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For example, sulfuric acid (H 2 SO 4) is a diprotic acid. Since only 0.5 mol of H 2 SO 4 are needed to neutralize 1 mol of OH −, the equivalence factor is: f eq (H 2 SO 4) = 0.5. If the concentration of a sulfuric acid solution is c(H 2 SO 4) = 1 mol/L, then its normality is 2 N. It can also be called a "2 normal" solution.
Molar concentration or molarity is most commonly expressed in units of moles of solute per litre of solution. [1] For use in broader applications, it is defined as amount of substance of solute per unit volume of solution, or per unit volume available to the species, represented by lowercase : [2]
It exists as the anhydrous salt Ce(SO 4) 2 as well as a few hydrated forms: Ce(SO 4) 2 (H 2 O) x, with x equal to 4, 8, or 12. These salts are yellow to yellow/orange solids that are moderately soluble in water and dilute acids. Its neutral solutions slowly decompose, depositing the light yellow oxide CeO 2. Solutions of ceric sulfate have a ...
4 and OH − do not account for a significant fraction of the total amount of ammonia except in extremely dilute solutions. [ 6 ] The concentration of such solutions is measured in units of the Baumé scale ( density ), with 26 degrees Baumé (about 30% of ammonia by weight at 15.5 °C or 59.9 °F) being the typical high-concentration ...
2 NH 3 + H 2 SO 4 → (NH 4) 2 SO 4. A mixture of ammonia gas and water vapor is introduced into a reactor that contains a saturated solution of ammonium sulfate and about 2% to 4% of free sulfuric acid at 60 °C. Concentrated sulfuric acid is added to keep the solution acidic, and to retain its level of free acid.
The yellow anhydrous form, NiSO 4, crystallizes in orthorhombic crystal system [2] and in standard pressure decomposes to NiO in temperatures above 640 °C, before reaching the melting point. [3] It melts only at high system pressure, using a constant volume method the melting point was found to be 1210 °C. [ 4 ]
Ammonium iron(II) sulfate, or Mohr's salt, is the inorganic compound with the formula (NH 4) 2 SO 4 ·Fe(SO 4)·6H 2 O. Containing two different cations, Fe 2+ and NH + 4, it is classified as a double salt of ferrous sulfate and ammonium sulfate. It is a common laboratory reagent because it is readily crystallized, and crystals resist oxidation ...
Na 2 SO 4 + 2 C → Na 2 S + 2 CO 2. This reaction was employed in the Leblanc process, a defunct industrial route to sodium carbonate. Sodium sulfate reacts with sulfuric acid to give the acid salt sodium bisulfate: [9] [10] Na 2 SO 4 + H 2 SO 4 ⇌ 2 NaHSO 4. Sodium sulfate displays a moderate tendency to form double salts.