10 pts
Question 2. Suppose 5*10-4 M chloroacetic acid
(a) What are the sources of proton? Which proton source can be
ignored and why?
(b) What is the pH of the solution?
(c) Show and confirm any assumptions made in calculation of
pH.
(d) What is analytical concentration of chloroacetic acid?
10 pts Question 2. Suppose 5*10-4 M chloroacetic acid (a) What are the sources of proton?...
Question 2. Suppose 10-4 M chloroacetic acid (a) (2.5 pts) What are the sources of proton? Which proton source can be ignored and why? (b) (2.5 pts) What is the pH of the solution? (c) (2.5 pts) Show and confirm any assumptions made in calculation of pH. (d) (2.5 pts) What is analytical concentration of chloroacetic acid?
Please show steps and thought process.
Suppose you have a 50.00ml of 0.0100 M chloroacetic acid solution, HC_2H_2O_2CI. K_a=1.40 Times 10^-3. What is the initial pH for this solution? What is the equivalence point pH if the chloroacetic acid was titrated with 0.0100M NaOH?
A 25.0 mL sample of 0.150 M chloroacetic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The of chloroacetic acid is 1.4 ×10-3.
An initial solution is made by combing 13 mL of 0.8 M chloroacetic acid with 20 mL of a NaCH2ClCOO solution. (Ka= 1.4x10-3) a) The pH of the resulting solution was measured to be 2.92. What is the concentration of the NaCH2ClCOO solution? b) The solution from part a) is then titrated with 5 mL of 0.8 M NaOH. What is the pH of the resulting solution? c) If the solution is then titrated to its equivalence point, how much...
13) (5 pts) Calculate the pH (aq., 25 °C) of a 0.0150 M chloroacetic acid (CH,CICOOH) whose Ka = 140 x 10-3.
Formic acid Ka: 1.80x10^-4
Propanoic acid Ka: 1.34x10^-5
Chloroacetic acid Ka: 1.36x10^-3
Iodic acid Ka: 1.7x10^-1
What is the pH of a solution that is (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a prepared by dissolving 8.20 g of formic acid (46.03 g/mol) and 10.74 g of sodium formate (68.01 g/mol)...
Question 6 (2 points) Chloroacetic acid, HC2H2CIO2, has a greater acid strength than acetic acid, because the electronegativity chlorine atom pulls eloectroms way from the O-H bond and thus weakens it. What is the pH of a 0.043 M aqueous solution of chloroacetic acid? The Ka for HF is 1.3x10-3. You must solve the quadric equation for this problem. Express your answer to two decimal places. Your Answer: Answer s7 Question 7 (2 points) What is the pH of a...
Question 1 5 pts If 27.2 mL of 0.102 M acid with a pKg of 5.44 is titrated with 0.1 M NaOH solution, what is the pH of the titration mixture after 11.3 mL of base solution is added? 5 pts Question 2 If 20.7 mL of 0. 102 M acid with a pKa 4.33 is titrated with 0.107 M NAOH solution, what is the pH of the acid solution before any base solution is added? Question 3 5 pts...
5. What is the pH of a solution with a OH concentration of 2.52 x 10'M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 6. What is the pH of a solution with a H2O* concentration of 2.7 x 10 M? Is this solution acidic, basic, or neutral? Show the steps in your calculation. Answer 7. What is the pH of a solution with a OH concentration of 5.53 x 10-M? Is this solution...
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...