1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of...

1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of solid NaOH to the original buffer solution.

2) Calculate the pH of 1.0 L of the solution upon addition of 30.0 mL of 1.0 MHCl to the original buffer solution.

3) A 1.0L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.

3A) Calculate the pH of the solution upon the addition of 0.015 mol of NaOH to the original buffer.

3B) Calculate the pH of the solution upon the addition of 10.0 mL of 1.00 MHCl to the original buffer.

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queen_honey_blossom answered 2 years ago

Calculate the pH of 1.0 L upon addition of 0.190 mol of solid NaOH to the...

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A.) Calculate the pH of 1.0 L of the solution, upon addition of 49.00 mL of...

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Upon mixing 0.050 L of 0.010 M aqueous solution of mercury (II) nitrate with 0.020 L...

Upon mixing 0.050 L of 0.010 M aqueous solution of mercury (II) nitrate with 0.020 L of 0.10 M aqueous solution of sodium sulfide, a precipitate of mercury (II) sulfide forms. A) Write a balanced molecular equation of this reaction. B) Determine the theoretical yield of mercury (II) sulfide formed from the limiting reagent. C) Calculate the % yield of product when 0.082 grams of mercury (II) sulfide is isolated.

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1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of...

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