A titration is carried out to determine the molecular weight of oxalic acid. In this experiment, 0.617g of oxalic acid was dissolved in water and 18.3 mL of 0.75 M NaOH were used to reach the equivalence point of the titration. However, each mol of oxalic acid reacts with 2 mols of NaOH. A.What is the molecular weight of oxalic acid? B. What is the concentration of oxalic acid in the original solution if the total volume was 100mL

Consider Titration of 25 mL of .1 M CH3CO2H With .1 M NaOH. Calculate The pH After Adding The Following Volumes of NaOH: a. 0 mL b. 12.5 mL c. 20 mL d. 25 mL e. 37.5 mL I do know the correct answers, I just don't how to get to the answers. a. pH = 2.87 b. pH = 4.74 c. pH = 5.34 d. pH = 8.72 e. pOH = -log (0.0192 M) = 1.72  14 - 1.72 = 12.28 (I been having a hard time people getting the correct answer for part e, people keep getting 12.30 as the answer, but it is not. The correct answer is 12.28. I only remember how to do the last steps to get part e answer, which is 12.28, as it can be seen).

Consider the titration curve describing the titration of a strong acid by addition of a strong base. Which of the following statements is incorrect? a. The equivalence point is at pH = 7.0. b. The pH is lower at the end of the titration than at the beginning. c. The pH increases rapidly around the equivalence point. d. At the equivalence point, the only species present are water and a neutral salt. e. The pH does not increase very rapidly at the beginning of the titration.

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH,NH2, are titrated with 0.100 M HI. a. What is the volume of added acid at the equivalence point for each titration? b. Is the pH at the equivalence point for each titration acidic, basic, or neutral? c. Which titration curve has the lower initial pH? d. Sketch each titration curve.

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?

What is the least volume of 3.10 M HCl(aq) that will exceed the buffer capacity of 1.00 L of a buffer that is composed of 0.40 M acetic acid and 0.72 M sodium acetate?(Ka for acetic acid = 1.8 × 10−5.)   a. 0.55 L   b. 5.5 L   c. 0.14 L   d. 1.6 L   e. 0.20 L

12.0 10.0 8.0 pH 6.0 4.0 D 2.0 0.0 O 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. O The titration curve labelled "D" is generated by the strongest acid in the series. O The pk, of the conjugate base of the acid which generates curve "B" is about 6. O The Ka of the acid which generates curve "A" is about 10-5. O Titrating the acid in curve "A" requires the most acidic indicator in the series. O The Ka of the acid which generates curve "B" is about 10-6, The stronger the acid the higher its pH value at the beginning of the titration.

Question 7

23.Determine the pH ranges of the equivalence points in the titration curve below.

#9 plz