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NH 4 Cl + NaOH → NH 3 + NaCl + H 2 O. Similarly, ammonium chloride also reacts with alkali-metal carbonates at elevated temperatures, giving ammonia and alkali-metal chloride: 2 NH 4 Cl + Na 2 CO 3 → 2 NaCl + CO 2 + H 2 O + 2 NH 3. A solution of 5% by mass of ammonium chloride in water has a pH in the range 4.6 to 6.0. [12]
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
R 2 NH + NaOCl → R 2 NCl + NaOH. Tert-butyl hypochlorite can be used instead of bleach: [9] R 2 NH + t-BuOCl → R 2 NCl + t-BuOH. Very few chloramines are stable, and they easily decompose. In acid, they homolyze in the Hofmann-Löffler reaction; in base, they eliminate to the corresponding imines.
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
In thermochemistry, the enthalpy of solution (heat of solution or enthalpy of solvation) is the enthalpy change associated with the dissolution of a substance in a solvent at constant pressure resulting in infinite dilution.
In chemistry, an acid dissociation constant (also known as acidity constant, or acid-ionization constant; denoted ) is a quantitative measure of the strength of an acid in solution.
The reduction of nitroaromatics is conducted on an industrial scale. [1] Many methods exist, such as: Catalytic hydrogenation using: Raney nickel [2] or palladium-on-carbon, [3] [4] [5] platinum(IV) oxide, or Urushibara nickel.
Fe/MnWO 4 + 2 NaOH + 2 H 2 O → Na 2 WO 4 ·2H 2 O + Fe/Mn(OH) 2 Scheelite is treated similarly using sodium carbonate . Sodium tungstate can also be produced by treating tungsten carbide with a mixture of sodium nitrate and sodium hydroxide in a fusion process which overcomes the high exothermicity of the reaction involved.