Chemical Forums

Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: raafiki on October 15, 2012, 09:10:39 PM

Title: net Bronsted equations
Post by: raafiki on October 15, 2012, 09:10:39 PM

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
sulfuric acid + sodium carbonate
nitrous acid + sodium fluoride
Na2HPO4 + KClO
H2SO3 + K2SO4


I cant figure out the equations:/ Please *delete me* I keep getting it wrong!
Also, how do you figure our K if you dont have any quantitative data given?..

Title: Re: net Bronsted equations
Post by: Borek on October 16, 2012, 03:33:05 AM

You are probably expected to calculate K constants from Ka/Kb values you were given in separate tables.

Writing reactions is about identifying acids and bases. What is the acid in the first reaction? What is the base?