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Consider the titration of 52.0 mL of 1.2 M NaOH with 1.0 M HCl. Find the pH at all the following points.
A). At the start of the titration. I know this answer is 14.08
B). At the equivalence point.
C). After the addition of a large excess of acid (in comparison with the acid volume needed to reach the equivalence point).
D). Tell how many milliliters of acid are required to reach the equivalence point.
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An equilibrium mixture for the reaction above contains [H2] = 1.00 M, [N2] = 1.50 M, and [NH3] = 2.00 M. What is the value of the equilibrium constant, Kc, for the reaction?
Calculate the expectation values for a particle in the state n = 5 moving in a one-dimensional box of length 2.48×10^(?10)m If someone can just help me out with the set up of the problem thatd be helpful.
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calculate the ph of buffer solution made from .20 M HC2H3O2 and .050 M C2H3O2 that has an acid dissociation constant for HC2H3O2 of 1.8*10-5.
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