The solution was created by dissolving .34 mol Na(OH) and 0.15 miles Ca(OH)2 in water. The final volume of the solution was 2.5 L. calculate the pH of the solution.

Answer 1

To find the pH of the solution, we first need to calculate the total concentration of hydroxide ions (OH-) in the solution.

Given:
- Na(OH) moles = 0.34 mol
- Ca(OH)2 moles = 0.15 mol
- Total volume of solution = 2.5 L

1. Calculate the total moles of hydroxide ions:
- Na(OH) contributes 1 mole of OH- for every mole
- Ca(OH)2 contributes 2 moles of OH- for every mole

Total moles of OH- = (0.34 mol Na(OH) * 1 mol OH-) + (0.15 mol Ca(OH)2 * 2 mol OH-) = 0.34 mol + 0.30 mol = 0.64 mol

2. Calculate the concentration of hydroxide ions:
- Concentration = Total moles / Total volume = 0.64 mol / 2.5 L = 0.256 M

3. Calculate pOH:
- pOH = -log[OH-] = -log(0.256) = 0.59

4. Calculate pH:
- pH = 14 - pOH = 14 - 0.59 = 13.41

Therefore, the pH of the solution is approximately 13.41.