Asked by Sally Perez
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of a monoprotic strong acid HX. (a) How many moles of HX have been added at the equivalence point? (b) What is the predominant form of B at the equivalence point? (c) What factor determines the pH at the equivalence point? (d) Which indicator, phenolphthalein or methyl red, is likely to be the better choice for this titration?
Answers
Answered by
DrBob222
a. moles HX added = M x L.
b. B + HX ==> BH^+ + X^-
c. The hydrolysis of the salt BH^+. Said another way, the strength of BH^+ as an acid.
d. Phenolphthalein changes color at pH about 9. Methyl red changes color about 5. Which do you think?
b. B + HX ==> BH^+ + X^-
c. The hydrolysis of the salt BH^+. Said another way, the strength of BH^+ as an acid.
d. Phenolphthalein changes color at pH about 9. Methyl red changes color about 5. Which do you think?
Answered by
serjon
a. 2.7 x 10 -3 moles or 0.0027
b. BH + (aq)
c. Already given.
d. phenolphthalein
b. BH + (aq)
c. Already given.
d. phenolphthalein
Answered by
Diggity dogg
hi to you. is this right?
Answered by
Boxer Boy
c. is actually methyl red
Answered by
Allison
For c it is both the Ka for BH^+ and concentration of BH^+ to determine pH at the equivalence point.
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