A sample of pure lead weighing `2.07 g` is dissolved in nitric acid to give a solution of lead nitrate. This solution is treated with hydrochloric acid, chlorine gas and ammonium chloride. The result is a precipitate of `(NH_(4))_(2) PbCl_(6)`. What is the maximum weight of this product that could be obtained form the lead sample?

Write the balanced chemical equation and identify the type of reaction in each case. Lead acetate solution is treated with dilute hydrochloric acid to form lead chloride and acetic acid solution.

Write a balanced chemical equation of the following reactions and also classify them. Lead acetate solution is treated with dilute hydrochloric acid to form lead chloride and acetic acid solution.

Elemental silicon is oxidized by O_(2) to give a compound shich dissolves in molten Na_(2)CO_(3) . When this solution is treated with aqueous hydrochloric acid, a precipitate forms. What is the precipitate?

2 g of a metal when dissolved in nitric acid converted to its nitrate. The nitrate was then precipitated to 2.66 g of the metal chloride. Find the equivalent weight of the metal.

2 g of a metal when dissolved in nitric acid converted to its nitrate. The nitrate was then precipitated to 2.66 g of the metal chloride. Find the equivalent weight of the metal.

A sample of iron ore, weighing 0.700 g, is dissolved in nitric acid. The solution is then, diluted with water, following with sufficient concentrated aqueous ammonia, to quantitative precipitation the iron as Fe(OH)_(3) . The precipitate is filtered, ignited and weighed as Fe_(2)O_(3) . If the mass of the ignited and dried preciipitate is 0.541 g, what is the mass percent of iron in the original iron ore sample (Fe=56)

Write a balanced chemical equation for each of the following reactions and also classify them . Lead acetate solution is treated with dilute hydrochloric acid to form lead chloride and acetic acid solution.