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We have a 0.0100 M solution of ammonium acetate (Nh4C2H3O2), an ionic compound that dissociates completely in water. The ammonium cation is a weak acid (pKa=9.24) and the acetate anion is the conjugate base of acetic acid, another weak acid (pKa=4.76).
a.) Set up the problem by listing the reactions unknowns equations and knowns
b.) Calculate the concentrations of all chemical species present in the solution, and the pH.
60.0 mL of a 0.450 M solution is titrated with 0.570 M . Calculate the volume of required to reach the equivalence point.
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Determine the number of grams of sodium acetate and the amounts in mLs of 6.00M acetic acid that you would need to make 50.00mL of a sodium acetate/acetic acid buffer solution at the pH equal to 5.00 in order to make a final concentration of 0.05M..
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