A solution is prepared using 15.0 mL of 1.0 M HCl and 20.0 mL of 0.5 M HNO3. The final volume of the solution is 1.25 L. What are the [H3O+] and [OH-] in the final solution? What is the pH of the final solution?
Ok. I got 0.015 mol HCl and 0.1 mol HNO3. Do I just add the moles to get the total? So 0.115 total moles. Which would make a the Molarity of the final solution 0.092M?
add the moles, in reality you are adding the H+ concentrations.
It is the concentration of H+ which determines pH
ok thankyou!
for what works the 1.25L that they give you in the problem?
never mind, just figure it out
To calculate the molarity of the final solution, you need to add the moles of acid from HCl and HNO3 and divide it by the final volume of the solution.
First, let's calculate the moles of acid from HCl:
Moles of HCl = Volume of HCl (in liters) × Concentration of HCl
= 15.0 mL ÷ 1000 mL/L × 1.0 mol/L
= 0.015 mol
Next, let's calculate the moles of acid from HNO3:
Moles of HNO3 = Volume of HNO3 (in liters) × Concentration of HNO3
= 20.0 mL ÷ 1000 mL/L × 0.5 mol/L
= 0.01 mol
Now, add the moles of HCl and HNO3 together to get the total moles of acid:
Total moles of acid = Moles of HCl + Moles of HNO3
= 0.015 mol + 0.01 mol
= 0.025 mol
To determine the molarity of the final solution, divide the total moles of acid by the final volume of the solution:
Molarity of the final solution = Total moles of acid ÷ Final volume of solution
= 0.025 mol ÷ 1.25 L
= 0.02 M
Therefore, the molarity of the final solution is 0.02 M.