1. Write the net ionic equation for the reaction that occurs when equal volumes
ID: 965008 • Letter: 1
Question
1. Write the net ionic equation for the reaction that occurs when equal volumes of 0.256 M aqueous hypochlorous acid and sodium fluoride are mixed (there should be 2 spots before and after arrows)
at equilibrium is it product or react favored
and is the ph <, =, or > than 7?
2. Write the balanced NET IONIC equation for the reaction that occurs when hydrochloric acid and potassium cyanide are combined. (there should be 2 spots on both sides of arrows)
Also, is the reaction classified as: strong acid + strong base, weak acid + strong base, strong acid + weak base, or weak acid + weak base?
The extent of this reaction is: below 50, 50, above 50, or 100%?
3. Write the balanced net ionic equation for he reaction that occurs when acetic acid and barium hydroxide are combined. (2 on the left and 3 spots on the right of arrows)
Also, is the reaction classified as: strong acid + strong base, weak acid + strong base, strong acid + weak base, or weak acid + weak base?
The extent of this reaction is: below 50, 50, above 50, or 100%?
Explanation / Answer
Sol:-
Chemical equation is :-
HClO (aq) + NaF (aq) <------------> NaClO (aq) + HF (aq)
HClO and HF are weak acids i.e weak electrolytes and we know weak electrolytes do not completely dissociated into its ions in aqueous solution .
NaF and NaClO are strong electrolytes and strong electrolytes are completely dissociated into its ions in aqueous solution.
therefore Ionic equation is :-
HClO (aq) + Na+ (aq) + F-(aq) <--------------> Na+(aq) + ClO- (aq) + HF (aq)
and Net ionic equation after the cancellation of Na+ (aq) on both side is :-
HClO (aq) + F-(aq) <--------------> ClO- (aq) + HF (aq)
Ka value of HF = 6.6 x 10-4 and
Ka value of HClO = 2.9 x 10-8
Ka of HF > Ka of HClO therefore HF is stronger acid than HClO and hence equilibrium will shifts in backward direction i.e reactant side . backward reaction forms acidic buffer solution in which HF act as weak acid while F- act as its conjugate base therefore pH of the solution will be acidic i.e pH < 7 and exact pH value of acidic buffer solution can be calculated by using Henderson-Hasselbalch equation .
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