How would you complete and balance the acid base neutralizations reaction: $H_{S} O_{4} + M {g (O H)}_{2} \to$ $H_SO_4 + Mg(OH)_2 ->$ ?

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Answer 1 · 2017-03-27T03:15:14

$H_{2} S O_{4} (a q) + M {g (O H)}_{2} (a q) \to M g S O_{4} (a q) + 2 H_{2} O (l)$ $H_2SO_4(aq) + Mg(OH)_2(aq) rarr MgSO_4(aq) + 2H_2O(l)$

$Well, does garbage in equal garbage out?$ $"Well, does garbage in equal garbage out?"$

The net ionic equation is simply the acid-base reaction:

$H_{3} O^{+} +^{-} O H \to 2 H_{2} O (l)$ $H_3O^+ + ""^(-)OH rarr 2H_2O(l)$

The sulfate and magnesium ions are simply along for the ride.

How would you complete and balance the acid base neutralizations reaction: HSO4+Mg(OH)2→H_SO_4 + Mg(OH)_2 ->?