A titration of 35.0 mL of an unknown tribasic salt, Li₂A, requires 90.00 mL of 0.250 M HCI to reach the 3rd equivalence point. The titration data is shown below: Vol of HCI (mL) 15.00 30.00 45.00 60.00 75.00 90.00 10.45 8.62 6.79 4.86 2.93 1.35 pH Which conjugates are equal in concentrations at midpoint 2? A) [H₂A]=[H₂A] B) [A²]=[H₂A] C) [H₂A]=[HA²] D) [HA²]=[A³] E) None of these

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**Titration of Unknown Tribasic Salt**

A titration of 35.0 mL of an unknown tribasic salt, \(Li_3A\), requires 90.00 mL of 0.250 M HCl to reach the 3rd equivalence point. The titration data is shown below:

| Vol of HCl (mL) | 15.00 | 30.00 | 45.00 | 60.00 | 75.00 | 90.00 |
|-----------------|-------|-------|-------|-------|-------|-------|
| pH              | 10.45 | 8.62  | 6.79  | 4.86  | 2.93  | 1.35  |

**Question:**
Which conjugates are equal in concentrations at midpoint 2?

**Options:**

A) \([H_3A] = [H_2A^-]\)

B) \([A^{2-}] = [H_2A^-]\)

C) \([H_2A^-] = [HA^{2-}]\)

D) \([HA^{2-}] = [A^{3-}]\)

E) None of these

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This educational content explains how to determine the concentration equality of conjugates at the second titration midpoint using titration data for a tribasic salt.
Transcribed Image Text:**Titration of Unknown Tribasic Salt** A titration of 35.0 mL of an unknown tribasic salt, \(Li_3A\), requires 90.00 mL of 0.250 M HCl to reach the 3rd equivalence point. The titration data is shown below: | Vol of HCl (mL) | 15.00 | 30.00 | 45.00 | 60.00 | 75.00 | 90.00 | |-----------------|-------|-------|-------|-------|-------|-------| | pH | 10.45 | 8.62 | 6.79 | 4.86 | 2.93 | 1.35 | **Question:** Which conjugates are equal in concentrations at midpoint 2? **Options:** A) \([H_3A] = [H_2A^-]\) B) \([A^{2-}] = [H_2A^-]\) C) \([H_2A^-] = [HA^{2-}]\) D) \([HA^{2-}] = [A^{3-}]\) E) None of these --- This educational content explains how to determine the concentration equality of conjugates at the second titration midpoint using titration data for a tribasic salt.
Expert Solution
Step 1: Define pH

The question is based on the concept of pH of the solution.  It is defined as a negative logarithm of hydrogen ion concentration present in a solution.

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