A 1.00L buffer solution has the following concentrations: 1.50M formic acid and 1.25M sodium formate. The...

Question

Question

Answer 1

Answer #1

formic acid concentration = 1.50 M

concentration of sodium formate = 1.25 M

pKa = 3.74

pH = pKa + log [salt / acid]

= 3.74 + log [1.25 / 1.50]

pH = 3.66

concentration of NaOH = 0.20

pH = pKa + log [salt + C / acid - C]

= 3.74 + log [1.25 + 0.20 / 1.50 - 0.20]

pH = 3.787

pH change = 0.127

Add a comment

Answer 2

Similar Homework Help Questions

3. A 1.00L buffer solution has the following concentrations: 1.50M formic acid and 1.25M sodium formate....

3. A 1.00L buffer solution has the following concentrations: 1.50M formic acid and 1.25M sodium formate. The pK, for formic acid is 3.74. Determine the pH change of the buffer when 0.20moles of NaOH is added to the buffer. There is no change in the volume of the solution. (10 points)
A L.OOL buffer solution has the following concentrations: 1.50M formic acid and 1.25M sodium formate. The...

A L.OOL buffer solution has the following concentrations: 1.50M formic acid and 1.25M sodium formate. The pK, for formic acid is 3.74. Determine the pH change of the buffer when 0.20moles of NaOH is added to the buffer. There is no change in the volume of the solution. (10 points)
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for...

A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...

A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The...

A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The volume of the buffer is 100 mL ; with [HCOOH] = 0.110 mol L-1 and [HCOO- ] = 0.101 mol L-1 . The pKa of HCOOH = 3.74. What is the pH of this buffer? Write down the balanced chemical equation that describes the reaction of this buffer when an HCl solution is added. c) What is the resultant pH of this solution after...
Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO2. What is...

Suppose a buffer solution is made from formic acid, HCHO2, and sodium formate, NaCHO2. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? Select one: a. H3O+(aq) + OH–(aq) → 2H2O(l) b. OH–(aq) + HCHO2(aq) → CHO2–(aq) + H2O(l) c. NaOH(aq) + H3O+(aq) → Na+(aq) + 2H2O(l) d. NaOH(aq) + HCHO2(aq) → NaCHO2(aq) + H2O(l)
A buffer is composed of formic acid and its conjugate base, the formate ion. K for...

A buffer is composed of formic acid and its conjugate base, the formate ion. K for formic acid is 1.8 x 10. a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH

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...
4. Briefly explain the meaning of the term buffer capacity". A formic acid/sodium formate solution would...

4. Briefly explain the meaning of the term buffer capacity". A formic acid/sodium formate solution would be expected to buffer around what pH (use your textbook)? a) Calculate the pH for a solution containing 3.48 M CSHSN and 2.52 M C H NHBr. (Kb - 1.40 x 10" for CsH:N) Calculate the pH after 150.0 mL of 3.16 M HCl is added to 875.0 mL of the solution in part a) above.
inn? 1. Formic acid, (K= 1.8x10) a WA, and sodium formate, its' CB, are mixed together...

inn? 1. Formic acid, (K= 1.8x10) a WA, and sodium formate, its' CB, are mixed together in a 250.0 mL volume of 0.350 M formic acid and 0.455 M sodium formate- to form a buffer solution. a. If 1.00 mL of 1.00 M HCI is added to 250.0 mL of DI water, what is the new pH? What is the pH if the 250.0 mL of solution was only 0.350 M HCOH (no formate)? b. c. What is the pH...

a buffer solution with ph of 4.63 is prepared with 0.14m formic acid and ___m sodium...

a buffer solution with ph of 4.63 is prepared with 0.14m formic acid and ___m sodium formate. The ka of formic acid is 1.8*10^-4.