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Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed.
Instructions:
Enter all substances in the order listed at the top of the column.Use a carot to indicate a superscript, but do nothing for subscripts.Use a hyphen + greater than (->) for yields.Click on the eye symbol to check your formatting.Report K to three sig figs even though it is good to only two.Group 1A and 7A ions (except fluoride) are spectator ions.
Reactants Rxn: Acid(1) + Base(2) = Base(1) + Acid(2) K (three sig figs)
acetic acid + ammonia
perchloric acid + sodium cyanide
formic acid (HCHO2) + sodium nitrite
Na2HPO4 + KClO
H2SO3 + K2SO4
At 25C, H2O2 decomposes according to the following equation. 2H2O2(aq) => 2H2O (l) + O2(g) .55V
It was originally part of my ebook EVERYTHING YOU NEED TO KNOW ABOUT CHEMICAL NOMENCLATURE. If you want more information or a more complete description to include inorganic compounds please see the ebook section of this website.
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