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A solution containing HNO2 has pH=3.40 at equilibrium. Calculate the amount of HNO2 present in 575ml of this solution Ka=0.0004 answer is 0.01 g of HNO2
You perform column chromatography on a mixture of reaction products which shows two spots on TLC. However, under the column conditions you chose those two compounds do not separate.
A flask contains 0.500 mol of liquid bromine, rm Br_2. Determine the number of bromine molecules present in the flask.
What is the procedure for the extractions (to MAXIMIZE THE YIELD) and volumes? (i.e. How much water, NaCl, sodium bicarbonate and in what order)?
At a given temperature, 1.18 atm of F2 and 5.91 atm of Br2 are mixed and allowed to come to equilibrium. The equilibrium pressure of BrF is found to be 1.044 atm. Calculate Kp for the reaction at this temperature. F2(g) + Br2(g) 2 BrF(g)
Oleum or fuming sulfuric acid available commercially in concentrations ranging from 20 to 99.9% sulfur trioxide.
Calculate the volume of concentrated reagent required to prepare the diluted solutions indicated.
Deduce the structure of the molecule with the molecular formula C3H6 with a C13 NMR delta peak value of 27.8
Calculate the pH of the titration mixture after 10.0, 20.0 and 30.0 mL of base have been added. (the ka for acetic acid is 1.76 x 10^-5).
(the freezing point constant is 1.86 C/m). On the basis of these data, one can conclude that the nonelectrolyte has a molecular weight of?
A solution of acetic acid, HC2H3O2, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.39, what was the original concentration of the acetic acid? ___M
Calculate the equilibrium constant for the reaction. The standard enthalpy change delta H, for a strong acid-strong base reaction is -57.8k J. Determine the standard entropy change delta S for the reaction at 25 degrees C.
A process stream has 100 g/L NaCl in H2O. Prior to adding this to a batch bioreactor, the concentration must be reduced to 154 mM. The specific gravity of the solution is 1.075 at 20°C.
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