A solution of nitrous acid and potassium nitrite acts as a buffer due to reactions that occur within the solution when a strong acid or a strong base is added.
-
Write the net ionic equation for the reaction that occurs in this buffer to react away any added HCl (aq).
-
Write the net ionic equation for the reaction that occurs in this buffer to react away any added NaOH (aq).
Homework Answers
HNO2 + KNO2 is acid buffer solution
HNO2(aq) <-------------> H^+ (aq) + NO2^- (aq)
KNO2(aq) ----------> K^+ (aq) + NO2^- (aq)
By adding of strong acid HCl
NO2^- (aq) + HCl ((aq) --------> HNO2(aq) + Cl^-(aq) (aq)
Or
NO2^- (aq) + H^+ --------------> HNO2(aq) Net ionic equation
2.
By adding strong base NaOH
H^+ (aq) + OH^- (aq) -------------> H2O(l) net ionic equation
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(aq)(s)(l)(g)
+
(aq)(s)(l)(g)
(aq)(s)(l)(g)
+
(aq)(s)(l)(g)
+
(aq)(s)(l)(g)
This reaction is classified as .
A. Strong Acid + Strong Base
B. Weak Acid + Strong Base
C. Strong Acid + Weak Base
D. Weak Acid + Weak Base
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Use H3O+ instead of
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