[Safarinoise137]

Im in the chapter about acid, bases and equilibrium.
HCl + NH3
Both are solutions in water.
[HCl] = 0,122 mol/L
[NH3] = (What I need to find out)
To reach the equilibrium, we use 0,023 L of HCl and 0,02 L of NH3.
What is the concentration of NH3.

If I'm doing it correctly, it should be:
0,122 mol/L * 0,023L = 0,002806 moles.
NH3 should have the same amount of moles at the equilibrium. [NH3] = 0,002806moles ÷ 0.02L = 0,1403 moles/L.
Is this correct or am I doing something wrong? And what is the pH at the equilibrium?

[hypervalent_iodine]

Im in the chapter about acid, bases and equilibrium.
HCl + NH3
Both are solutions in water.
[HCl] = 0,122 mol/L
[NH3] = (What I need to find out)
To reach the equilibrium, we use 0,023 L of HCl and 0,02 L of NH3.
What is the concentration of NH3.

If I'm doing it correctly, it should be:
0,122 mol/L * 0,023L = 0,002806 moles.
NH3 should have the same amount of moles at the equilibrium. [NH3] = 0,002806moles ÷ 0.02L = 0,1403 moles/L.
Is this correct or am I doing something wrong? And what is the pH at the equilibrium?

I didn't check your math, but your process looks fine to me.

For the pH part, the questions you need to think about are what forms when you react HCl with NH₃, and what can you say about the product that forms in terms of its acidity or basicity?