Problem: In a 0.050 M solution of a weak monoprotic acid, [H  +] = 1.8 x 10 –3 . What is the Ka? (A) 3.6 x 10 –2 (B) 9.0 x 10 –5 (C) 6.7 x 10 –5 (D) 1.6 x 10 –7

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In a 0.050 M solution of a weak monoprotic acid, [H  +] = 1.8 x 10 –3 . What is the Ka?

(A) 3.6 x 10 –2

(B) 9.0 x 10 –5

(C) 6.7 x 10 –5

(D) 1.6 x 10 –7

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