Questions: b. If the molarity of the based added from the buret was 0.200 M , determine the volume of the base (in ml required to reach the end point of this titration.

b. If the molarity of the based added from the buret was 0.200 M , determine the volume of the base (in ml required to reach the end point of this titration.
Transcript text: b. If the molarity of the based added from the buret was 0.200 M , determine the volume of the base (in ml required to reach the end point of this titration.
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Solution

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Solution Steps

To solve this problem, we need to determine the volume of a base required to reach the endpoint of a titration. However, the problem does not provide information about the acid being titrated or the stoichiometry of the reaction. For the sake of this solution, let's assume we are titrating a monoprotic acid with a strong base.

Step 1: Understand the Reaction

Assume the reaction is between a monoprotic acid (HA) and a strong base (BOH), such as NaOH. The balanced chemical equation is: \[ \text{HA} + \text{BOH} \rightarrow \text{BA} + \text{H}_2\text{O} \]

Step 2: Use the Molarity Formula

The molarity formula is: \[ M_1V_1 = M_2V_2 \] where \( M_1 \) and \( V_1 \) are the molarity and volume of the acid, and \( M_2 \) and \( V_2 \) are the molarity and volume of the base.

Step 3: Solve for the Volume of the Base

Given:

  • \( M_2 = 0.200 \, \text{M} \)
  • Assume \( M_1 \) and \( V_1 \) are known for the acid.

Rearrange the formula to solve for \( V_2 \): \[ V_2 = \frac{M_1V_1}{M_2} \]

Final Answer

Without specific values for \( M_1 \) and \( V_1 \), we cannot calculate a numerical answer. However, the formula to find the volume of the base required is: \[ \boxed{V_2 = \frac{M_1V_1}{0.200}} \]

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