I need help with this please. 1. Calculate the volume of a 0.1M NaOH that 40.0...
I need help with this please.
1. Calculate the volume of a 0.1M NaOH that 40.0 ml of the buffer could neutralize ( the pH of the buffer is 4.9)
2. Calculate the volume of a 0.1M HCl that 40.0 ml of the buffer could neutralize ( the pH of the buffer is 4.9)
3. How would your answers to 1 and 2 change if the system was made starting with 100.00ml of 0.010 M sodium acetate.
The buffer is acetic acid
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I need help with this please.
1. Calculate the volume of a 0.1M NaOH that 40.0...
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
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...
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.
a)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to...
a)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92g of sodium acetate(molar mass = 82.03gmol^-1) in 250 ml of 0.150 mol L^-1 of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8*10^-5) b)Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer...
Calculate the volume of 3 M HCl needed to change the pH of 75 mL of...
Calculate the volume of 3 M HCl needed to change the pH of 75 mL of the undiluted buffer solution by one pH unit (buffer capacity). The undiluted solution was prepared using 100 mL of 1.0870M acetic acid and 100mL of 1.0027M sodium acetate.
Need help with number three please salt Find the pH of a buffer solution containing of...
Need help with number three please
salt 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. acid pH=pka + log I salt) pH =-103(18410 9) +10g -(-4.74)+(. 2a) =14.96 2. Find the pH of 100.0 mL of the buffer from exercise 1 after the addition of 0.030 mol of gascous hydrochloric acid. Assume no volume change. Find the pH of 200.0 mL buffer from...
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and...
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.
Do the calculations to make 200ml of 0.1M sodium acetate buffer with a pH of 5.1...
Do the calculations to make 200ml of 0.1M sodium acetate buffer with a pH of 5.1 starting with 5.0M acetic acid and 1.0M NaOH ****show calculations***** 1.How much acetic acid is needed? 2.What is the ratio of Ac- to HAc at pH of 5.1? 3. What fraction of total acetate is Ac-at pH 5.1 4. How much OH- is needed to obtain 68.7% Ac-?
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M acetic acid/sodium acetate buffer 50.0 mL 0.10 M acetic acid/sodium acetate buffer + 1.0 mL 1.0 M HCl 50.0 mL 0.10...
D. Buffers 1. A buffer solution was made by dissolving 10.0 grams of sodium acetate in...
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...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
Need help with number three please
salt 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. acid pH=pka + log I salt) pH =-103(18410 9) +10g -(-4.74)+(. 2a) =14.96 2. Find the pH of 100.0 mL of the buffer from exercise 1 after the addition of 0.030 mol of gascous hydrochloric acid. Assume no volume change. Find the pH of 200.0 mL buffer from...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...
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...
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