Calculate the pH of the following solutions 0.01M ammonium hydroxide; pKb= 4.76 0.01M acetic acid; pKa=...
Calculate the pH of the following solutions
0.01M ammonium hydroxide; pKb= 4.76
0.01M acetic acid; pKa= 4.76
A 1L solution prepared by mixing 500 ml of 0.02M acetic acid with 500 ml of 0.02M sodium acetate
can you solve with explanation please, thanks
Homework Answers
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Calculate the pH of the following solutions
0.01M ammonium hydroxide; pKb= 4.76
0.01M acetic acid; pKa=...
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic...
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.
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.
What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10...
What concentrations of acetic acid (pKa=4.76)(pKa=4.76) and acetate would be required to prepare a 0.10 M0.10 M buffer solution at pH 4.6pH 4.6? Note that the concentration, pH value, or both may differ from that in the first question. Strategy Rearrange the Henderson–Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A−]/[HA][A−]/[HA] . Use the mole fraction of acetate to calculate the concentration of acetate. Calculate the concentration of acetic acid. Step 1: The ratio...
Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and...
Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and sodium acetate). a. Calculate the volume of acetic acid and weight of sodium acetate necessary to prepare the buffer solution. pKa of acetic acid is 4.76
4. How much of (in mL) 0.15 M acetic acid (pKa 4.76) is needed to mix...
4. How much of (in mL) 0.15 M acetic acid (pKa 4.76) is needed to mix with 40 mL of 0.15 M sodium acetate to make a buffer of pH = 4.50 of 250 mL? (molar mass of acetic acid and sodium acetate are 60.0 g/mol and 82.0 g/ml, pKa of acetic acid is 4.76) (extra 10 pt)
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
Please Help a) Calculate the pH of a solution initially 0.1 M in acetic acid and...
Please Help 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 0.1 M HCL to 100ml of the buffer in part a.
what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M...
what concentration of acetic acid (pka=4.76) and acetate would be
required to prepare a .15 M buffer solution at pH 5.0?
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
A) Calculate the pH of an acetic acid solution. The concentration of acetic acid is 1.0696M...
A) Calculate the pH of an acetic acid solution. The concentration of acetic acid is 1.0696M and the pKa of acetic acid = 4.75. B) Calculate the pH of a sodium acetate solution of concentration 1.0401M. C) Calculate the pH of a solution made of 100 mL each of the two above solutions (200 mL total) D) Calculate the pH of a solution made of 40 mL of the solution in part C + 160 mL water (200 mL total)...
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.
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.
4. How much of (in mL) 0.15 M acetic acid (pKa 4.76) is needed to mix with 40 mL of 0.15 M sodium acetate to make a buffer of pH = 4.50 of 250 mL? (molar mass of acetic acid and sodium acetate are 60.0 g/mol and 82.0 g/ml, pKa of acetic acid is 4.76) (extra 10 pt)
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
what concentration of acetic acid (pka=4.76) and acetate would be
required to prepare a .15 M buffer solution at pH 5.0?
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
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