Using 4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid (pKa = 7.56) and 1.00 M NaOH or 1.00 M HCl; prepare 0.250...
Using 4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid (pKa = 7.56) and 1.00 M NaOH or 1.00 M HCl; prepare 0.250 L of 0.050 0 M buffer at pH 7.45. How many mL of the acid or the base is required?
Homework Answers
![pH = pka & log [AOT CHAT 7.45 = 7.5 >> log [AC]/[HA] = -0.11 > -100.11 20.78 » [A] = 0.78* [HA] THAT [no] + [HA] = 0.050 2) 0](http://img.homeworklib.com/questions/4ee6a8d0-9123-11ea-a716-29ca7bde2a08.png?x-oss-process=image/resize,w_560)
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Using 4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid (pKa =
7.56) and 1.00 M NaOH or 1.00 M HCl; prepare 0.250...
Given stocks of 1 M Lactic Acid (pKa 3.86) at pH 3.5, 2 M naOH, 2...
Given stocks of 1 M Lactic Acid (pKa 3.86) at pH 3.5, 2 M naOH, 2 M HCl and water: how would you prepare 4 liters of 0.05 M Lactic Acid at pH 3.25? Give 2 M Tris, pH 7.1 (pKa 8.0), 5 M NaOH, 5 M HCl, and water: how would you prepare 2 L of 0.2 M Tris, pH 7.4?
Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid...
Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the buffer...
1. Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic...
1. Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the...
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa...
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume: 1 volume: mL TOOLS x10
A 210.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium...
A 210.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate. 1) What is the pH after addition of 0.0050 mol of HCL 2) What is the pH after addition of 0.0050 mol of NaOH
Prepare a 100mL of a 0.050M buffer solution using trisodium phosphate/ phosphoric acid (pKa = 12.375) at pH 12.2. how much volume of 1M HCl or 1M NaOH is needed to adjust the pH
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1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is...
1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is the pH at the following "times?" (9 pts) a. Before any NaOH is added. b. After 20.00 mL of NaOH is added. c. After 500 mL of NaOH is added. 2. If 50.00 mL of 0.050 M formic acid, HCHO, (yes, you need to look up the Ka for formic acid) is titrated with 0.050 M NaOH, what is the pH at the following...
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...
When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact...
When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a: A. pH < pKa B. pH > 7.00 C. pH = pKa D. pH = 7.00 E. pH < 7.00
analytical chemistry A 1.00-L buffer solution was made with 0.150 M benzoic acid (HC7H3O2) and 0.250...
analytical chemistry
A 1.00-L buffer solution was made with 0.150 M benzoic acid (HC7H3O2) and 0.250 M lithium benzoate (LiCHO2). How many mL of 1.00 M HCI should be added to obtain the new pH of 3.97? The K of benzoic acid is 6.5 x 10 0.83 x 10 ml 1.0 x 102mL 1.3 x 102mL 5.6 mL 9.8 mL
Given stocks of 1 M Lactic Acid (pKa 3.86) at pH 3.5, 2 M naOH, 2 M HCl and water: how would you prepare 4 liters of 0.05 M Lactic Acid at pH 3.25? Give 2 M Tris, pH 7.1 (pKa 8.0), 5 M NaOH, 5 M HCl, and water: how would you prepare 2 L of 0.2 M Tris, pH 7.4?
1. Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the...
Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume: 1 volume: mL TOOLS x10
1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is the pH at the following "times?" (9 pts) a. Before any NaOH is added. b. After 20.00 mL of NaOH is added. c. After 500 mL of NaOH is added. 2. If 50.00 mL of 0.050 M formic acid, HCHO, (yes, you need to look up the Ka for formic acid) is titrated with 0.050 M NaOH, what is the pH at the following...
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...
analytical chemistry
A 1.00-L buffer solution was made with 0.150 M benzoic acid (HC7H3O2) and 0.250 M lithium benzoate (LiCHO2). How many mL of 1.00 M HCI should be added to obtain the new pH of 3.97? The K of benzoic acid is 6.5 x 10 0.83 x 10 ml 1.0 x 102mL 1.3 x 102mL 5.6 mL 9.8 mL
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