Consider the titration of a 26.0-mL sample of 0.175 M CH3NH2
with 0.155 M HBr. (The...
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Chemistry
Consider the titration of a 26.0-mL sample of 0.175 M CH3NH2with 0.155 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.)
A. Determine the initial pH.
B. Determine the pH at 6.0 mL of added acid.
C. Determine the pH at one-half of the equivalence point.
D. Determine the pH after adding 4.0 mL of acid beyond theequivalence point.
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A For initial pH Dissociation of base CH3NH2 H2O CH3NH3 OH We make our ICE table CH3NH2 CH3NH3 OH I 0175 M 0 0 C x x x E 0175 x x x Now with the definition of constant Kb CH3NH3 OH CH3NH2 44 x 104 x2 0175 x Isolating for x x OH 000855772 M Calculating pOH and pH pOH log000855772 20676 pH 14 20676 119323 B When
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