Formic acid,HCHO2 , is used to make methyl formate (a fumigant for dried fruit) and ethyl...

Formic acid,HCHO2 , is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). What is the pH of a 0.26 M solution of formic acid? What is the degree of ionization of HCHO2 in this solution

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queen_honey_blossom answered 2 years ago

With the same initial solution of 0.75 moles formate and 0.85 moles formic acid to make...

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 1.8x10-4. You add 60.7g hydrobromic acid to this solution, what is the new pH?

The formate ion, HCO2-, is formed when formic acid dissolves in water.

The formate ion, HCO2-, is formed when formic acid dissolves in water. A number of possible resonance structures for this ion are shown. Which of these structures are valid and which are invalid? Drag each item to the appropriate bin.

Calculate the pH at the following intervals if 30mL 0.20M of formic acid, HCHO2 is titrated...

Calculate the pH at the following intervals if 30mL 0.20M of formic acid, HCHO2 is titrated with 0.15M NaOH. For HCHO2 Ka = 1.8 x 10-4 a) before any NaOH has been added b) after a total of 15.0mL of NaOH has been added c) at the equivalence point d) after a total of 50.0mL of NaOH has been added.

(a) What is the pH of 0.89 M potassium formate, HCOOK? (The Ka of formic acid...

(a) What is the pH of 0.89 M potassium formate, HCOOK? (The Ka of formic acid is 1.8 ✕ 10−4.) (b) What is the pH of 0.65 M NH4Br? (The Kb of ammonia is 1.76 ✕ 10−5.)

1. Use the Henderson-Hasselbalch equation to determine the ratio of base/acid in a formic acid-formate buffer...

1. Use the Henderson-Hasselbalch equation to determine the ratio of base/acid in a formic acid-formate buffer with a pH of 3.00 2. Assume that the human blood buffer includes, at any one point, 0.00080 M carbonic acid and 0.0080 M hydrogen carbonate. What is the pH of 7.00 liter of blood under these conditions? 3. Metabolic acidosis results in the addition of excess acid to blood. How many moles of strong acid must be added to the blood in question...

Consider formic acid, HCHO2 (Ka = 1.9x10-4) and its conjugate base, CHO2-. a) A buffer is...

Consider formic acid, HCHO2 (Ka = 1.9x10-4) and its conjugate base, CHO2-. a) A buffer is prepared by dissolving 25.0 grams of sodium formate in 1.30 L of a solution of 0.660 M formic acid. Assume the volume remains constant after dissolving the sodium formate. i) Calculate the pH of this buffer. ii) Calculate the pH after 0.100 mole of nitric acid is added to this buffer. iii) Calculate the pH after 10.0 grams of potassium hydroxide...

A.You have 1 M solutions of formic acid and sodium formate. Calculate the volume of sodium...

A.You have 1 M solutions of formic acid and sodium formate. Calculate the volume of sodium formate required to make 1 liter of a solution with a pH of 4.1 in which the concentration of formic acid is 0.15 M. The pKa of formic acid is 3.75. B. Using the Henderson-Hasselbalch equation, explain why the pH of a solution of a weak acid and its conjugate base does not change upon dilution.

2.0 mL of 0.5M HCl was added to 50 mL of 0.5M Formate-formic acid buffer at...

2.0 mL of 0.5M HCl was added to 50 mL of 0.5M Formate-formic acid buffer at pH 3.6. (pKa= 3.75) What is the resulting pH after the addition of HCl? 2.0 mL of 0.5M HCl was added to 50 mL of 0.0625M Formate-formic acid buffer at pH 3.6. (pKa= 3.75) What is the resulting pH after the addition of HCl? 1.0 mL of 0.6M NaOH was added to 10 mL of 0.5M Acetate-acetic acid buffer at pH 4.2. What is...

Suppose we titrate 20.0 mL of 0.20 M of formic acid (HCHO2, Ka= 1.8 x 10^-4)...

Suppose we titrate 20.0 mL of 0.20 M of formic acid (HCHO2, Ka= 1.8 x 10^-4) with 0.20 M KOH. Calculate the pH for the following: a) before any base is added b) when half of the formic acid has been neutralized c) after a total of 15 mL has been added d) at the equivalence point

Ethyl butyrate, CH3CH2CH2CO2CH2CH3, is an artificial fruit flavor commonly used in the food industry for such...

Ethyl butyrate, CH3CH2CH2CO2CH2CH3, is an artificial fruit flavor commonly used in the food industry for such flavors as orange and pineapple. Its fragrance and taste are often associated with fresh orange juice, and thus it is most commonly used as orange flavoring. It can be produced by the reaction of butanoic acid with ethanol in the presence of an acid catalyst (H+): CH3CH2CH2CO2H(l)+CH2CH3OH(l)H+⟶CH3CH2CH2CO2CH2CH3(l)+H2O(l) Part A) Given 7.50 g of butanoic acid and excess ethanol, how many grams of ethyl butyrate...

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