1. Estimate the pH of a buffer consisting of 0.4 M acetic acid and 0.3 M acetate. The pKa of acetic is 4.75.
a) Why is the pH approximately equal to the pKa?
b) Will the exact pH be larger or smaller than the pKa? Explain.
2. How would you use a pH titration to determine the concentration of a weak base?
a) What kind of substance would you titrate with?
b) What is the major species at the beginning of the titration?
c) What is the major species at the equivalence point?
1. Estimate the pH of a buffer consisting of 0.4 M acetic acid and 0.3 M...
1. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 2. Without doing any math, which solution has a lower pH: (a) 0.05 M acetic acid that has been titrated to its endpoint using NaOH, or (b) a buffer prepared from 0.05 acetic acid and 0.05 M sodium acetate. Explain your answer. 3. What pH did you...
You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate
Suppose you want to make an acetic acid/acetate buffer to a pH of 5.00 using 10.0 mL of 1.00 M acetic acid solution. How many milliliters of 1.00 M sodium acetate solution would you need to add? The pKa for acetate buffer is 4.75.
calculate the ph of a buffer solution that contains 1.5 M acetic acid (CH3COOH) and 0.3 M sodium acetate (CH3COONa) [Ka=1.8x10-5 for acetic acid]
1- Calculate the PH of a buffer made by mixing 20ML of .125M acetic acid with 30ML of .100M sodium acetate 2- calculate the equivalence point from a titration of .30ML of .125 M acetic acid with 1.00 M NaOH
Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is 4.75. How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 4.90 ? ___mL?
1. You need to prepare an acetate buffer of pH 5.93 from a 0.833 M acetic acid solution and a 2.56 M KOH solution. If you have 475 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.93? The pKa of acetic acid is 4.76. 2. If a buffer solution is 0.110 M in a weak acid (Ka = 1.6 × 10-5) and 0.570 M...
You need to prepare an acetate buffer of pH 6.29 from a 0.704 M acetic acid solution and a 2.48 M KOH solution. If you have 575 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 6.29? The pKa of acetic acid is 4.76. You need to prepare an acetate buffer of pH 6.29 from a 0.704 M acetic acid solution and a 2.48 M...
Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is 4.75. 1st attempt FeedbackSee HintSee Periodic Table How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.05 ?
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...