# Problem: 1.00 g CH3NH3Cl (MW = 67.52 g/mol) and 1.00 g Ba(OH) 2∙8H2O (a strong base, MW = 315.47 g/mol) are added to 80 mL of water and dissolved. The resulting solution is diluted to 100 mL with water at 25°C.Calculate the pH of the solution (pKa(CH3NH3+) = 10.62).A. 11.00B. 10.49C. 10.00D. 11.17E. 10.75

###### FREE Expert Solution

We are being asked to calculate the pH of a solution prepared by dissolving 1.00 g CH3NH3Cl (MW = 67.52 g/mol) and 1.00 g Ba(OH) 2∙8H2O (a strong base, MW = 315.47 g/mol) to 80 mL of water. The resulting solution is diluted to 100 mL with water at 25°C.

We will calculate the pH of the solution at the equivalence point using the following steps:

Step 1. Write the chemical equation for the reaction between CH3NH3Cl and Ba(OH)2.
Step 2. Calculate the initial amounts of CH3NH3Cl and Ba(OH)2 in moles before the reaction happens.
Step 3. Construct an ICF Chart.
Step 4. Calculate pH.

Step 1. Write the chemical equation for the reaction between CH3NH3Cl and Ba(OH)2. ###### Problem Details

1.00 g CH3NH3Cl (MW = 67.52 g/mol) and 1.00 g Ba(OH) 2∙8H2O (a strong base, MW = 315.47 g/mol) are added to 80 mL of water and dissolved. The resulting solution is diluted to 100 mL with water at 25°C.

Calculate the pH of the solution (pKa(CH3NH3+) = 10.62).

A. 11.00

B. 10.49

C. 10.00

D. 11.17

E. 10.75