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18 Dec 2019

A buffer solution is prepared by dissolving 1.25 g each of benzoic acid, C6H5CO2H, and sodium benzoate, NaC6H5CO2, in 300.0 mL of solution. Look in your textbook for any necessary equilibrium constants. What is the pH of this buffer solution? Show all work

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Elin Hessel
Elin HesselLv2
31 Dec 2019

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Related questions

Calculate the pH of a solution made by adding 10.0 g of sodium benzoate, NaC6H5CO2 , to 3.0g of benzoic acid, C6H5COOH, and dissolving in water to make1.00 L of solution.

a solution is prepared by dissolving a 90.0 g of benzoIc acid (HC7H5O2) and 90.0 g of sodium benzoate (NaC7H5O2) in enough water to give total volume of 500 ml

a. calculate the pH of the solution?

b. A 10.0 ml sample of 0.50 M HCl is added to 90.0 ml of the solution from part (a). assuming volumes are additve, calculate the pH of the solution.?

C. you are tasked with making exactly 5.00L of a pH 4.50 buffer using 1.0 M benzoic acid and 1.5 M sodium benzoate solutions. what volume of each solution will you need to use to prepare this buffer.?

You need to prepare 100.0 mL of a pH=4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.140 M sodium benzoate. How much of each solution should be mixed to prepare this buffer?

mL benzoic acid?

mL sodium benzoate?

The answer is not 57mL benzoic acid and 43mL sodium benzoate

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