What volume of 0.406 M KOH is required to completely react with 18.50 mL of 0.287 M H2SO4?
H2SO4 + 2KOH ==> K2SO4 + 2H2O
moles H2SO4 initially = M x L = ??
moles KOH (from the equation) = 2x that.
M KOH = moles KOH/L soln.
You have M and moles, solve for L and convert to mL.
1.683
To determine the volume of 0.406 M KOH required to completely react with 18.50 mL of 0.287 M H2SO4, you need to use the stoichiometry and the concept of molarity.
Step 1: Write the balanced chemical equation for the reaction between KOH and H2SO4:
2 KOH + H2SO4 -> K2SO4 + 2 H2O
Step 2: Determine the mole ratio between KOH and H2SO4. From the balanced chemical equation, the mole ratio is 2:1. This means that for every 2 moles of KOH, 1 mole of H2SO4 reacts.
Step 3: Calculate the number of moles of H2SO4 in 18.50 mL of 0.287 M H2SO4. The molarity (M) is given as 0.287 M, which means there are 0.287 moles of H2SO4 in 1 liter (1000 mL) of solution. Therefore, the number of moles of H2SO4 in 18.50 mL can be calculated as follows:
moles of H2SO4 = (0.287 mol/L) * (18.50 mL / 1000 mL) = 0.0053095 moles
Step 4: Use the mole ratio to calculate the number of moles of KOH required to react with the given moles of H2SO4. Since the mole ratio of KOH to H2SO4 is 2:1, the number of moles of KOH required is twice the number of moles of H2SO4:
moles of KOH = 2 * 0.0053095 moles = 0.010619 moles
Step 5: Calculate the required volume of 0.406 M KOH solution using the equation:
Volume (L) = moles / Molarity
Volume = 0.010619 moles / 0.406 mol/L = 0.02611 L
Since we want the volume in milliliters (mL), we multiply by 1000:
Volume = 0.02611 L * 1000 mL/L = 26.11 mL
Therefore, approximately 26.11 mL of 0.406 M KOH solution is required to completely react with 18.50 mL of 0.287 M H2SO4.