Question Completion Status: QUESTION 8 What is the percent dissociation of acetic acid if the solution...
4. Calculate the pH and percent dissociation of the solution when 125.0 mL of 0.100 M HCI is added to 500.0 mL of 0.150 M sodium acetate (Kb = 5.71 x 10-10) ANSWER: pH = 5.456, 16.7%
What is the pH of a solution that is 0.100 M in acetic acid and 0.150 M in sodium acetate? pKa of acetic acid = 4.76 A. 6.26 B. 4.58 C. 2.94 D. 4.94
A) A beaker with 1.80×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.50 mL of a 0.340 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. B)You need to produce a buffer solution that has a pH of 5.37. You already have a solution...
A sample of 0.100 M acetic acid (Kg = 1.8 x 10-5) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 15.0 mL of NaOH? O a. 11.40 O b. 3.18 O c. 1.88 O d. 4.38 Oe. 4.74
Acetic acid has a pKa of 4.74. A stock solution of 1.0 M acetic acid is available. A stock solution of 2.0 M potassium acetate is available. Show all the calculations and explain how to make 560.0 mL of 250. mM acetate buffer that has a pH = 5.0. (Hint: first make a 250 mM potassium acetate solution and a 250 mM acetic acid solution. Then determine how much of each to use.). pH = pKa + log {[acetate]/[acetic acid]}
Consider the titration of 100.0 mL of 0.200 M acetic acid ( Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a 0.0 mL pH= 50.0 mL pH = C 100.0 mL pH = 140.0 mL pH= C 200.0 mL pH = f 240.0 mL pH=
Solution C is a 1.00 L buffer solution that is 1.240 M in acetic acid and 0.56 Min sodium acetate. Acetic acid has a pKa of 4.74. What is the pH change of this solution upon addition of 0.07700 mol of HCI? Enter a negative number to 3 decimal places.
=Assume you have prepared 100.0 mL of a buffer solution using 0.400 mol of acetic acid (pKa = 4.74) and 0.400 mol of sodium acetate. The pH of this buffer solution is initially 4.74. After preparing this buffer solution, you added 55.0 mL of a 1.10 M NaOH solution to your buffer to see what would happen. What will the pH of this new solution be?
17. What is the volume of 1M acetic acid that needs to be added to 1L of 25mM sodium acetate solution to achieve pH of 5.5? Assume pka of 4.8 and the added acid to have negligible effect on volume. 18. For question 17 above, what will be the answer if concentration of sodium acetate in the initial 1L solution is 40mm? 19. What is the pH of a solution of 10-3 M HCI? Assume complete dissociation of hydrochloric acids...
Consider the titration of the titration of 50.0 mL of 0.100 M acetic acid (HC2H2O2) with 0.100 M. The pka = 4.76. d. Determine the pH after 50.0 mL of titrant (NaOH) have been added. This is the equivalence point. All of the acid has been converted to its conjugate base, pH is determined by the equilibrium for the conjugate base