Consider the titration of a 21.0-mL sample of 0.110 M HC2H3O3 (Ka=1.8×10−5) with 0.120 M NaOH... 1. Determine the initial pH and the volume of added base required to reach the equivalence point. 2. Determine the pH at 5.00 mL of the added base, the pH at one-half of the equivalence point, and the pH after adding 6.00 mL of base beyond the equivalence point..

Q: Suppose you add a strong base to the hypochlorous acid/hypochlorite buffer. Write out the chemical reaction equation that would occur when you add a strong base to this buffer. English (United States) O Focus MacBook PrO A B IU @ #3 2$ & 3 4 7 8 !! く ○

4. A buffer is prepared containing 1.00 M acetic acid and 1.00 M sodium acetate. What is its pH?

Suppose that 50.00 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. (Weak Acid - Strong Base Titration) Find the pH if the following volume of NaOH are added. i. 30 mL NaOH ii. 35 mL NaOH iii. 40 mL NaOH iv. 45 mL NaOH v. 50 mL NaOH

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 answers, I just don't know the way to get to these answers. a. pH = 2.87 b. pH = 4.74 c. pH = 5.34 d. pH = 8.72 e.  pOH = -log(.0192 M) = 1.72 pOH 14-1.72 = 12.28 pH (I just know the last steps to  the answer for part e, but don't know all the other steps to get to answer).

Find the pH of the reaction mixture after the addition of the given volume (see below for your assignment) of 0.25M hydrochloric acid to a 20.0 mL sample of .15M potassium fluoride (Ka for HF =7.2 x 10^-4) 13.5 mL HCl added Weak base, strong acid pH curve Titration, post equivalence point

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).

1. A student titrates 25.0 mL of an unknown base with 0.10 M HCI. During the titration the pH is monitored and the collected data is recorded. These data are shown in the table at the right. a. Use the information provided to draw a titration curve showing the pH as a function of the volume of added HCI. Be certain to label your axes. b. Identify the equivalence point on your graph and justify your selection of this particular point. c. Use the data to determine the Kö value for the weak base. Be certain to show the mathematical steps you take to arrive at the answer. Report your final answer to the correct number of significant digits. d. The student has three indicators that she could use for this experiment. The indicators (with their endpoints) are: Bromophenol Blue (3.0 - 4.6), Methyl Red (4.2 – 6.3), and phenolphthalein (8.3 – 10.0). Which indicator would be appropriate for this titration? Justify your selection. e. Determine the (i) molarity and the (ii) % ionization of the…

Regarding titrations, which of the following is TRUE? A plot of pH vs. the [base]/[acid] ratio is known as a titration curve. The equivalence point is when the moles of base equals the moles of acid during any acid–base titration. Indicators do not respond to changes in pH. The pH is always 7 once the equivalence volume has been delivered. None of the answers are true.

In the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaOH a) the initial pH; b) pH after 50.0% completion of neutralization; c) pH after 100.0% completion of neutralization; d) Calculate the pH when 1 mL more NaOH is added after the equivalence point.