Question 2.
pH = pKa + Log{[CH3COONa - HCl]/[CH3COOH + HCl]}
Moles of CH3COONa = (100/1000) L * 1.5 mol/L = 0.15 mol
Moles of CH3COOH = (100/1000) L * 0.9 mol/L = 0.09 mol
Now, pH = 4.74 + Log{(0.15 - 0.03)/(0.09 + 0.03)}
Therefore, pH = 4.74
Question 3.
pH = pKa + Log{[CH3COONa + NaOH]/[CH3COOH - NaOH]}
Moles of CH3COONa = (200/1000) L * 1.5 mol/L = 0.3 mol
Moles of CH3COOH = (200/1000) L * 0.9 mol/L = 0.18 mol
Moles of NaOH = (150/1000) L * 0.02 mol/L = 0.003 mol
Now, pH = 4.74 + Log{(0.3 + 0.003)/(0.18 - 0.003)}
Therefore, pH = 4.97
Need help with number three please salt Find the pH of a buffer solution containing of...
Module 11 Homework 1. Find the pH of a buffer solution containing of 1.5M sodium acetate and 0.9M acetic acid. The K, of acetic acid is 1.8 x 105. 2. Find the pH of 100.0 mL of the buffer from exercise 1 after the addition of 0.030 mol of gaseous hydrochloric acid. Assume no volume change. 3. Find the pH of 200.0 mL buffer from exercise 1 after the addition of 150.0 mL of 0.020M NaOH. 4. What conjugate acid-base...
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
=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?
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?
With this information how would I calculate the pH of .01 M Ammonia solution and the pH of .01 M Ammonia buffer solution I need Ph of acetic acid! sorry for the wrong wording! A. Preparation of Acetic Acid-Acetate Buffer Solution An acetate buffer contains the acid-base pair, acetic acid and the acetate fon (typically added as sodium acetate). For acetic acid, pk, = -log (1.8 10 = 4.74. Consider the con ditions that will yield 100 ml of an...
(4 pts) What is the pH of the a buffer solution containing 0.10 moles of acetic acid and 0.12 moles of sodium acetate in 45 ml after adding 0.030 moles of KOH? 3. 0.049L Acenc acid + KOH CH3CO0K t H20 HOE
You need to produce a buffer solution that has a pH of 5.50. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74.
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...
You need to produce a buffer solution that has a pH of 5.36. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles.
this is my answer but I’m not sure if it is correct 8. A buffer solution is made by adding 20.4 grams of sodium acetate (NaCH CO) to a 0.2M acetic acid (CH3CO2H) solution. The total volume of the resulting soluti exactly 1L. What is the pH of this solution? (Note: the pKa of acetic acid is 4.74) uffer solution is made by adding 204 grams of sodium acetate (NaCHsCOn) to a 0.2M acetic acid ( HCOH) solution. The total...