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A sample of KHP weighed 1.126 g. Titration of this KHP required 20.19 ml of base (NaOH). What is the molarity of the base?
What volume will 1.56 liters of a gas at 27°C and 745 mmHg of pressure occupy at 100°C and 700 mmHg of pressure?
A student wants to prepare a dilute solution of iron (III) solution, . The student is provided with a stock solution of 0.800 +/- 0.001 M and a 100.00 +/- 0.008 mL volume trick flask since the experiment trquires about 80 mL of the dilute iron (II..
Calculate the volume of glacial acetic acid (17.6M) and eight of sodium acetate (mm=82.03) that is required to make 102 mL of 0.2M buffer at ph 4.85. The Ka of acetic acid is 1.4*10^-5.
An empty aerosol can at 25 degree celcius still contains gas at 1.00 atmosphere pressure. If an empty can is thrown into a 488.2 degree celcius fire, what is is the final pressur in the heated can.
what is the energy of a single UV photon and a mole of UV photons having a wavelength of 25 nm?
Assuming the kinetics of teh microorganisms enzymatic action is responsible for the rate of decay
A 26.0-g sample of ice at -11.0°C is mixed with 123.0 g of water at 90.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
What is the molarity of a solution of 14.0 g NH4Br in enough H2O to make 150 mL of solution?
A saturated solution of CaF2 had a calcium ion concentration of 2.20 x 10^-4 M. What is the Ksp for CaF2?
A 24.7 g sample of pure iron at 61°C is dropped into 99 g of water at 25°C. What is the final temperature of the water-iron mixture?
The vapor pressure of benzene is 53.3 kPa at 60.6°C, but it falls to 51.5 kPa when 19.0 g of a nonvolatile unknown organic compound is dissolved in 500 g of benzene. Calculate the molar mass of the compound.
If you have 400mL of .5 M NH3, how many moles of .47 M HCl must be added to the ammonia solution to reach the equivalence point.
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