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 =  



(b) 6.3 mL

pH =  



(c) 12.5 mL

pH =  



(d) 18.8 mL

pH =  



(e) 25.0 mL

pH =  



(f) 30.0 mL

pH =  

Answer & Explanation Solved by verified expert
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    See Answer
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