b. State which reagent(s) and exactly how much you used of each to create the buffer!
Reagents |
|
Please show relevant calculations.
d. Would your buffer you made guard better against acid or base? What is the change in pH (a) 100 mL of 0.1 M HCl was added to the buffer (b) 100 mL of 0.1 M NaOH was added to the buffer? MUST SHOW WORK!!!
change in pH (a) 100 mL of 0.1 M HCl ____________________
change in pH (a) 100 mL of 0.1 M NaOH______________________
Would your buffer you made guard better against acid or base?_________________
Reagents |
Ka |
pKa |
0.1 M Hydrochloric acid, HCl |
1.3 x 106 |
- 6.11 |
0.1 M Nitric acid, HNO3 |
2.4 x 101 |
- 1.38 |
0.1 M Acetic acid, CH3COOH |
1.7 x 10-5 |
4.77 |
0.1 M Sodium Acetate, CH3COONa |
||
0.1 M Benzoic Acid, C6H5COOH |
6.3 x 10-5 |
4.20 |
0.1 M Sodium Benzoate, C6H5COONa |
||
0.1 M Carbonic acid,H2CO3 |
4.3 x 10-7 |
6.37 |
0.1 M NaHCO3- |
4.8 x 10-11 |
10.32 |
Reagents |
Kb |
pKb |
0.1 M Ammonia, NH3 |
1.8 x 10-5 |
4.74 |
0.1 M Ammonium Chloride, NH4Cl |
||
0.1 M Methylamine, CH3NH2 |
4.4 x 10-4 |
3.36 |
0.1 M Methyl Ammonium Chloride, CH3NH3Cl |
||
0.1 M Sodium Hydroixde, NaOH |
- 20 |
You must prepare a solution to use as an environment that involves a particular strain of...
You are asked to prepare a pH=4.00 buffer starting from 1.50 L of 0.0200M solution of benzoic acid (C6H5COOH) and an excess of sodium benzoate (C6H5COONa). How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when the sodium benzoate is added.
Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL. measured pH 0.0 20 Did the pH change a little or a lot when NaOH was added to the butter? Was the change you observed consistent with the action of a butter? For the ammonium chloride-ammonia buffer give the measured pH for the 50.0 mL of 0.10 Mammonia. Is this solution acidic, neutral, or basic? Did the pH of the ammonia increase or decrease...
4. (5 pts) Explain if pH of solution will increase, no change, or decrease) if: - add solid ammonium nitrate to 0.02 M nitric acid - add 1.0 g of sodium hydroxide to 100.0 mL of 1.0 M acetic acid - add 1.0 g of sodium chloride to 100.0 mL of 0.01 M HCI - add 1.0 mL of 0.10 M HCl to 20.0 mL of 0.01 M ammonia - add 0.1 g of NaOH to 100.0 L of distilled...
1) How would you make 300 ml of a 0.1 M sodium phosphate buffer, pH 7.0 (pKa = 7.2) phosphate dibasic (the conjugate base). 2) What are the concentrations of acetate and acetic acid in a 0.2 M acetate buffer pH 5.3? The pKa for acetic acid is 4.76. 3)You have 100 ml of 0.1 M acetate buffer pH 5.2 (pKa 4.76). You add 10 ml of 0.1 M NaOH. Calculate the resulting change in pH and the buffering capacity...
D. Buffers 1. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.50 M acetic acid. Assuming the change in volume when the sodium acetate is added is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The K, for acetic acid is 1.8 x 105. 2. Calculate the pH of a buffer solution that initially consists of 0.0400 moles of ammonia and 0.0250 moles of ammonium ion, after 20.0...
Your lab TA asks you to prepare a buffer solution with a pH of 7.40. The following reagents are all available to you: 550 mL of 0.200 M formic acid, 450 mL of 0.200 M hypochlorous acid, solid sodium formate and solid sodium hypochlorite. a) Which 2 ingredients will you use to prepare the desired buffer? b) What is the base/acid ratio in the desired buffer? c) What mass (in g) of solid base must you dissolve in the corresponding...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
1. A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of this solution after 5.00 mL 10.0 M HCl is added? 2. Which of the following solution(s) is a buffer? 100 mL of 0.1 M acetic acid mixed with 25 mL of 0.5 M NaOH 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.05 M sodium...
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.