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Zinc sulfate is used to supply zinc in animal feeds, fertilizers, toothpaste, and agricultural sprays. Zinc sulfate, [6] like many zinc compounds, can be used to control moss growth on roofs. [7] Zinc sulfate can be used to supplement zinc in the brewing process. Zinc is a necessary nutrient for optimal yeast health and performance, although it ...
Single displacement reaction. A single-displacement reaction, also known as single replacement reaction or exchange reaction, is an archaic concept in chemistry. It describes the stoichiometry of some chemical reactions in which one element or ligand is replaced by atom or group. [ 1 ][ 2 ][ 3 ] It can be represented generically as: where either.
Standard electrode potential (data page) The data below tabulates standard electrode potentials (E °), in volts relative to the standard hydrogen electrode (SHE), at: Temperature 298.15 K (25.00 °C; 77.00 °F); Effective concentration (activity) 1 mol/L for each aqueous or amalgamated (mercury-alloyed) species; Unit activity for each solvent ...
Reduction: As 2 O 3 + 12 e − + 6 H + → 2 As 3− + 3 H 2 O. Overall, we have this reaction: As 2 O 3 + 6 Zn + 6 H + → 2 As 3− + 6 Zn 2+ + 3 H 2 O. In an acidic medium, As 3− is protonated to form arsine gas (AsH 3), so adding sulphuric acid (H 2 SO 4) to each side of the equation we get: As 2 O 3 + 6 Zn + 6 H + + 6 H 2 SO 4 → 2 As 3 ...
The concept of neutralization is not limited to reactions in solution. For example, the reaction of limestone with acid such as sulfuric acid is also a neutralization reaction. [Ca,Mg]CO 3 (s) + H 2 SO 4 (aq) → (Ca 2+, Mg 2+)(aq) + SO 2− 4 (aq) + CO 2 (g) + H 2 O. Such reactions are important in soil chemistry.
Half-reaction. In chemistry, a half reaction (or half-cell reaction) is either the oxidation or reduction reaction component of a redox reaction. A half reaction is obtained by considering the change in oxidation states of individual substances involved in the redox reaction. Often, the concept of half reactions is used to describe what occurs ...
Daniell cell. Daniell cells, 1836. The Daniell cell is a type of electrochemical cell invented in 1836 by John Frederic Daniell, a British chemist and meteorologist, and consists of a copper pot filled with a copper (II) sulfate solution, in which is immersed an unglazed earthenware container filled with sulfuric acid and a zinc electrode.
The water molecule is amphoteric in aqueous solution. It can either gain a proton to form a hydronium ion H 3 O +, or else lose a proton to form a hydroxide ion OH −. [5] Another possibility is the molecular autoionization reaction between two water molecules, in which one water molecule acts as an acid and another as a base.