Consider the titration of 50.0 mL of 0.0500 M
C2H5NH2 (a weak base;
Kb = 0.000640) with...
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Chemistry
Consider the titration of 50.0 mL of 0.0500 MC2H5NH2 (a weak base;Kb = 0.000640) with 0.100 M HIO4. Calculatethe pH after the following volumes of titrant have beenadded:
(a) 0.0 mL
pH =Â Â
(b) 6.3 mL
pH =Â Â
(c) 12.5 mL
pH =Â Â
(d) 18.8 mL
pH =Â Â
(e) 25.0 mL
pH =Â Â
(f) 30.0 mL
pH =Â Â
Answer & Explanation
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3.7 Ratings (627 Votes)
pH of a Monoprotic Base This is a base in water so let the base be B and HB the protonated base HB there are free OH ions so expect a basic pH B H2O HB OH The equilibirum Kb Kb HBOHB let x be OH in solution in equilibrium due to sotichiometry HB x OH
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