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.
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Write the net ionic equation for the reaction that occurs in this buffer to react away any added HCl (aq).
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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
Add Answer to:
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1)Write the balanced NET IONIC equation for the reaction that occurs when hydrocyanic acid and potassium...
1)Write the balanced NET IONIC equation for the reaction that
occurs when hydrocyanic acid and potassium
hydroxide are combined.
(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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