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The drug zalcitabine (also known as ddC) is a weak base with the following molecular structure. It has a pKb of 9.8. What is the percentage of the base is protonated in aqueous solution and contains 565mg/mL?
What characteristic absorption bands would you expect to find the infared spectrum of caffeine
What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Sn(s) and Pb2+(aq) to give Pb(s) and Sn2+(aq) Use the reduction potential values for Sn2+(aq) of -0.14 V and for Pb2+(aq) of -0.13 V
the thermite reaction is performed using 8.6g Fe2O3 and 1.8g powdered Al metal. which reactant is in excess and by how much?
When a base is added to an acid they neutralize each other except when they make a pH of 7, in this case find the exact amount for the two solutions below
How does solubility of polar and non-polar molecules in water set up cell membranes and disolve essential bio chemicals
A gaseous fuel mixture stored at 749 and 298 contains only methane (CH_4) and propane (C_3H_8) . When 11.3 of this fuel mixture is burned, it produces 776 of heat. What is the mole fraction of methane in the mixture
Still on Le Chatelier's principle, Ketones are known to be less reactive in aldol condensations.
What would be the molarity of a nonelectrolyte in an aqueous solution if it exhibited an osmotic pressure of 14060torr at 220C
In the carbonic acid equilibrum, what happened to the sized of the balloon upon addtion of more acid (HCl), and what happened to the sized of balloon upon addition of NaOH (Show the answer using equilibrum equation).
write the expression for the base dissociation constant for hydrazine, N2H4, a weak base. Hydrazine reacts with water to form the N2H5+ ion.
Draw the skeletal structure of the major organic product produced when 2-methylpropanoyl chloride reacts with 3-methylbutanoic acid in the presence of the weak base, pyridine.
What are the equilibrium concentrations of NH2OH (hydroxylamine), NH3OH+, and OH- in a 0.15 M solution of hydroxylamine (Kb=6.6*10^-9)? What is the pH of the solution
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