Determine how many mL of 0.102 mol NaOH solution is needed to neutralize 35.0 mL of 0.125 mol H2SO4 solution.
See your previous post. Post you work if you still have questions. It's the same concept. Four steps.
1. Write and balance the equation.
2. Calculate mols of what you have. That's the H2SO4.
3. Using the coefficients in the balanced equation, convert mols of what you have to mols of what you want. That's convert mols H2SO4 to mols NaOH.
4. M NaOH= mols NaOH/L NaOH. You have M NaOH and mols NaOH, solve for L NaOH and convert to mL.
To determine how many mL of 0.102 mol NaOH solution is needed to neutralize 35.0 mL of 0.125 mol H2SO4 solution, we can use the concept of stoichiometry and the balanced equation of the reaction between NaOH and H2SO4.
The balanced equation is:
2 NaOH + H2SO4 → Na2SO4 + 2 H2O
From the balanced equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4. This means that the mole ratio of NaOH to H2SO4 is 2:1.
First, we need to determine the number of moles of H2SO4 present in the given solution:
moles of H2SO4 = volume of H2SO4 solution (in L) × molarity of H2SO4 solution
Given that the volume of H2SO4 solution is 35.0 mL (0.0350 L) and the molarity of H2SO4 solution is 0.125 mol/L:
moles of H2SO4 = 0.0350 L × 0.125 mol/L = 0.004375 mol H2SO4
Since the mole ratio of NaOH to H2SO4 is 2:1, the number of moles of NaOH required is twice the number of moles of H2SO4:
moles of NaOH = 2 × moles of H2SO4 = 2 × 0.004375 mol NaOH = 0.00875 mol NaOH
Now, we can determine the volume of 0.102 mol NaOH solution needed, using the molarity of NaOH:
volume of NaOH solution (in L) = moles of NaOH / molarity of NaOH solution
Given that the molarity of NaOH solution is 0.102 mol/L:
volume of NaOH solution = 0.00875 mol NaOH / 0.102 mol/L = 0.0858 L = 85.8 mL
Therefore, approximately 85.8 mL of 0.102 mol NaOH solution is needed to neutralize 35.0 mL of 0.125 mol H2SO4 solution.