hello this is ellie again. I need help on this one problem A solution of 0.314M KOH is used to neutralize 10.0mL H3PO4 solution.
H3PO4(aq) + 3KOH(aq) → K3PO4(aq) + 3H2O(l) If 29.3mL KOH solution is required to reach the endpoint, what is the molarity of the H3PO4 solution? I got .3215 but that isn't correct. What is the correct way to solve this problem?
See your post below.
To solve this problem, you can use the concept of stoichiometry and the equation provided to determine the molarity of the H3PO4 solution.
First, let's calculate the moles of KOH used. Since we know the concentration of the KOH solution (0.314M) and the volume used (29.3 mL), we can use the formula:
moles of KOH = concentration × volume
= 0.314 mol/L × 0.0293 L
= 0.00919 mol
From the balanced equation, we can see that the molar ratio between KOH and H3PO4 is 3:1. This means that for every 3 moles of KOH, there is 1 mole of H3PO4.
Using the molar ratio, we can calculate the moles of H3PO4:
moles of H3PO4 = moles of KOH × (1/3)
= 0.00919 mol × (1/3)
= 0.00306 mol
Now, we need to determine the volume of the H3PO4 solution used. We know that the KOH solution used was 29.3 mL and that the molar ratio between KOH and H3PO4 is 1:1. Therefore, the volume of the H3PO4 solution used is also 29.3 mL.
Next, we can calculate the molarity of the H3PO4 solution using the formula:
molarity of H3PO4 = moles of H3PO4 / volume of H3PO4 solution
= 0.00306 mol / 0.0293 L
= 0.104 M
Therefore, the molarity of the H3PO4 solution is 0.104 M.
It seems that your previous answer of 0.3215 was incorrect. Double-check your calculations, specifically when calculating the moles of H3PO4 and the volume of the H3PO4 solution.