Final answer:
To determine the volume of a 0.182 M NaOH solution needed to neutralize a 135 mL solution of 0.121 M HCl and 0.242 M H2SO4, you can use the mole ratio between NaOH and HCl in the balanced chemical equation. By solving for the volume of NaOH using the given molarity and the moles of HCl and H2SO4, you can find the volume in milliliters of the NaOH solution.
Step-by-step explanation:
To determine the volume of a 0.182 M NaOH solution needed to neutralize a 135 mL solution of 0.121 M HCl and 0.242 M H2SO4, we first need to find the moles of HCl and H2SO4 in the given solution. Using the balanced chemical equation HCl(aq) + NaOH(aq) -> NaCl(aq) + H2O(l), we know there is a 1:1 mole ratio between HCl and NaOH. So the moles of HCl is equal to the moles of NaOH needed to neutralize it.
Next, we can use the molarity and volume of NaOH to find the moles of NaOH:
0.182 mol/L NaOH x V NaOH (in L) = 0.121 mol HCl + 0.242 mol H2SO4
Solving for V NaOH, we find:
V NaOH = (0.121 mol HCl + 0.242 mol H2SO4) / 0.182 mol/L NaOH
Finally, we convert V NaOH from liters to milliliters:
V NaOH (in mL) = V NaOH (in L) x 1000 mL/L
Substituting the values:
V NaOH (in mL) = (0.121 mol HCl + 0.242 mol H2SO4) / 0.182 mol/L NaOH x 1000 mL/L
After evaluating this expression, you can find the volume of the 0.182 M NaOH solution needed to neutralize the given solution.
J11