show all work please QUESTION 16 A titration of 200.0 mL of 1.00 MH2A was done...
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Calculate the pH when 200.0 mL of a 1.00 M solution of H2A(Kal = 1.0 x 10-6, K22 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. 600.0 mL of 1.00 M NaOH A) 13.40 B) 11.70 C) 14.00 D) 10.00 E) none of these
Consider the titration of 100.0 mL of the weak diprotic acid H2A (0.10 M) with 0.20 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) 1. Before any NaOH is added 2. After 25.0 mL of 0.20 M NaOH is added 3. After 50.0 mL of 0.20 M NaOH is added 4. After 75.0 mL of 0.20 M NaOH is added 5. After 200.0...
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Calculate the pH when 200.0 mL of a 1.00 M solution of H2A(Kal = 1.0 104, K22 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. 3. 600.0 mL of 1.00 M NaOH A) 13.40 B) 11.70 C) 14.00 D) 10.00 E) none of these
Consider the titration of 100.0 mL of 0.200 M acetic acid ( Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a 0.0 mL pH= 50.0 mL pH = C 100.0 mL pH = 140.0 mL pH= C 200.0 mL pH = f 240.0 mL pH=
A 100.0-mL aliquot of 0.100 M diprotic acid H2A (PK1 = 4.00, PKa2 = 8.00) was titrated with 1.00 M NaOH. Find the pH at the following volumes of base added. a) 1 ml, b) 11 mL, c) 20 mL and d) 22 mL.
consider the titration of 100.0 ml of 1.00 M HCN with 1.00 NAOH solution. Find the pH of the soultion at the equivalence point. ka (HCN)= 4.0*10^-10
Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 10.0 mL pH = c. 60.0 mL pH = d. 80.0 mL pH = e. 110.0 mL pH = Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the...
Consider the titration of 100.0 mL of 0.75 M H3A by 0.75 M KOH for the next three questions. The triprotic acid has Ka1 = 1.0 x 10-5, Ka2 = 1.0 x 10-8, and an unknown value for Ka3. 1) Calculate the pH after 100.0 mL of KOH has been added. pH = Tries 0/45 2) Calculate the pH after 150.0 mL of KOH has been added. pH = Tries 0/45 3) The pH of the solution after 200.0 mL...
Calculate the pH at each of the following points along the titration of 25.0 mL of 0.185 M HNO2 with 0.185 M NaOH. [K, = 4.3x10-61 pka = -109(4.3x10-6 - 5136 5.36 +log 185/. 185 = 5. 4 5 20 0 5.0 odstoty D oonboe 3.1 HOMO 4 5: 2 . SI. OLD 0 mL of NaOH added pH = _ 8.5 mL of NaOH added pH = 12.5 mL of NaOH added pH = 22.0 mL of NaOH added...
Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 x 10–6, Ka2 = 1.0 x 10–10) is titrated with the following volumes of 1.00 M NaOH. 250.0 mL of 1.00 M NaOH Group of answer choices