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Hydrobromic acid is an aqueous solution of hydrogen bromide.It is a strong acid formed by dissolving the diatomic molecule hydrogen bromide (HBr) in water. "Constant boiling" hydrobromic acid is an aqueous solution that distills at 124.3 °C (255.7 °F) and contains 47.6% HBr by mass, which is 8.77 mol/L. Hydrobromic acid is one of the strongest mineral acids known.
KBr + H 2 SO 4 → KHSO 4 + HBr. Concentrated sulfuric acid is less effective because it oxidizes HBr to bromine: 2 HBr + H 2 SO 4 → Br 2 + SO 2 + 2 H 2 O. The acid may be prepared by: reaction of bromine with water and sulfur: [14] 2 Br 2 + S + 2 H 2 O → 4 HBr + SO 2; bromination of tetralin: [14] C 10 H 12 + 4 Br 2 → C 10 H 8 Br 4 + 4 HBr
The pH of a simple solution of an acid in water is determined by both and the acid concentration. For ... HBr: −8.8 ± 0.8: −6.8 ± 0.8 Hydroiodic acid: HI:
Addition of bromine to water gives hypobromous acid and hydrobromic acid (HBr(aq)) via a disproportionation reaction.. Br 2 + H 2 O HOBr + HBr. In nature, hypobromous acid is produced by bromoperoxidases, which are enzymes that catalyze the oxidation of bromide with hydrogen peroxide: [2] [3]
The pH range is commonly given as zero to 14, but a pH value can be less than 0 for very concentrated strong acids or greater than 14 for very concentrated strong bases. [2] The pH scale is traceable to a set of standard solutions whose pH is established by international agreement. [3]
In this case H 0 and H − are equivalent to pH values determined by the buffer equation or Henderson-Hasselbalch equation. However, an H 0 value of −21 (a 25% solution of SbF 5 in HSO 3 F ) [ 5 ] does not imply a hydrogen ion concentration of 10 21 mol/dm 3 : such a "solution" would have a density more than a hundred times greater than a ...
The pH at the end-point depends mainly on the strength of the acid, pK a. The pH at the end-point is greater than 7 and increases with increasing concentration of the acid, T A, as seen in the figure. In a titration of a weak acid with a strong base the pH rises more steeply as the end-point is approached. At the end-point, the slope of the ...
Bases are proton acceptors; a base will receive a hydrogen ion from water, H 2 O, and the remaining H + concentration in the solution determines pH. A weak base will have a higher H + concentration than a stronger base because it is less completely protonated than a stronger base and, therefore, more hydrogen ions remain in its solution.