0.0520

Consider the titration of a 40.0 mL of 0.211 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH.     c. How many mL of the LiOH would be required to reach the halfway point of the titration?   d. What is the pH of the solution at the equivalence point?   e. What would be the pH of the solution after that addition of 100.0 mL of LiOH?

Determine the pH at the point in the titration of 40.0 mL of 0.200 M HNNH2 with 0.100 M HNO: after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. = 3.0 x 10-6 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x]

Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C₁H₁N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH = pH = pH = 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect

In the titration of a 25.0-mL sample of 0.145 M HCOOH with 0.122 M NaOH, where K, HCOOH = 1.8x10-4 %3D the volume of NAOH added at one-half the equivalence point is about 27.4 mL O the volume of NaOH added at one-half the equivalence point is about 7.45 mL O the volume of NaOH added at one-half the equivalence point is about 12.6 mL O the volume of NaOH added at one-half the equivalence point is about 14.9 mL

Calculate the pH at the given points in the titration between 100.0 mL of 0.05000 m NH3 (Kb = 1.8 x 10-5) after adding the following volumes of 0.100 m HCI: 50.00 mL HCI

12.0 10.0 8.0 A pH 6.0 4.0 2.0 0.0 C 0 5 10 15 20 25 30 mL of 0.1 M NaOH The graph above shows the titration curves of four monoprotic acids of varying strengths. All of the acids start out at 0.1 M concentration and 25.0 mL volume. Choose all of the correct statements about these titration curves from the choices below. The titration curve labelled "D" is generated by the strongest acid in the series. In the curves shown above the stronger the acid the less NaOH required for neutralization. The stronger the acid the more important is the pKa of the Indicator used for titration. The Ka of the acid which generates curve "C" is about 103 The weaker the acid the lower the pH of the neutralization point. The acid which generates curve "D" has the highest neutralization-point pH in the series.

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