1a)Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250

Question

1a)Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250 M nitric acid. What is the final concentration of OH- ions in the solution after the reaction has gone to completion. Assume that there is no volume change when adding the grams of NaOH

1b)A monoprotic acid is an acid that donates a single proton to the solution. Suppose you have 0.140 g of a monoprotic acid dissolved in 35.0 mL of water. This solution is then neutralized with 14.5 mL of 0.110 M NaOH. What is the molar mass of the acid? Express your answer in g/mol.

Explanation / Answer

1a)

Verify the proportion:

NaOH:         15g / 40g/mol = 0.375 mol

Nitric acid     0.15L x 0.25 mol/L = 0.0375 mol

Conclusion:

Nitric acid is partially neutralized by NaOH and remains 0.375-0.0375 = 0.3375 mol strong acid.

Calculate pH:

pH = log 3.337

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