Question

[Tutorial: Titrgtion stoichiometry] This question will walk you through the steps of calculating the volume of titrant required to reach the 3 endpoint based on the volume and concentration of analyte. Consider the standardization of NaOH by titration with C

4
​
H
4
​
O, according to the following chemical reaction: 3NaOH(aq)+ClH
2
​
O(aq)⇌NaC
2
​
H
2
​
O(aq)+3H
4
​
O(1) a Step 1: Evaluate the question. How many moles of aqueous sodium hydroxide (NaCH) 0/0.25 Points Enrned will react to completely neutralize one mole of aqueous citric acid (C
4
​
H
3
​
O−)
−
)? 3/3 Alterrpts Remaining b Which equation will be most helpful for solving this problem? 0/0.25 Points Eamed 3/3 Attempts Remaing Calculate the volume in mL of a 0.200MNaOH solution needed to neutralize 345 mL 0. 0.25 Points Eatned of 0.0333MC C.H.O standard solution. 3/3 Attempts fersaining Based on the fact that NaOH is a strong base and CH
1
​
O is a weak acid. how would you describe the pH of the solution at the endpoint. where moles of base =3 limes the 010.25 Point Earnod molos of acid? 3/3Atteripls Remaring

Answer 1

In the titration of NaOH with C4H4O, the molar ratio between NaOH and C4H4O is 3:1. To calculate the moles of NaOH that react with 1 mole of C4H4O, divide the moles of NaOH by the molar ratio. To calculate the volume of a 0.200 M NaOH solution needed to neutralize 345 mL of a 0.0333 M C4H4O solution, use the equation Moles of NaOH = Molarity of NaOH * Volume of NaOH.

Step-by-step explanation:

In the titration of NaOH with C4H4O, the molar ratio between NaOH and C4H4O is 3:1. This means that for every 3 moles of NaOH, 1 mole of C4H4O is neutralized. To calculate the moles of NaOH that react with 1 mole of C4H4O, simply divide the moles of NaOH by the molar ratio. Therefore, 1 mole of C4H4O would react with 3 moles of NaOH.

To calculate the volume of a 0.200 M NaOH solution needed to neutralize 345 mL of a 0.0333 M C4H4O solution, you can use the equation:

Moles of NaOH = Molarity of NaOH * Volume of NaOH

Then, use the moles of NaOH and the molar ratio to calculate the volume:

Volume of NaOH = Moles of NaOH / Molarity of NaOH

Answer 2

To determine the volume of NaOH titrant required for neutralization, calculate the moles of citric acid using its given concentration and volume, apply the stoichiometric ratio from the reaction equation, and then calculate the volume of NaOH solution needed using its molarity.

Step-by-step explanation:

The process of calculating the volume of titrant required to reach the endpoint in a titration involves understanding the stoichiometry of the reaction between the titrant and the analyte. In the given example, the stoichiometric equation provided is:

NaOH(aq) + ClH₂O(aq) ⇌ NaCl (aq) + H₂O(l)

From the equation, we can infer that:

1. One mole of NaOH neutralizes one mole of ClH₂O.
2. To calculate the moles of NaOH required, we use the molarity of the NaOH solution and the volume of NaOH added to the unknown citric acid solution in the titration.
3. The pH at the endpoint of the titration will be neutral (pH = 7.00) because no acid-base ionization remains, as only water and NaCl are present, which do not undergo acid-base ionization themselves.

For example, to calculate the volume of a 0.200 M NaOH needed to neutralize 345 mL of a 0.0333 M citric acid solution, we apply the following steps:

• Determine the moles of citric acid using its volume and concentration.
• Use the stoichiometric ratio to find the moles of NaOH needed.
• Calculate the volume of NaOH solution based on its molarity and the moles required for neutralization.