A sample of 7.80 L of (ammonia) gas at 22 C and 735 torr is bubbled into a 0.500L solution of 0.400 M HCl (hydrochloric acid). The Kb value for is 1.8 *10^-5.

Assuming all the NH3 dissolves and that the volume of the solution remains at 0.500 L, calculate the pH of the resulting solution.

Question

A sample of 7.80 L  of  (ammonia) gas at 22 C and 735 torr is bubbled into a 0.500L  solution of 0.400 M HCl   (hydrochloric acid). The Kb value for  is 1.8 *10^-5. 

Assuming all the NH3 dissolves and that the volume of the solution remains at 0.500 L, calculate the pH  of the resulting solution.

jfraser · Answer

use the ideal gas law to find moles of NH3. Use the concentration and volume of the solution to find moles of HCl. Now you have moles of each, you have a limiting reactant problem. Find the reactant that's left over, and plug it into a RICE box (or ICE table) and solve for an equilibruim concentration of H+. Find pH from the [H+]

anonymous · Answer

Thank you very much