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Phosphorous acid, H, PO, (aq), is a diprotic oxyacid that is an important compound in industry and agriculture. pKal pKa2 но -HO- 1.30 6.70 Calculate the pH for each of the points in the titration of 50.0 mL of 1.8 M H,PO, (aq) with 1.8 M KOH(aq). before addition of any KOH: 0.05 after addition of 25.0 mL KOH: 1.3 Incorrect after addition of 50.0 mL KOH: 4.0 after addition of 75.0 mL KOH: 6.7 after addition of 100.0 mL KOH: 10.32

Phosphorous acid, H, PO, (aq), is a diprotic oxyacid that is an important compound in industry and agriculture. pKal pKa2 но -HO- 1.30 6.70 Calculate the pH for each of the points in the titration of 50.0 mL of 1.8 M H,PO, (aq) with 1.8 M KOH(aq). before addition of any KOH: 0.05 after addition of 25.0 mL KOH: 1.3 Incorrect after addition of 50.0 mL KOH: 4.0 after addition of 75.0 mL KOH: 6.7 after addition of 100.0 mL KOH: 10.32

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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### Phosphorous Acid Titration with KOH **Phosphorous acid, \( \text{H}_3\text{PO}_3 (\text{aq}) \),** is a diprotic oxyacid that serves as an important compound in both industry and agriculture. **Dissociation Constants:** - \( pK_{a1} = 1.30 \) - \( pK_{a2} = 6.70 \) **Molecular Structure:** The structure of phosphorous acid includes an atom of phosphorus (P) bonded to two hydroxy groups (OH) and one hydrogen (H) atom, along with a double-bonded oxygen (O). **Titration Details:** Calculate the pH at various points during the titration of \( 50.0 \, \text{mL} \) of \( 1.8 \, \text{M} \, \text{H}_3\text{PO}_3 (\text{aq}) \) with \( 1.8 \, \text{M} \, \text{KOH} (\text{aq}) \). **pH Calculations at Specific Volumes of KOH Added:** - **Before addition of any KOH:** - Incorrect trial: \( 0.05 \) - **After addition of 25.0 mL KOH:** - pH = 1.3 - **After addition of 50.0 mL KOH:** - pH = 4.0 - **After addition of 75.0 mL KOH:** - pH = 6.7 - **After addition of 100.0 mL KOH:** - pH = 10.32 This information is critical for understanding the titration curve, behavior of phosphorous acid, and for calculating the point at which neutralization occurs with potassium hydroxide.
Transcribed Image Text:### Phosphorous Acid Titration with KOH **Phosphorous acid, \( \text{H}_3\text{PO}_3 (\text{aq}) \),** is a diprotic oxyacid that serves as an important compound in both industry and agriculture. **Dissociation Constants:** - \( pK_{a1} = 1.30 \) - \( pK_{a2} = 6.70 \) **Molecular Structure:** The structure of phosphorous acid includes an atom of phosphorus (P) bonded to two hydroxy groups (OH) and one hydrogen (H) atom, along with a double-bonded oxygen (O). **Titration Details:** Calculate the pH at various points during the titration of \( 50.0 \, \text{mL} \) of \( 1.8 \, \text{M} \, \text{H}_3\text{PO}_3 (\text{aq}) \) with \( 1.8 \, \text{M} \, \text{KOH} (\text{aq}) \). **pH Calculations at Specific Volumes of KOH Added:** - **Before addition of any KOH:** - Incorrect trial: \( 0.05 \) - **After addition of 25.0 mL KOH:** - pH = 1.3 - **After addition of 50.0 mL KOH:** - pH = 4.0 - **After addition of 75.0 mL KOH:** - pH = 6.7 - **After addition of 100.0 mL KOH:** - pH = 10.32 This information is critical for understanding the titration curve, behavior of phosphorous acid, and for calculating the point at which neutralization occurs with potassium hydroxide.
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