A solution is prepared by dissolving 0.12 mol of acetic acid and 0.12 mol of ammonium chloride in enough water to make 1.0 L of solution. Find the concentration of ammonia in the solution.
NH4Cl + HAc ==> an acid + an acid
I would set up an ICE chart for HAc (0.12M) and solve for (H^+). Then set up an ICE chart for hydrolysis of NH4^+, use the H^+ from HAc as a common ion and solve for NH3.
NH4^+ + H2O ==> NH3 + H3O^+
To find the concentration of ammonia in the solution, we first need to determine the number of moles of ammonia present.
Based on the chemical equation for the reaction between acetic acid (CH3COOH) and ammonium chloride (NH4Cl):
CH3COOH + NH4Cl → CH3COONH4 + HCl
We can see that 1 mole of ammonium chloride produces 1 mole of ammonia (CH3COONH4).
Therefore, since we have 0.12 moles of ammonium chloride, we also have 0.12 moles of ammonia.
Next, we need to calculate the concentration of ammonia in the solution. Concentration is given in moles per liter (mol/L).
We know the volume of the solution is 1.0 L, and we have 0.12 moles of ammonia.
Therefore, the concentration of ammonia in the solution is:
Concentration = Number of moles / Volume of solution
Concentration = 0.12 mol / 1.0 L
The concentration of ammonia in the solution is 0.12 mol/L.