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2 Fe(NO 3) 3 + 3 K 2 CrO 4 → Fe 2 (CrO 4)3 + 6 KNO 3 It also can be formed by the oxidation by air of iron and chromium oxides in a basic environment: 4 Fe 2 O 3 + 6 Cr 2 O 3 + 9 O 2 → 4 Fe 2 (CrO 4 ) 3
Acid rain is rain or any other form of precipitation that is unusually acidic, meaning that it has elevated levels of hydrogen ions (low pH). Most water, including drinking water, has a neutral pH that exists between 6.5 and 8.5, but acid rain has a pH level lower than this and ranges from 4–5 on average.
Diagram depicting the sources and cycles of acid rain precipitation. Freshwater acidification occurs when acidic inputs enter a body of fresh water through the weathering of rocks, invasion of acidifying gas (e.g. carbon dioxide), or by the reduction of acid anions, like sulfate and nitrate within a lake, pond, or reservoir. [1]
Fe 2 O 3 + H 2 → 2 Fe 3 O 4 + H 2 O. Iron(III) oxide is insoluble in water but dissolves readily in strong acid, e.g., hydrochloric and sulfuric acids. It also dissolves well in solutions of chelating agents such as EDTA and oxalic acid. Heating iron(III) oxides with other metal oxides or carbonates yields materials known as ferrates (ferrate ...
Ferric chloride is an alternative name for iron(III) chloride (FeCl 3). The adjective ferrous is used instead for iron(II) salts, containing the cation Fe 2+. The word ferric is derived from the Latin word ferrum, meaning "iron". Although often abbreviated as Fe 3+, that naked ion does not exist
The chromate ion is the predominant species in the region to the right of the green and blue lines. Above pH ~6.75 it is always the predominant species. At pH < 5.89 (pH < p K 1 ) the hydrogen chromate ion is predominant in dilute solution but the dichromate ion is predominant in more concentrated solutions.
When metallic iron (oxidation state 0) is placed in a solution of hydrochloric acid, iron(II) chloride is formed, with release of hydrogen gas, by the reaction Fe 0 + 2 H + → Fe 2+ + H 2 Iron(II) is oxidized by hydrogen peroxide to iron(III) , forming a hydroxyl radical and a hydroxide ion in the process.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.