arsenic acid (H3AsO4) is a triprotic acid with a Ka1=5E-3 Ka2=8E-8 and Ka3=6E-10. calculate [H+], [OH-], [H3AsO4], [H2AsO4-][HAsO4 2-], and [AsO43-] in a 0.20 M arsenic acid solution.
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Arsenic acid (H3AsO4) is a triprotic acid with Ka1=5e-3, Ka2=8e-8, and Ka3=6e-10?
ca 2. What is the charge balance for an aqueous solution of arsenic acid, H3AsO4, in which the acid can dissociate to H2AsO4 , HASO4+-, and AsO4”. a) [H+] = [OH-] + [H2AsO4] + 2[HASO42-] + 3[AsO43-] (b) [H+] = [OH-] + [H2AsO4] + [HASO42-] + [AsO43-] c) [H+] = 2[OH-] + 2[H2AsO4] + 2[HASO42-] + 2[AsO43-] d) [H3AsO4) = 2[H2As04] + 2[HAsO42-] + 2[AsO4?]
Calculate the pH of a 0.100M solution of arsenic acid, H3AsO4. Triprotic Acids Formula M.W. g/mol Ka1 pKa1 Ka2 pKa2 Ka3 pKa3 Arsenic H3AsO4 141.94 5.5*10–3 2.26 1.7*10–7 6.77 5.1*10–12 11.29
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2620 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M
Calculate the pH and the equilibrium concentrations of H2AsO4-, HAsO42- and AsO43- in a 0.2380 M aqueous arsenic acid solution. For H3AsO4, Ka1 = 2.5×10-4, Ka2 = 5.6×10-8, and Ka3 = 3.0×10-13 pH = [H2AsO4-] = M [HAsO42-] = M [AsO43-] = M
Part A Arsenic acid (H3ASO4) is a polyprotic acid with Ka1 = 5.5x10-3, Ka2 = 1.7x10-7, and Ka3 = 5.1*10-12 Which statement describes best the pH of a 0.010 M solution of this acid. (Hint: Start with calculating the pH as if this were a monoprotic acid.) O The value of pH is somewhat higher than 2.13. O The value of pH is somewhat lower than 2.13. O The value of pH is somewhat higher than 6.65. The value of...
The triprotic acid H3A has ionization constants of Ka1=5.37×10−3 , Ka2=4.31×10−6 , and Ka3=1.04×10−11 . Calculate the H+ concentration and the ratio [H2A−]/[H3A] for a 0.0170 M solution of NaH2A . [H+]= [H2A−]/[H3A]= Calculate the H+ concentration and the ratio [HA2−]/[H2A−] for a 0.0170 M solution of Na2HA . [ H + ]= [HA2−]/[H2A−]=
-The triprotic acid H3A has ionization constants of Ka1 = 4.9× 10–2, Ka2 = 6.0× 10–6, and Ka3 = 2.0× 10–13. Calculate the following values for a 0.0700 M solution of NaH2A (H+)=? (H2A-)/(H3A)=? -Calculate the following values for a 0.0700 M solution of Na2HA. (H+)=? (HA2-)/(H2A-)=?
A triprotic acid, H3A has the following Kas: Ka1 = 4.22 x 10-4 , Ka2 = 7.51 x 10-8 and Ka3 = 7.51 x 10-15. What is the Kb of H2A-? QUESTION 5 1 points Save Answer A triprotic acid, H3A has the following Kas: Ka1 = 4.22 x 10-4, Ka2 = 7.51 x 10-8 and Ka3 = 7.51 x 10-15. What is the Kb of H2A?
Arsenic Acid (H3AsO4) has the ability to act as a trip as the ability to act as a triprotic acid. Calculate the equilibrium concentration of all possible species in a 0.483 M arsenic acid solution. The Kal = 6.0 x 10-3, K2 = 1.0 x 10-7, and Ka3 = 3.2 x 10.
Consider a triprotic acid, H3A, with the following Ka’s: Ka1 = 2.4 x 10-3, Ka2 = 3.5 x 10-7, Ka3 = 1.6 x 10-11. What is the Kb3 value?