b. To 1.200 liters of the buffer in part a, you add 3.75 mL of 2.500...
b. To 1.200 liters of the buffer in part a, you add 3.75 mL of 2.500 M barium hydroxide. What is the pH after that addition? Yes, you may use the H-H equation here. For your convenience, the buffer is 0.125 M formic acid (?a = 1.77 x 10!!) and 0.140 M sodium formate. (8 pts.)
The previous question it is referring too is a buffer of 0.125 M formic acid Ka=1.77X 10^-4 and 0.140 M sodium formate. with a PH of 3.75
Homework Answers
![I mol. Balottle produ 2 mol. OHO hydroxide xide in concentration, [OH-] = = 2x 7.768 2 * 10 m) 0.01558 (M) ce more Now given](http://img.homeworklib.com/questions/0ebbcf80-dac7-11ea-9eaa-37bad3b00d01.png?x-oss-process=image/resize,w_560)
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b. To 1.200 liters of the buffer in part a, you add 3.75 mL of
2.500...
c. To 238.00 milliliters of the buffer in part a, you add 13.38 mL of 2.500...
c. To 238.00 milliliters of the buffer in part a, you add 13.38 mL of 2.500 M HClO!. What is the pH after that addition? Yes, you may use the H-H equation here. For your convenience, the buffer is 0.125 M formic acid (?! = 1.77 x 10!!) and 0.140 M sodium formate. (6 pts.)
Describe the preparation of 2 liters of 0.25 formate buffer, pH 4.5, starting with 1M formic...
Describe the preparation of 2 liters of 0.25 formate buffer, pH 4.5, starting with 1M formic acid and solid sodium formate (HCOONa). pKa of HCOOH, formic acid is 3.75
You combine 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The...
You combine 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4 what is the pH of the solution? With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4. You add 8g sodium hydroxide to this solution, what is the new pH? With the same initial solution of 0.75 moles formate and 0.85 moles...
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning...
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning to use formic acid (HCOOH) and sodium formate (HCOONa) for this job. What should the mass of sodium formate that he should add to 250,0 mL of 0.20 M formic acid solution to prepare this buffer? (K =1.8x10 for formic acid.) 3. If 0.10 M solution of a weak acid has a pH of 3.90, find the Ka for the acid.
A student must make a buffer solution with a pH of 1.50. Determine which weak acid...
A student must make a buffer solution with a pH of 1.50. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, Ka = 1.34 x 10-5, 3.00 M formic acid, Ka = 1.77 x 10-4, 2.00 M O acetic acid, Ka = 1.75 x 10-5,5.00 M O sodium bisulfate monohydrate, Ka = 1.20 x 10-2, 3.00 M Determine which conjugate base is the best option to make a buffer at...
Calculate how to prepare 750 ml of 0.25 M sodium formate buffer at pH 4. Use...
Calculate how to prepare 750 ml of 0.25 M sodium formate buffer
at pH 4. Use your textbook to determine the molecular weight and
pKa of the acid and base. Calculate the grams of sodium formate and
number of milliliters of formic acid required. THEN using this
stock solution, calculate and describe how you would prepare 100 ml
of a 10 mM formate buffer, pH 3.5. By the way, what is the molarity
of formic acid?
with pH 7.6 and...
Suppose you want to prepare a buffer with a pH of 4.35 using formic acid. What...
Suppose you want to prepare a buffer with a pH of 4.35 using formic acid. What ratio of [sodium formate]/[formic acid] do you need to make this buffer? Formic acid has a Ka of 1.8x10-4. Show work please.
please show work :) 7. You need to make a buffer to keep a solution at...
please show work :)
7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K4 = 1.40 x 103) and sodium chloroacetate 2. Formic acid (Ka = 1.77 x 10-4) and sodium formate 3. Iodic acid (Ka = 1.60 x 10-1) and sodium iodate 4. Phosphoric acid (K. = 7.52 x 10-3) and sodium phosphate 5. Propionic...
A buffer solution with a pH of 4.25 is prepared with the same volumes of _________...
A buffer solution with a pH of 4.25 is prepared with the same volumes of _________ M formic acid and 0.12 M sodium formate. The Ka of formic acid is 1.8 ⋅ 10-4. 3.7×10−2 0.38 1.8×104 7.5×10−2 1.9×10−2
Calculate the pH of a buffer solution that is 0.30 M formic acid (HCO2H) and 0.50...
Calculate the pH of a buffer solution that is 0.30 M formic acid (HCO2H) and 0.50 M sodium formate (HCO2Na). Ka of HCO2H is 1.8 x 10-4
You combine 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4 what is the pH of the solution? With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make a buffer solution. The Ka of formic acid is 1.8xl0'4. You add 8g sodium hydroxide to this solution, what is the new pH? With the same initial solution of 0.75 moles formate and 0.85 moles...
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning to use formic acid (HCOOH) and sodium formate (HCOONa) for this job. What should the mass of sodium formate that he should add to 250,0 mL of 0.20 M formic acid solution to prepare this buffer? (K =1.8x10 for formic acid.) 3. If 0.10 M solution of a weak acid has a pH of 3.90, find the Ka for the acid.
A student must make a buffer solution with a pH of 1.50. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, Ka = 1.34 x 10-5, 3.00 M formic acid, Ka = 1.77 x 10-4, 2.00 M O acetic acid, Ka = 1.75 x 10-5,5.00 M O sodium bisulfate monohydrate, Ka = 1.20 x 10-2, 3.00 M Determine which conjugate base is the best option to make a buffer at...
Calculate how to prepare 750 ml of 0.25 M sodium formate buffer
at pH 4. Use your textbook to determine the molecular weight and
pKa of the acid and base. Calculate the grams of sodium formate and
number of milliliters of formic acid required. THEN using this
stock solution, calculate and describe how you would prepare 100 ml
of a 10 mM formate buffer, pH 3.5. By the way, what is the molarity
of formic acid?
with pH 7.6 and...
please show work :)
7. You need to make a buffer to keep a solution at a pH of 2.50. You have several combinations of weak acids and their conjugate bases to choose from. 1. Chloroacetic acid (K4 = 1.40 x 103) and sodium chloroacetate 2. Formic acid (Ka = 1.77 x 10-4) and sodium formate 3. Iodic acid (Ka = 1.60 x 10-1) and sodium iodate 4. Phosphoric acid (K. = 7.52 x 10-3) and sodium phosphate 5. Propionic...
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