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. what are the molar concentrations of Na and Ca in the final solution?
To find the molar concentrations of Na and Ca in the final solution, we first need to calculate the moles of Na and Ca present in the solution.
Moles of Na(OH): 0.34 mol
Moles of Ca(OH)2: 0.15 mol (since each mole of Ca(OH)2 contains 2 moles of OH- ions)
Total moles of OH- ions present in the solution:
0.34 mol (from Na(OH)) + 0.15 mol * 2 (from Ca(OH)2) = 0.64 mol
Since NaOH and Ca(OH)2 are strong electrolytes, they dissociate completely in water to form Na+, Ca2+, and OH- ions.
Molar concentration of Na+ ions:
Concentration of Na+ ions = moles of Na+ ions / volume of solution
Concentration of Na+ ions = 0.34 mol / 2.5 L = 0.136 M
Molar concentration of Ca2+ ions:
Concentration of Ca2+ ions = moles of Ca2+ ions / volume of solution
Concentration of Ca2+ ions = 0.15 mol / 2.5 L = 0.06 M
Therefore, the molar concentration of Na+ ions in the final solution is 0.136 M and the molar concentration of Ca2+ ions is 0.06 M.