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How many grams of water are contained in 2.78g og CaSo4*2H2O
A 15.01g sample of MgSO4*xH2O leave a residue of 6.01g upon heating. What is the value of x?
How many moles of barium metal react to produce 0.100mol of barium nitride? Hpw many moles of nitrogren gas react?
Ba(s) + N2(g) -> Ba3N2(s)
Ba(s) + N2(g) -> Ba3N2(s)
The below chemicals are added into a closed (no gas phase), perfectly
mixed vessel containing 1 litre of pure water, temperature remains constant at 25ºC.
Propionic Acid (CH3CH2COOH) = 0.03 mol
Sodium acetate (CH3COONa) = 0.02 mol
Sodium bicarbonate (NaHCO3) = 0.04 mol
Calcium carbonate (CaCO3) = 0.01 mol
Ammoniun Chloride (NH4Cl) = 0.02 mol
Ammonia (NH3) = 0.01 mol
Salt (NaCl) = 0.05 mol
NaOH = 0.02 mol
HCl = 0.0075 mol
1) 0.01 mol of hydrogen chloride (HCl) are added into the solution, calculate the new resulting
equilibrium pH.
2) After the addition of the HCl above the vessel is opened and left in contact with the
atmospheric air for a very long time. Assuming no liquid volume changes, calculate the new
equilibrium pH of the solution.
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
Equilibrium data for the temperature selected:
pKw = 13.669
pKProH = 4.733
pKAcH = 4.777
pKCO2 = 6.319
pKNH4+ = 8.979
KH,CO2 = 37.909 bar/M
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
mixed vessel containing 1 litre of pure water, temperature remains constant at 25ºC.
Propionic Acid (CH3CH2COOH) = 0.03 mol
Sodium acetate (CH3COONa) = 0.02 mol
Sodium bicarbonate (NaHCO3) = 0.04 mol
Calcium carbonate (CaCO3) = 0.01 mol
Ammoniun Chloride (NH4Cl) = 0.02 mol
Ammonia (NH3) = 0.01 mol
Salt (NaCl) = 0.05 mol
NaOH = 0.02 mol
HCl = 0.0075 mol
1) 0.01 mol of hydrogen chloride (HCl) are added into the solution, calculate the new resulting
equilibrium pH.
2) After the addition of the HCl above the vessel is opened and left in contact with the
atmospheric air for a very long time. Assuming no liquid volume changes, calculate the new
equilibrium pH of the solution.
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
Equilibrium data for the temperature selected:
pKw = 13.669
pKProH = 4.733
pKAcH = 4.777
pKCO2 = 6.319
pKNH4+ = 8.979
KH,CO2 = 37.909 bar/M
Concentration of CO2 in the atmosphere is 388 ppm (volumetric)
a gaseous organic compound X was burnt in the excess of oxygen.A 0.112 dm3 sample of X measured at s.t.p produced 0.88 grams of CO2 how many carbon atoms are present in one molecule of x ?
How to calculate the mass of calcium nitrate that can be made from *example* 3.15g *example* of pure nitric acid
suppose the assigned metal in hair is iron, and the mass of hair in a spiked sample is 1.217g.calculate the volume in µL of the stock Fe solution ( concentration 1008 mg/l) that we need to add to the hair sample?
When 83.5 moles of calcium acetate are dissolved in enough water to make 710.3 milliliters of solution, what is the molarity of acetate ions? Answer in units of M
Observe the following RXN:
CH4 + O2 --> CO + 2H2O
Carbon has a mass of 12 amu, Hydrogen 1 amu and Oxygen 16 amu.
If 16g of CH4 and 32g of O2 are reacted, how much CO is produced?
CH4 + O2 --> CO + 2H2O
Carbon has a mass of 12 amu, Hydrogen 1 amu and Oxygen 16 amu.
If 16g of CH4 and 32g of O2 are reacted, how much CO is produced?
heeey can someone explain to me how to do my hw :(
A. calculate the relative molecular mass of sodium sulfate, Na2SO4.
B. if 12 grams of Na2SO4 is dissolved in water and made up to a total volume of 500 cm3, calculate the concentration of the solution (as molarity i.e. mol dm^-3).
C. how many moles of sodium, Na, would be in 1 dm3 of the solution (b) above?
A. calculate the relative molecular mass of sodium sulfate, Na2SO4.
B. if 12 grams of Na2SO4 is dissolved in water and made up to a total volume of 500 cm3, calculate the concentration of the solution (as molarity i.e. mol dm^-3).
C. how many moles of sodium, Na, would be in 1 dm3 of the solution (b) above?
