****I have attempted these all on my own and I cannot get them correct. Please o
ID: 879256 • Letter: #
Question
****I have attempted these all on my own and I cannot get them correct. Please only respond if you are confident in your answer, because I only have a few attempts allowed. Also, I am looking for a good explanation of how to work these out on my own*****
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.
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 hydrochloric acid + sodium hydroxide hydrazoic acid + sodium hypochlorite KHSO4 + NH3 H2S + KClOExplanation / Answer
1)
CH3COOH(Bronsted acid) + NH3(Bronsted base) ------------> CH3COO^-(conjugate base) + NH4^+(conjugate acid)
K = [CH3COO^-][ NH4^+] / [CH3COOH][NH3]
2)
HCl (Bronsted acid)+ NaOH (Bronsted base) ------------> NaCl (conjugate base)+ H2O (conjugate acid)
K = [ NaCl][H2O] / [HCl ][NaOH]
3)
N3H (Bronsted acid)+ NaOCl (Bronsted base) ------------> HOCl (conjugate base) + NaN3 (conjugate acid)
K = [HOCl ][NaN3] / [N3H][NaOCl]
4)
KHSO4 here K+ spectator ion so leave that
HSO4^- (Bronsted acid)+ NH3 (Bronsted base) ------------> SO4^2- (conjugate base)+ NH4^+ (conjugate acid)
K = [SO4^2-][NH4^+] / [HSO4^-][ NH3]
5)
H2S (Bronsted acid)+ ClO^- (Bronsted base) -------------> HS^- (conjugate base) + HOCl (conjugate acid)
K = [HS^-][HOCl] / [H2S][ ClO^-]
Note: here you did not mention the numerical values so i could not solve K in values.
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