How do you balance $H_{2} S O_{4} + N H_{4} O H \to H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4$ ?

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How do you balance $H_{2} S O_{4} + N H_{4} O H \to H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4$ ?

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Answer 1 · 2016-06-02T00:23:29

The balanced equation is
$H_{2} S O_{4} + 2 N H_{4} O H \to 2 H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + 2 NH_4OH -> 2 H_2O + (NH_4)_2SO_4$

Explanation:

This is a neutralization equation of an acid $H_{2} S O_{4}$ $H_2SO_4$ , sulfuric acid with a base $N H_{4} O H$ $NH_4OH$ ammonium hydroxide to form water $H_{2} O$ $H_2O$ and a salt ${(N H_{4})}_{2} S O_{4}$ $(NH_4)_2SO_4$ ammonium sulfate.

When balancing a neutralization, balance the water $H_{2} O$ $H_2O$ is $H O H$ $HOH$ and the rest of the equation will balance.

$H_{2} S O_{4} + N H_{4} O H \to H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4$

The 2 $H^{+}$ $H^+$ ions in the acid need 2 $O H^{-}$ $OH^-$ ions to form 2 water molecules $H O H$ $HOH$ or $H_{2} O$ $H_2O$

Therefore the equation balances at

$H_{2} S O_{4} + 2 N H_{4} O H \to 2 H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + 2 NH_4OH -> 2 H_2O + (NH_4)_2SO_4$

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How do you balance $H_{2} S O_{4} + N H_{4} O H \to H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4$ ?

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How do you balance H2SO4+NH4OH→H2O+(NH4)2SO4H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4?

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How do you balance $H_{2} S O_{4} + N H_{4} O H \to H_{2} O + {(N H_{4})}_{2} S O_{4}$ $H_2SO_4 + NH_4OH -> H_2O + (NH_4)_2SO_4$ ?