PH = Pka1 + log ( [ HA-] /[H2A] )
= -log ka1 + log ( [ HA-] / [ H2A] )
8.43 = -log (4.65×10-6) + log ([HA-][H2A])
log ([HA-][H2A]). = 3.098
[HA-][H2A] = 103.098
= 1253.1411
[HA-]. = 1253.1411 [ H2A]
PH= Pka2+log ([A-][HA-])
8.43 = -log ka2 + log ([A2-][HA-])
log ([A2-][HA-]) = -1.3
[A2-] = 0.05011[HA-]
= 62.794[H2A]
Fraction of H2A = [H2A]÷ ( [ H2A] + [HA-] + [ A2-]
=[H2A] ÷( [H2A] + 1253.1411[H2A] + 62.794[H2A])
= 1÷( 1+ 1253.1411+ 62.794)
=7.593 × 10-4
Fraction of HA- = [HA-] ÷([ H2A]+ [ HA-]+[A2-])
= 1253.1411[H2A] ÷([H2A] +[1253.1411[H2A]+62.794[H2A])
= 1253.1411 ÷(1+1253.1411+62.794)
= 9.515×10-1
Fraction of A2- = [A2-] ÷ ([H2A]+[HA-] +[A2-])
= 62.794[H2A] ÷([H2A] +1253.1411[H2A] +[62.794[H2A])
= 62.794 ÷ (1+1253.1411+62.794)
=4.7 × 10-2
What fraction of piperazine (perhydro-1,4-diazine) is in each of its three forms (H.A, HA", A?) at...
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You have a 0.025 L solution of piperazine (perhydro-1,4-diazine), a weak dibasic base. The Ka values for its conjugate acid are 4.65*10-6 and 1.86*10-10 (in a solution with an ionic strength of zero). You would like to know the concentration of your solution and decide to titrate with HCl. You make a 0.10 M solution of the acid and use methyl orange as an indicator. You reach the endpoint after adding 54.16 mL of your HCl solution. (c) How many...
) is in each of its three forms (H acid dissociation constant values for piperazine are Ka 4.65x10-6 and Ka2 1.86 10-0 Number H.A Number α= HA Number
Dont need (a) or (b) thank you
You have a 0.025 L solution of piperazine (perhydro-1,4-diazine), a weak dibasic base. The K, values for its conjugate acid are 4.65*10 and 1.86*10-10 (in a solution with an ionic strength of zero). You would like to know the concentration of your solution and decide to titrate with HCl. You make a 0.10 M solution of the acid and use methyl orange as an indicator. You reach the endpoint after adding 54.16 mL...