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?

Expert Solution

queen_honey_blossom answered 2 years ago

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?

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate...

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate in 200 ml of 1M acetic acid? The Ka for acetic acid id 1.7*10-5. B. Calculate the pH of the solution if 10 ml of 0.100M HCl is added to the solution. C. What will the pH be if 5.00 ml of 0.150M NaOH was added to solution in B? D. Write the equation when an acid and a base are added to the...

A solution is made by a dissolving 16.8 g of sodium fluoride , NaF , in...

A solution is made by a dissolving 16.8 g of sodium fluoride , NaF , in enough water to make exactly 500.ml of solution . Calculate the molarity of each species: NaF, Na+ and F-.

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.

A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of...

A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M hypochlorous acid (HClO). What is the pH of the solution after 0.0100 moles of sodium hydroxide is added? (The Ka of HClO is 2.9

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A solution is made by dissolving 10.0 g of sodium chloride in 110.5 g of water at 25oC. The density of the solution is 1.021 g/mL 1.What is the osmotic pressure of this solution? 2.What is the boiling point of this solution? 3.What is the freezing point of this solution?

A solution is made by dissolving 45.5 g of sodium phosphate in 265 g of ethanol....

A solution is made by dissolving 45.5 g of sodium phosphate in 265 g of ethanol. The resulting solution has a volume of 225 mL. Using the above information, values found in Table 14.6, a vapor pressure of 5.87×10−2 atm at 20 oC, and the theoretical van’t Hoff factor, determine the following for the resulting solution: A. M of Na3PO4 B. m of Na3PO4 C. Freezing point in oC D. Boiling point in oC E. Osmatic pressure at 20 oC...

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.

A buffer solution is prepared by dissolving 1.50 g each of sodium benzoate, C6H5COONa, and benzoic...

A buffer solution is prepared by dissolving 1.50 g each of sodium benzoate, C6H5COONa, and benzoic acid, C6H5COOH (Ka = 6.45 × 10-5), in 150.0 mL of solution. The molar mass of benzoic acid is 122.12 g/mol and that of sodium benzoate is 144.10 g/mol. a) What is the pH of this buffer solution? b) Which buffer component must be added to change the pH to 4.00? What mass of that component is required? c) What volume of 2.0 M...

Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.969 g...

Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 4.969 g KH2PO4 and 1.757 g K2HPO4 in water to give 200. mL of solution. Stepwise acid dissociation constants for phosphoric acid may be found in your textbook. (b) a solution made by mixing 10.00 mL 0.29 M (CH3)2NH with 40.00 mL 0.17 M (CH3)2NH2Cl. The base dissociation constant Kb is 7.40 x 10-4 for (CH3)2NH. Assume that the final volume is the sum of the...

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