Question

To determine the concentration of a solution of sulfuric acid, a 125.0-mL sample is placed in a flask and titrated with a 0.1433 M solution of cesium hydroxide. A volume of 20.29 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of sulfuric acid in the original sample.

A student has 530.0 mL of a 0.1474 M aqueous solution of MnSO₄ to use in an experiment. He accidentally leaves the container uncovered and comes back the next week to find only a solid residue. The mass of the residue is 18.83 g. Determine the chemical formula of this residue.

It is desired to neutralize a solution X that contains a mixture of potassium iodide and hydrobromic acid. Titration of 11.0 mL X with 0.147 M silver nitrate required 39.9 mL of the latter. The resulting precipitate, containing a mixture of AgI and AgBr, was dried and found to weigh 1.170 g. How much 0.142 M sodium hydroxide should be used to neutralize 11.0 mL solution X?

Answer 1