Ag+ , K+ , Pb2+, Zn2+ : Classify the Bronsted-Lowry acidity of these cations
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Ag+ , K+ , Pb2+, Zn2+ : Classify the Bronsted-Lowry acidity of these cations
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- Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when half of a solution of acetic acid is dissociated to acetate (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76Bicarbonate/carbonic acid buffer in blood is an example of an equilibrium reaction that is meant to be very insensitive to change. How does the bicarbonate/carbonic acid buffer re-establish equilibrium if acidity increases? How does the bicarbonate/carbonic acid buffer re-establish equilibrium if alkalinity increases?Indicate the ionic species of phosphoric acid that predominates at pH 4, 8, and 11.
- determine the pKa of the acid and ph of the buffer sol'n of a buffer mixed with 0.1 M tris and 0.5 M chloine salt having dissociation constant of 1.072x10^-6.Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when the ratio of acetic acid to acetate is 10 to 1 (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76For each of the following reactions, give a balanced net-ionic equation. Sulfate Ion a) MgSO4 + H2SO4 b) MgSO4 + BaCl2 Sulfite Ion a) Na2SO3 + H2SO4 b) Na2SO3 + BaCl2 c) BaSO3 + HNO3 Iodide Ion a) NaI + NaOCl b) NaI + AgNO3 c) AgI + NH3 d) NaI + H2SO4