Complete the equations for the following equilibria, calculate Ke for each reaction and express its value in proper scientific notation. (a) ammonia (acting as a base) reacts with water (acting as an acid) Kc = ammonia as base: NH3 + H₂O= (b) ammonia (acting as an acid) reacts with water (acting as a base) ammonia as acid: NH3 + H₂O= Species NH3 NH pKa 35 9.25

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**Equilibrium Reactions Involving Ammonia and Water**

Complete the equations for the following equilibria, calculate \( K_c \) for each reaction and express its value in proper scientific notation.

**(a) Ammonia (acting as a base) reacts with water (acting as an acid):**

- **Equilibrium Reaction:**  
  \(\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons\)

- **Equilibrium Constant (\( K_c \)):**  
  \[ \boxed{} \]

**(b) Ammonia (acting as an acid) reacts with water (acting as a base):**

- **Equilibrium Reaction:**  
  \(\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons\)

- **Equilibrium Constant (\( K_c \)):**  
  \[ \boxed{} \]

**Species and \( pK_a \) values:**

\[
\begin{array}{|c|c|}
\hline
\text{Species} & pK_a \\
\hline
\text{NH}_3 & 35 \\
\text{NH}_4^+ & 9.25 \\
\hline
\end{array}
\]

This exercise involves completing and analyzing the given equilibrium reactions where ammonia acts in different roles, either as a base or an acid. The \( pK_a \) values of the involved species are provided to assist in these calculations.
Transcribed Image Text:**Equilibrium Reactions Involving Ammonia and Water** Complete the equations for the following equilibria, calculate \( K_c \) for each reaction and express its value in proper scientific notation. **(a) Ammonia (acting as a base) reacts with water (acting as an acid):** - **Equilibrium Reaction:** \(\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons\) - **Equilibrium Constant (\( K_c \)):** \[ \boxed{} \] **(b) Ammonia (acting as an acid) reacts with water (acting as a base):** - **Equilibrium Reaction:** \(\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons\) - **Equilibrium Constant (\( K_c \)):** \[ \boxed{} \] **Species and \( pK_a \) values:** \[ \begin{array}{|c|c|} \hline \text{Species} & pK_a \\ \hline \text{NH}_3 & 35 \\ \text{NH}_4^+ & 9.25 \\ \hline \end{array} \] This exercise involves completing and analyzing the given equilibrium reactions where ammonia acts in different roles, either as a base or an acid. The \( pK_a \) values of the involved species are provided to assist in these calculations.
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