Calculate the volume of a 0.200 solution that will completely neutralize 40.0 of a 0.264 solution. Where do I begin with this problem?
First you add units. Is that 0.200 M or some other unit? Second, you must know if this is a 1:1 reaction or not.
If M and if 1:1 acid/ base ratios, then
mL acid x M acid = mL base x M base.
To solve this problem, you need to apply the concept of stoichiometry and use the information given. Here are the steps you can follow:
1. Identify the balanced chemical equation for the reaction. This will help you determine the mole-to-mole ratio between the reactants.
2. Calculate the number of moles of the known substance. In this case, you know the volume and concentration of the 0.264 M solution, so you can use the formula: moles = concentration (M) × volume (L).
3. Use the mole-to-mole ratio from the balanced chemical equation to determine the number of moles of the unknown substance that will react.
4. Calculate the volume of the unknown solution using the formula: volume (L) = moles / concentration (M).
Let's go through these steps to solve the problem:
1. Assuming that the acid-base neutralization reaction occurs, we can write the balanced equation as follows:
HX (acid) + NaOH (base) → NaX (salt) + H2O (water)
2. Calculate the number of moles of HX (acid):
moles of HX = concentration of HX × volume of HX
= 0.264 mol/L × 40.0 L
= 10.56 mol HX
3. Based on the balanced equation, the mole-to-mole ratio between HX (acid) and NaOH (base) is 1:1. Therefore, 10.56 moles of HX will react with 10.56 moles of NaOH.
4. Calculate the volume of the 0.200 M NaOH solution needed to react with 10.56 moles of NaOH:
volume = moles / concentration
= 10.56 mol / 0.200 mol/L
= 52.8 L
Therefore, you would need a volume of 52.8 L of the 0.200 M NaOH solution to completely neutralize 40.0 L of the 0.264 M HX solution.