Education • All: 4.3: Neutralization Reactions

NEUTRALIZATION REACTIONS

ACID (H+) + BASE (OH-) -------> SALT (Ionic compound) + WATER

STRONG ACIDS: Completely ionize, that is they are soluble in water.

HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4

All other acids are weak and therefore they stay together in H2O (do not separate as ions)

Example:

MOLECULAR EQUATION:

$\large \fn_cm 2CH_{3}COOH\;\;+\;\;Ba(OH)_{2}\;\;\rightarrow \;\;(CH_{3}COO)_{2}Ba\;\;+\;\;2H_{2}O$

IONIC EQUATION:

$\dpi{120} \fn_cm 2CH_{3}COOH\;+\;\underline{Ba^{2+}}\;+\;2OH^{-}\;\rightarrow \;(2CH_{3}COO)^{-}\;+\;\underline{Ba^{2+}}\;+\;2H_{2}O$

NET IONIC EQUATION:

$\dpi{120} \fn_cm 2CH_{3}COOH\;\;+\;\;2OH^{-}\;\rightarrow \;(2CH_{3}COO)^{-}\;\;+\;\;2H_{2}O$

NEUTRALIZATION REACTION WITH GAS FORMATION

#1.

ACID (H+) + METAL SULFIDE -------> SALT + HYDROSULFURIC ACID

HCl + Na2S -------> NaCl + H2S

ACID (H+) + METAL CARBONATE -------> SALT + CARBONIC ACID

HCl + Na2CO3 -------> NaCl + H2CO3

#3.

ACID (H+) + METAL SULFITE -------> SALT + SULFURIC ACID

HCl + Na2CO3 -------> NaCl + H2SO3

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4.3: Neutralization Reactions

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