Question

Question: To of 1.00 L of a 100 M AgNO₃ solution is added an excess of sodium chloride. Then 1.00 L of 0.500 M NH₃ (aq) is added. Finally, sufficient nitric acid is added until the pH of the resulting solution is . Write balanced equations for the reactions that take place (if any) at each of three steps in this process.

Short answer

Answer

Balanced equation :

${\left[Ag{\left(N{H}_3\right)}_2\right]}^{+}\left(aq\right)+2H_3{O}^{+}\left(aq\right)+C{l}^{-}\left(aq\right)\to AgCl\left(s\right)+2N{H_4}^{+}\left(aq\right)+2H_{2}O\left(l\right)$

Step-by-step solution

  Given data 

It’s given that;

$$\begin{gathered} {\text{V(AgNO}}_{\text{3}}\text{) = 1.00L} \\ {\text{c(AgNO}}_{\text{3}}\text{) = 0.100M} \\ {\text{V(NH}}_{\text{3}}\text{(aq) = 1.00L} \\ {\text{c(NH}}_{\text{3}}\text{(aq) = 0.500M} \end{gathered}$$

And$\text{pH = 1.0}$

The required chemical equations

First step in this step:

$A{g}^{+}\left(aq\right)+C{l}^{-}\left(aq\right)\to AgCl\left(s\right)$

Second step, where we add $N{H}_3$to the product at the first step:

$AgCl\left(s\right)+2N{H}_3\left(aq\right)\to {\left[Ag{\left(N{H}_3\right)}_2\right]}^{+}\left(aq\right)+C{l}^{-}\left(aq\right)$

In the third step, we add hydroxide ion and chloride ion to the product of the second step where we get the product of the first step :$\left(AgCI\right)$

${\left[Ag{\left(N{H}_3\right)}_2\right]}^{+}\left(aq\right)+2H_3{O}^{+}\left(aq\right)+C{l}^{-}\left(aq\right)\to AgCl\left(s\right)+2N{H_4}^{+}\left(aq\right)+2H_{2}O\left(l\right)$