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Explain which statement is correct concerning the resulting titration curve when a weak acid is titrated with a strong base?
A) The pH at halfway to the equivalence point is equal to the pKa of the weak acid
B) The pH after the equivalence point is determined using the Ka of the weak acid.
C) The pH of the solution before the addition of titrant is greater than 7.
D) The pH at the equivalence point is 7.00.
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Find the value of the equilibrium constant at each temperature you must first find the value of G0 at each temperature by using the equation G0 = H0 - TS0 For this reaction the values are H0 = +88.3 kJ/mol and S0= 151.3 J/mol*K
The dissociation pK for acetic acid is 4.76. Suppose that we dissolve a mole of this weak acid in 10L of water
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