1.Determine the pH (to two decimal places) of a solution prepared by adding 51.3 mL of 0.0915 M sodium hydrogen sulfite (NaHSO3) to 39.4 g of sodium sulfite (Na2SO3). Assume the volume of the solution does not change and that the 5% approximation is valid.
2.Calculate the pH (to two decimal places) of the buffer solution after the addition of 1.15 g of sodium butanoate (NaC3H7COO) to the buffer solution above.
Assume 5% approximation is valid and that the volume of solution does not change.
3. The mole fraction of an aqueous solution of ammonium nitrite is 0.494. Calculate the molarity (in mol/L) of the ammonium nitrite solution, if the density of the solution is 1.45 g mL-1.
4. Determine the mole fraction of calcium nitrite in a 9.28 M aqueous solution of calcium nitrite. The density of the solution is 1.47 g mL-1.
Please answer the following 4 questions. Will upvote
1.Determine the pH (to two decimal places) of a solution prepared by adding 51.3 mL of 0.0915 M sodium hydrogen sulfite (NaHSO3) to 39.4 g of sodium sulfite (Na2SO3). Assume the volume of the solution does not change and that the 5% approximation is valid.
2.Calculate the pH (to two decimal places) of the buffer solution after the addition of 1.15 g of sodium butanoate (NaC3H7COO) to the buffer solution above.
Assume 5% approximation is valid and that the volume of solution does not change.
3. The mole fraction of an aqueous solution of ammonium nitrite is 0.494. Calculate the molarity (in mol/L) of the ammonium nitrite solution, if the density of the solution is 1.45 g mL-1.
4. Determine the mole fraction of calcium nitrite in a 9.28 M aqueous solution of calcium nitrite. The density of the solution is 1.47 g mL-1.
Please answer the following 4 questions. Will upvote
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