Question 9.Q.29: Write an equation for the reaction of each of the following ......
Write an equation for the reaction of each of the following with water:
a. \mathrm{HNO}_{2}
b. \mathrm{HCN}
Step 1:
The given chemical equations are both acid-base reactions involving a weak acid and water.
Step 2:
In both equations, the weak acid donates a proton (H+) to water, forming hydronium ions (H3O+) and the conjugate base of the weak acid.
Step 3:
The equilibrium arrows indicate that the reactions can proceed in both directions, meaning that the hydronium ions can also donate a proton to the conjugate base, forming the weak acid and hydroxide ions.
Step 4:
The equilibrium constant (K) for each reaction can be determined by the concentrations of the reactants and products at equilibrium.
Step 5:
The value of K for each reaction will depend on the strength of the weak acid and the stability of the conjugate base.
Step 6:
Based on the given information, it is not possible to determine the specific values of K for each reaction.
Step 7:
However, it can be concluded that both reactions involve the transfer of a proton between the weak acid and water, resulting in the formation of hydronium ions and the conjugate base.
Step 8:
Therefore, the correct answer is a. [HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2-(aq)] and b. [HCN(aq) + H2O(l) ⇌ H3O+(aq) + CN-(aq)].
Final Answer
a. \mathrm{HNO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q)
b. \mathrm{HCN}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CN}^{-}(a q)
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