A 29.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 24.63 mL of NaOH solution is added?
What is the concentration of the unknown H3PO4 solution? The neutralization reaction is
H3PO4(aq)+3NaOH(aq)→3H2O(l)+Na3PO4(
How would I solve this equation?
Thanks!
the neutralization equation:
concAcid*VolumeAcid=concBase*volumebase
29ml*Normality acid=.1M*24.63ml
Normality acid= 2.463/29= 0.085N
molarity acid*3=.085
molarity acid= .028 M
Well, let's dive into this chemistry puzzle, shall we? First things first, we need to determine the number of moles of NaOH that were added to reach the equivalence point.
We have the volume of NaOH solution used, 24.63 mL, but we need to convert that into moles. To do that, we can use the formula:
moles = Molarity x Volume (in liters)
Let's plug in the values, using the molarity of the NaOH solution (0.100 M) and converting the volume in milliliters to liters:
moles of NaOH = 0.100 M x (24.63 mL / 1000 mL)
Now we have the number of moles of NaOH used. Since the neutralization reaction has a 1:1 stoichiometric ratio between NaOH and H3PO4, the moles of NaOH used is equal to the moles of H3PO4 in the original solution.
Now we just need to calculate the concentration of the H3PO4 solution. We know that the volume of the H3PO4 solution used is 29.00 mL, so we can use the formula:
concentration (in M) = moles / volume (in liters)
Plugging in the values:
concentration of H3PO4 = moles of H3PO4 / (29.00 mL / 1000 mL)
Simplify that, and you've got your answer! I hope that helps, and keep up the great work in chemistry!
To solve this equation, you can use the concept of stoichiometry.
First, let's define the stoichiometry of the reaction:
1 mole of H3PO4 reacts with 3 moles of NaOH to produce 3 moles of H2O and 1 mole of Na3PO4.
Given that the volume of NaOH solution added at the equivalence point is 24.63 mL, we can determine the moles of NaOH used.
Step 1: Convert the volume of NaOH solution to moles:
moles of NaOH = volume of NaOH (L) × concentration of NaOH (mol/L)
Since the volume of NaOH is given in mL, we need to convert it to L:
volume of NaOH (L) = 24.63 mL ÷ 1000 mL/L = 0.02463 L
Step 2: Calculate the moles of NaOH:
moles of NaOH = 0.02463 L × 0.100 mol/L = 0.002463 mol
Step 3: Use the stoichiometry of the reaction to determine the moles of H3PO4:
moles of H3PO4 = moles of NaOH ÷ 3
moles of H3PO4 = 0.002463 mol ÷ 3 = 0.000821 mol
Step 4: Calculate the concentration of H3PO4:
concentration of H3PO4 = moles of H3PO4 / volume of H3PO4 (L)
Given that the volume of the unknown H3PO4 solution is 29.00 mL, we need to convert it to L:
volume of H3PO4 (L) = 29.00 mL ÷ 1000 mL/L = 0.02900 L
concentration of H3PO4 = 0.000821 mol / 0.02900 L = 0.02828 M
Therefore, the concentration of the unknown H3PO4 solution is 0.02828 M.
To solve this problem, you need to use the concept of the stoichiometry of the neutralization reaction and the balanced chemical equation.
First, let's determine the number of moles of NaOH used. The volume of the NaOH solution used is 24.63 mL, which can be converted to liters:
24.63 mL * (1 L / 1000 mL) = 0.02463 L
Using the molarity (0.100 M) and volume (0.02463 L) of NaOH, you can calculate the number of moles of NaOH used:
moles of NaOH = molarity of NaOH * volume of NaOH = 0.100 M * 0.02463 L = 0.002463 moles
According to the balanced chemical equation, the stoichiometric ratio between H3PO4 and NaOH is 1:3. This means that one mole of H3PO4 reacts with three moles of NaOH.
Therefore, the moles of H3PO4 present in the solution can be calculated using the stoichiometry:
moles of H3PO4 = moles of NaOH * (1 mol H3PO4 / 3 mol NaOH) = 0.002463 moles * (1 mol H3PO4 / 3 mol NaOH) = 0.000821 moles
Now, we can calculate the concentration of the unknown H3PO4 solution. The concentration is expressed as moles of H3PO4 per liter (mol/L or M):
concentration of H3PO4 = moles of H3PO4 / volume of H3PO4 solution in liters
The volume of the H3PO4 solution is given as 29.00 mL, which can be converted to liters:
29.00 mL * (1 L / 1000 mL) = 0.02900 L
Now we can calculate the concentration:
concentration of H3PO4 = 0.000821 moles / 0.02900 L = 0.0283 M
Therefore, the concentration of the unknown H3PO4 solution is 0.0283 M.