calculate the pH of a .250 M sodium formate, NaCHO2 solution. SHow all work, including your...

calculate the pH of a .250 M sodium formate, NaCHO2 solution. SHow all work, including your balanced chemical equation and law of mass action.

Expert Solution

queen_honey_blossom answered 2 years ago

Part A: Calculate the pH of a solution that is 0.250 M in sodium formate (HCOONa)...

Part A: Calculate the pH of a solution that is 0.250 M in sodium formate (HCOONa) and 0.110 M in formic acid (HCOOH). Part B: Calculate the pH of a solution that is 0.520 M in pyridine (C5H5N) and 0.470 M in pyridinium chloride (C5H5NHCl). Part C: Calculate the pH of a solution that is made by combining 55 mL of 0.040 M hydrofluoric acid with 125 mL of 0.120 M sodium fluoride.

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate,...

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+]----------------M pH--------------------- 2. What are the equilibrium concentrations of NH3, NH4+, and OH- in a 0.42 M solution of ammonia? What is the pH of the solution? Kb = 1.8 * 10^-5 [OH-] ----------------------- M [NH4+] ----------------------M [NH3] ---------------------- M pH----------------------------

Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2....

Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+] =_____ M pH =______

Calculate the pH of a solution made by adding 44.0 g of sodium formate, NaHCOO, to...

Calculate the pH of a solution made by adding 44.0 g of sodium formate, NaHCOO, to 200. mL of 0.23 M formic acid, HCOOH. Hint what kind of solution is made? The Ka for HCOOH is 1.8 x 10-4 M. As usual, report pH to 2 decimal places.

12. Calculate the pH of a 0.10 M solution of potassium formate, KHCOO. Ka of formic...

12. Calculate the pH of a 0.10 M solution of potassium formate, KHCOO. Ka of formic acid (HCOOH) = 1.8 x 10^-4. Write the dissociation equation and label each ion as acidic, basic, or neutral. Also write the hydrolysis equation. Dissociation equation: _____________________________________ cation: __________ anion: __________ Hydrolysis equation: _________________________________________________________________________

An aqueous solution is prepared to be 0.243 M in sodium formate and 0.120 M in...

An aqueous solution is prepared to be 0.243 M in sodium formate and 0.120 M in benzoic acid. (1) Is this solution a buffer solution? (2) What is the pH of this solution? (3) If 0.124 moles of hydrobromic acid are added to one liter of this solution, what is the pH of the resulting solution? Ka value of benzoic acid = 6.3X10^-5

A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of...

A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of a 0.30 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4. a) What is the pH of this buffer? b) Write two chemical equations showing how this buffer neutralizes added acid and added base. c) What mass of solid NaOH can be added to the solution before the pH rises above 4.60?

A buffer is made by dissolving 4.900 g of sodium formate (NaCHO2) in 100.00 mL of...

A buffer is made by dissolving 4.900 g of sodium formate (NaCHO2) in 100.00 mL of a 0.31 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4. a) What is the pH of this buffer? b) Write two chemical equations showing how this buffer neutralizes added acid and added base. c) What mass of solid NaOH can be added to the solution before the pH rises above 4.60?

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.

Calculate the pH of a 0.01 M solution of sodium benzoate. A: Dissociation constant of benzoic...

Calculate the pH of a 0.01 M solution of sodium benzoate. A: Dissociation constant of benzoic acid. B: Calculate the hydrolysis constant of sodium benzoate. C: Calculate the pH of the 0.01 M solution.

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