The fact that a reaction takes place when potassium hydroxide is added to a solution of nickel(II) ions is an example of a  property.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO (aq) → Cu(s) + FeSO4(aq) ? Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 150. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 89. mg. 00. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits. 0 || 09 Explanation Check x10 X G 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility Ar

A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction:   A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant.  If 45.0 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? _ g     [Number in standard notation; round your answer to one decimal place]   The following molar masses may or may not be needed, but are provided to save you time: barium sulfate = 233 g/mol sulfuric acid = 98.0 g/mol

Write a balanced equation for the reaction of nitric acid, HNO3(aq), with magnesium hydroxide, Mg(OH)2(aq). Include physical states.