Given the following information, what is the concentration of NH3?[NH4Cl](eq) = 1.94 M[HCl](eq) = 1.57 MKc = 0.627NH3(aq) + HCl(aq) ⇌ NH4Cl(aq)0.197 M1.97 M0.297 M2.97 M

The given reaction is: NH3(aq) + HCl(aq) ⇌ NH4Cl(aq)

The equilibrium constant expression for this reaction is: Kc = [NH4Cl] / ([NH3][HCl])

We are given the following equilibrium concentrations:

[NH4Cl] = 1.94 M [HCl] = 1.57 M Kc = 0.627

We are asked to find the concentration of NH3. Let's denote it as [NH3] = x.

Substituting the given values into the equilibrium constant expression, we get:

0.627 = 1.94 / (x * 1.57)

To solve for x, we rearrange the equation:

x = 1.94 / (0.627 * 1.57)

Now, calculate the value of x to get the concentration of NH3.

The given reaction is:

NH3(aq) + HCl(aq) ⇌ NH4Cl(aq)

The equilibrium constant expression for this reaction is:

Kc = [NH4Cl] / ([NH3][HCl])

We are given the equilibrium concentrations of NH4Cl and HCl, and the value of Kc. We can substitute these values into the equilibrium constant expression to solve for the concentration of NH3.

1.94 M = 0.627 / ([NH3] * 1.57 M)

To isolate [NH3], we divide both sides of the equation by 1.57 M:

[NH3] = 0.627 / 1.94 M = 0.323 M

So, the concentration of NH3 at equilibrium is 0.323 M.