A chemist performs an acid–base titration using 0.176 M aqueous NaOH as the titrant with 26.15 mL of 0.102 M H2SO4. The endpoint of the titration is detected using phenolphthalein as the indicator.
The balanced equation for the reaction is shown below:
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What volume of NaOH is expected to be required to consume all of the acid initially present?
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
mols H2SO4 = M x L = 0.102 x 0.02615 = ?
Using the coefficients in the balanced equation, convert mols H2SO4 to mols NaOH. That is 2 mol NaOH to 1 mol H2SO4; therefore, mols NaOH = 2 x mols H2SO4.
Then M NaOH = mols NaOH/L NaOH. You know M and mols, solve for L and convert to mL if desired.
Post your work if you get stuck.
To determine the volume of NaOH required to consume all of the acid initially present, we first need to calculate the moles of acid present.
The balanced equation for the reaction between NaOH and H2SO4 is as follows:
2 NaOH + H2SO4 → Na2SO4 + 2 H2O
From the equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4.
Given:
- Volume of H2SO4 solution = 26.15 mL
- Concentration of H2SO4 solution = 0.102 M
First, let's convert the volume of H2SO4 solution to liters:
26.15 mL = 26.15 mL * (1 L / 1000 mL) = 0.02615 L
Now, let's calculate the moles of H2SO4 using the concentration and volume:
moles of H2SO4 = concentration * volume
= 0.102 M * 0.02615 L
= 0.0026693 mol
Since the stoichiometry of the balanced equation shows us that 2 moles of NaOH react with 1 mole of H2SO4, we can use this ratio to determine the moles of NaOH required to consume all of the acid initially present.
moles of NaOH = 2 * moles of H2SO4
= 2 * 0.0026693 mol
= 0.0053386 mol
Now, let's calculate the volume of NaOH using its molarity:
volume of NaOH = moles of NaOH / concentration
= 0.0053386 mol / 0.176 M
≈ 0.0303 L
Finally, let's convert the volume of NaOH from liters to milliliters:
volume of NaOH = 0.0303 L * (1000 mL / 1 L)
≈ 30.3 mL
Therefore, approximately 30.3 mL of NaOH is expected to be required to consume all of the acid initially present.
To find the volume of NaOH required to consume all of the acid initially present, we need to use the balanced equation and the given concentrations and volumes of the acid and NaOH.
The balanced equation for the reaction between NaOH and H2SO4 is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, we can see that the stoichiometric ratio between NaOH and H2SO4 is 2:1. This means that for every 2 moles of NaOH, we need 1 mole of H2SO4.
First, we need to determine the number of moles of H2SO4 present in the given volume of 0.102 M H2SO4 solution:
Moles of H2SO4 = concentration (M) × volume (L)
= 0.102 M × (26.15 mL / 1000 mL/L)
= 0.0026793 moles
Since the stoichiometric ratio between NaOH and H2SO4 is 2:1, we know that we need double the number of moles of NaOH to completely react with the H2SO4. Therefore, the number of moles of NaOH required is:
Moles of NaOH = 2 × moles of H2SO4
= 2 × 0.0026793 moles
= 0.0053586 moles
Now, we can use the concentration of the NaOH solution to find the volume of NaOH required to consume all of the acid initially present:
Volume of NaOH = Moles of NaOH / Concentration of NaOH
= 0.0053586 moles / 0.176 M
= 0.0304409 L (or 30.4409 mL)
Therefore, the expected volume of NaOH required to consume all of the acid initially present is approximately 30.4409 mL.