A sample of 7.80L of NH3(ammonia) gas at 22 degrees Celsius and 735torr is bubbled into a 0.350L solution of 0.400M HCl (hydrochloric acid).

The Kb value for NH3 is 1.8x10-5.

Assuming all the NH3 dissolves and that the volume of the solution remains at 0.350L , calculate the pH of the resulting solution.

Use PV = nRT to calculate moles NH3.

Use M x L to calculate moles HCl.
Write the equation to determine how much NH4Cl is formed and how much NH3 or HCl is left. I suspect NH3 is in excess; therefore, I suspect all of the HCl will be used and you will be left with NH4Cl and NH3 which is a buffered solution.
Use the Henderson-Hasselbach equation to solve for the pH. Post your work if you get stuck.

thnaks...

To calculate the pH of the resulting solution, we need to determine the concentration of OH- ions in the solution.

First, let's calculate the number of moles of NH3 gas using the ideal gas law: PV = nRT

Convert the temperature to Kelvin:
22 degrees Celsius = 22 + 273.15 = 295.15 K

Now, rearrange the ideal gas law equation to solve for n (number of moles):
n = PV / RT

Given:
P = 735 torr
V = 7.80 L
R = 0.0821 L·atm/mol·K (universal gas constant)
T = 295.15 K

Substitute the values into the equation:
n = (735 torr * 7.80 L) / (0.0821 L·atm/mol·K * 295.15 K)

Calculate the value of n.

Next, we need to determine the number of OH- ions produced from the reaction between NH3 and H2O. The balanced equation is as follows:
NH3 + H2O -> NH4+ + OH-

Since the stoichiometry is 1:1, the number of moles of OH- ions will be equal to the number of moles of NH3.

Now, calculate the concentration of OH- ions in moles per liter (Molarity, M):
OH- concentration (M) = Number of moles of OH- / Volume of solution (L)

Given:
Volume of solution (V) = 0.350 L

Substitute the values into the equation to find the molarity of OH- ions.

Now, we can use the Kb value for NH3 to calculate the concentration of OH- ions using the equation for Kb:

Kb = [OH-] * [NH4+] / [NH3]

Given:
Kb = 1.8 x 10^-5
[NH4+] (concentration of NH4+) = [OH-] (concentration of OH-)

Substitute the values into the equation:
1.8 x 10^-5 = [OH-]^2 / [NH3]

Now, rearrange the equation to solve for [OH-]:
[OH-]^2 = Kb * [NH3]

Calculate the value of [OH-]:

Finally, we can calculate the pH using the equation:
pH = 14 - pOH

Given the value of pOH, calculate the pH.

Therefore, using the above calculations, you can determine the pH of the resulting solution.