Answer : option (b) CH3 COO-
Reaction is :
CH3COOH + NaOH ----> CH3 COO- (aq) + Na+ (aq) + H2O
Which of the following species is present in the solution at the equivalence point of the titration of acetic acid...
Species Present in Regions of the Titration Curve List the major species present before any NaOH is added (i.e. start of the titration) The major species may be ions and/or molecules. Include spectator ions. % & BI U XX, 12 List the major species present in the buffer region * BI U x' x 12 List the major species present at the equivalence point % B I U xº x, 12 List the major species present beyond the equivalence point...
Find Pka value and equivalence point for each :) Titration of Acetic Acid with Sodium Hydroxide PH 0 0.1 0.2 0.3 04 Volume NaOH added 0.5 0.6 Titration of Selenious Acid with Sodium Hydroxide PH + NO R 0.1 0.2 0.3 0.4 Volume NaOH added (L) 0.5 0.6 Titration of Selenious Acid with Sodium Hydroxide PH 0.1 0.5 0.6 0.2 0.3 0.4 Volume NaOH added (L)
At the equivalence point of a titration of HOAc (acetic acid, pKa = 1.76 x 10-5) with NaOH, the species present of OAc" and H20. If the concentration of OAc at the equivalence point is 0.50 M, what is the pH of the solution? Remember that Kb x Ka = 10-14 and that the OAc will react with water as follows: OAC- + H20 --> HOÀc + OH- . 1 4.77 2. 10.23 3 5.68 4. 9.23
What is the pH at the equivalence point in the titration of a 29.4 mL sample of a 0.403 M aqueous acetic acid solution with a 0.386 M aqueous sodium hydroxide solution? What is the pH at the equivalence point in the titration of a 29.4 mL sample of a 0.403 M aqueous acetic acid solution with a 0.386 M aqueous sodium hydroxide solution?
In the titration of acetic acid (CH3COOH) and sodium hydroxide (NaOH), what are the major sepcies present at the following points? a) Before any NaOH is added (at the start of the titration). b) In the buffer region. Are there any spectator ions? c) At equivalence point. What is equivalent at this point? What has been used up? Are there any spectator ions? d) Beyond equivalence point. What has been added since the equivalence point? Has anything reacted further since...
Titrations 10. Calculate the pH at the equivalence point for the titration above of Sun acid (K=1.8x105) titrated with 0.2M sodium hydroxide. oint for the titration above of 50mL of 0.2M acetic 11. Sketch the titration curve when 50mL of 0.2M acetic acid (K 1.8x105) titrated with 0.2M sodium hydroxide.
Assuming that Ka is 1.85 *10-5 for acetic acid, calculate the pH at one-half the equivalence point and at the equivalence point for titration of 50mL of 0.100M acetic acid with 0.100M NaOH.
Answer the following questions for titration of 10.00 mL of a hypochlorous acid solution with a 0.09975 M sodium hydroxide. 1. If 20.05 mL of the sodium hydroxide solution were required to reach the endpoint in the titration, what was the original concentration of the hypochlorous acid solution? 2. What was the initial pH of the hypochlorous acid solution (before any sodium hydroxide was added)? 3. What was the pH in the titration after addition of 4.01 mL of NaOH?...
1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 2. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid that has been titrated to its endpoint using NaOH, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 3. What pH did you...
Consider a titration of 25.00 mL Chloroacetic Acid solution [ka=1.4x10^-3] with 0.1202 M solution of sodium hydroxide. The volume of 27.40 mL of NaOH(aq) was needed to reach the equivalence point. Calculate: a) The concentration of the chloroacetic acid solution before the titration b) the pH of the chloroacetic acid solution before titration c) the pH of the solution at half equivalence point d) the pH of the solution at the equivalence point e) the pH of the solution when...