry's constant kH for N2 in H2O at 25oC = 7 x 10-4 mol/L.atm)?
How many moles of HNO3 are present in 35.0 mL of a 4.50 M solution of nitric acid?
When 0.78 g of an unknown gas in contained solely in a 560 mL container, the pressure is 780 Torr at 5 degrees Celcius. What is the molar mass of the gas in grams/mole?
Phosphorus-32 has a half-life of 14.0days . Starting with 6.00g of 32p , how many grams of phosphorous will remain after 42.0days.
The piston is then moved in and the heat rejected by the air reversibly at constant pressure until the volume is= initial volume. compute The net heat flow and the overall change in entropy?
Nitrogen and hydrogen gases react to form ammonia gas as follows: N2(g)+3H2(g)-->2NH3(g) At a certain temperature and pressure, 1.7 L of N2 reacts with 5.1 L of H2. If all of the N2 and H2 are consumed, what volume of NH3(g) is produced at the sam..
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