=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?
pH of a buffer
pH = pKa + log(A-/HA)
before addition of base
mol of acid = 0.4
mol of conjguate = 0.4
then after addition of base
mmol of base added = M*V = 55*1.1 = 60.5 mmol = 0.0605 mol of base
mmol of conjugate = 0.4+0.0605 = 0.4605
mmol of acid = 0.4-0.0605 = 0.3395
substitue in pH of buffer
pH = pKa + log(A-/HA)
pH = 4.75 + log(0.4605/0.3395) = 4.882
=Assume you have prepared 100.0 mL of a buffer solution using 0.400 mol of acetic acid...
A solution is prepared by adding 0.400 mol of hydrogen sulfide, H2S (pKa = 7.00) and 0.400 mol of the hydrogen sulfide ion, HS to 100.0 mL of water. Predict the final pH when 55.0 mL of 1.10 M NaOH is added to this buffer solution. Please explain. Thank you!
A 1.00 L buffer solution with pH = 4.74 is composed of 0.30 mol acetic acid and 0.30 mol sodium acetate. A) Determine the pKa of acetic acid B) If 0.030 mol of NaOH is added, determine the pH of the solution
what is the ph of a solution prepared by dissolving 0.50 mol of acetic acid and 0.2 mol of sodium acetate in water and adjusting the volume of 0.5L if the pka for acetic acid is 4.75. of 0.010 mol of sodium hydroxide is added to the buffer solution from part (a), determine the ph of the new solution
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH and 0.05 mole of sodium acetate CH3COONa. Calculate a. pH of that solution b. How much of a strong base, say NaOH, in mol/L needs to be added to that solution to change its pH to 6.0? Notes and useful data: For acetic acid pK4.75 For carbonic acid pKa 6.3 and pKa 10.3 Sodium acetate CH3COONa dissociates entirely to Na'CH3COO
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M HCl to it, then what is the pH of this new solution?
9.30 mL of 0.1 M HCl are added to 200 mL of the buffer solution prepared in #8. What is the resulting pH? 8. A buffer solution is made by adding 20.4 grams of sodium acetate (NaCH CO2) toa 0.2M acetic acid (CH,CO2H) solution. The total volume of the resulting solution is exactly 1L. What is the phH of this solution? (Note: the pK, of acetic acid is 4.74) 20.4q NaCH3(02 82.034 9/mO 8203y g/mol .25 025 nol 1.0しー= 0.25mol...
You have 125 mL of an 0.19 M acetic acid solution. What volume (V) of 1.10 M NaOH solution must you add in order to prepare an acetate buffer of pH = 4.20? (The pKa of acetic acid is 4.76.)
Solution A is a 1.00 L buffer solution that is 1.196 M in acetic acid and 1.196 M in sodium acetate. Acetic acid has a pKa of 4.74. What is the pH change of this solution upon addition of 0.1 mol of HCl? Enter your answer numerically to three significant figures.
A buffer formed from 20.0 mL of 0.120 M Acetic acid (CH3COOH) (pKa = 4.74) and 12.0 mL of 0.200 M sodium acetate (CH3COONa). What is the pH of this buffer after addition of 0.0001 mol of HCl?
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.