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
A 1.00 L buffer solution with pH = 4.74 is composed of 0.30 mol acetic acid...
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.
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?
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
A 1.00-litre buffer solution is made up containing 0.100 mol acetic acid and 0.200 mol sodium acetate: what is its’ pH? Then, 0.0500 mol of HCl gas is bubbled into the solution (assume no change in volume): what is the new pH? Data: pKa for acetic acid = 4.76
Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid and 1.00 M in sodium acetate after the addition of 0.150 mole of NaOH.
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
Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the buffer...
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]}
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...