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phew, too much edits in one post, need to take a break...
Gaurang Tandon
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$$\ce{2 NH4OH(aq) + H2SO4(aq) -> (NH4)2SO4(aq) + 2 H2O(l)}$$

This is an acid base reaction. $$\ce{NH4}$$ compounds are always water-soluble, so no precipitate, and no color change will be observed. Neutralization reactions like the one above are generally exothermic (they release heat).

This can be proved by observing their heats of formation:

• $$\Delta H_{f(\ce{(NH4)2SO4})} = \pu{-1181 kJ/mol * 1 mol = -1181 kJ}$$
• $$\Delta H_{f(\ce{H2O(l))}} = \pu{-285.8 kJ/mol * 2 mol = -571.6 kJ}$$
• $$\Delta H_{f(H2SO4)} = \pu{-909 kJ/mol * 1 mol = -909 kJ}$$
• $$\Delta H_{f(NH4OH)} = \pu{-80.8 kJ/mol * 2 mol = -161.6 kJ}$$

Thus the $$\Delta H_{rxn}=\pu{(-1181 kJ + -571.6 kJ) - ( -909 kJ + -161.6 kJ) = -682 kJ}$$ is negative, hence the reaction is exothermic.