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11 Dec 2019

2. Consider the triprotic acid, H3A, with the following acid dissociation contants: Ka1 = 1.5 x 10-5 , Ka2= 5.0 x 10-9 , and Ka3 = 5.0 x 10-12

a.) What is the pH of an aqueous solution of 0.200 M H3A?

b.) What is the pH of an aqueous solution of 0.200 M NaH2A?

c.) What is the pH of an aqueous solution of 0.200 M Na2HA?

d.) What is the pH of an aqueous solution of 0.200 M Na3A?

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Tod Thiel
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13 Dec 2019

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Related questions

Which of the following expressions hold for 0.10 mol/L Na2HA(aq). (HA2- is the doubly-ionized form of H3A, a weak triprotic acid.) a) [H2A-] = 2 [HA2-] = 3 [A3-] b)0.5 [Na+] = [H3A] + [H2A-] + [HA2-]+[A3-] c) [H+] = [H2A-] + 2 [HA2-] + 3 [A3-] + [OH-] d)[H+] = [H2A-] + [HA2-] + [A3-] + [OH-] E) Ka1=[H2A-][H+]/[H3A] F)Ka2=Kw/Ka1 G)[H+] + [OH-] = Kw

1)Diethylamine, (C2H5)2NH, is a weak base (pKb=3.16 at 25oC). What is the pH of 0.155 mol/L (C2H5)2NH(aq) at 25oC? Give your answer accurate to two decimal places.2)Which of the following expressions hold for 0.10 mol/L Na2HA(aq). (HA2- is the doubly-ionized form of H3A, a weak triprotic acid.) A) [H2A-] = 2 [HA2-] = 3 [A3-] B)0.5 [Na+] = [H3A] + [H2A-] + [HA2-]+[A3-] C) [H+] = [H2A-] + 2 [HA2-] + 3 [A3-] + [OH-] D)[H+] = [H2A-] + [HA2-] + [A3-] + [OH-] E) Ka1=[H2A-][H+]/[H3A] F)Ka2=Kw/Ka1 G)[H+] + [OH-] = Kw

1)Diethylamine, (C2H5)2NH, is a weak base (pKb=3.16 at 25oC). What is the pH of 0.155 mol/L (C2H5)2NH(aq) at 25oC? Give your answer accurate to two decimal places. 2)Which of the following expressions hold for 0.10 mol/L Na2HA(aq). (HA2- is the doubly-ionized form of H3A, a weak triprotic acid.) A) [H2A-] = 2 [HA2-] = 3 [A3-] B)0.5 [Na+] = [H3A] + [H2A-] + [HA2-]+[A3-] C) [H+] = [H2A-] + 2 [HA2-] + 3 [A3-] + [OH-] D)[H+] = [H2A-] + [HA2-] + [A3-] + [OH-] E) Ka1=[H2A-][H+]/[H3A] F)Ka2=Kw/Ka1 G)[H+] + [OH-] = Kw

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