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Aqueous solutions of zinc sulfate consist of the aquo complex [Zn(H 2 O) 6] 2+. Zinc sulfate is produced by treating virtually any zinc-containing material (metal, minerals, oxides) with sulfuric acid. [4] Specific reactions include the reaction of the metal with aqueous sulfuric acid: Zn + H 2 SO 4 + 7 H 2 O → ZnSO 4 ·7H 2 O + H 2
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.
Lucas' reagent. Lucas test: negative (left) with ethanol and positive with t -butanol. "Lucas' reagent" is a solution of anhydrous zinc chloride in concentrated hydrochloric acid. This solution is used to classify alcohols of low molecular weight. The reaction is a substitution in which the chloride replaces a hydroxyl group.
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 same equation relating the concentrations of acid and base applies. 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
NaCl + H 2 SO 4 → NaHSO 4 + HCl. Aluminium sulfate, also known as paper maker's alum, is made by treating bauxite with sulfuric acid: 2 AlO(OH) + 3 H 2 SO 4 → Al 2 (SO 4) 3 + 4 H 2 O. Sulfuric acid can also be used to displace weaker acids from their salts. Reaction with sodium acetate, for example, displaces acetic acid, CH 3 COOH, and ...
Ga(s) + 3 OH −-1.22: 3 [6]: 788 Ti Ti 2 O 3 (s) + 2 H + + 2 e −: ⇌ 2TiO(s) + H 2 O-1.23 2 [6]: 792 Zn Zn(OH) 2− 4 + 2 e −: ⇌ Zn(s) + 4 OH −-1.199 2 [10] Mn Mn 2+ + 2 e −: ⇌ Mn(s) -1.185 2 [10] Fe Fe(CN) 4− 6 + 6 H + + 2 e −: ⇌ Fe(s) + 6HCN(aq) -1.16 2 [12] C: C(s) + 3 H 2 O (l) + 2 e −: ⇌: CH 3 OH (l) + 2 OH −-1. ...
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.