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The false statement of the acids of phos...

The false statement of the acids of phosphorus `H_3 PO_2, H_3 PO_3` and `H_3 PO_4` is

A

The order of their acidity is `H_3PO_4 gt H_3PO_3 gt H_3PO_2`

B

All the them are reducing in nature

C

All of them are tribasic acids

D

The geometry of phosphorus is tetrahedral in all the three.

Text Solution

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The correct Answer is:
To determine the false statement regarding the acids of phosphorus \( H_3PO_2 \), \( H_3PO_3 \), and \( H_3PO_4 \), we will analyze each statement step by step. ### Step 1: Analyze the Acidity Order The first statement claims that the order of acidity is \( H_3PO_4 > H_3PO_3 > H_3PO_2 \). - **Explanation**: - \( H_3PO_4 \) (phosphoric acid) is a stronger acid than \( H_3PO_3 \) (phosphorous acid), which in turn is stronger than \( H_3PO_2 \) (hypophosphorous acid). This is because the number of \( OH \) groups and the oxidation state of phosphorus influence acidity. More \( OH \) groups generally lead to stronger acids due to increased ability to donate protons. - **Conclusion**: This statement is **true**. ### Step 2: Check Reducing Nature The second statement asserts that all of them are reducing in nature. - **Explanation**: - All these acids can donate hydrogen ions in aqueous solution, which allows them to act as reducing agents. Therefore, they can reduce other substances. - **Conclusion**: This statement is **true**. ### Step 3: Determine Basicity The third statement claims that all of them are tri-basic acids. - **Explanation**: - \( H_3PO_4 \) is a tribasic acid because it can donate three protons. \( H_3PO_3 \) is dibasic (can donate two protons), and \( H_3PO_2 \) is monobasic (can donate one proton). Thus, not all of them are tribasic. - **Conclusion**: This statement is **false**. ### Step 4: Geometry of Phosphorus The fourth statement states that the geometry of phosphorus is tetrahedral in all three acids. - **Explanation**: - In all three acids, phosphorus is sp³ hybridized, leading to a tetrahedral geometry. This is consistent across \( H_3PO_2 \), \( H_3PO_3 \), and \( H_3PO_4 \). - **Conclusion**: This statement is **true**. ### Final Conclusion The false statement among the given options is that all of them are tri-basic acids.
To determine the false statement regarding the acids of phosphorus \( H_3PO_2 \), \( H_3PO_3 \), and \( H_3PO_4 \), we will analyze each statement step by step. ### Step 1: Analyze the Acidity Order The first statement claims that the order of acidity is \( H_3PO_4 > H_3PO_3 > H_3PO_2 \). - **Explanation**: - \( H_3PO_4 \) (phosphoric acid) is a stronger acid than \( H_3PO_3 \) (phosphorous acid), which in turn is stronger than \( H_3PO_2 \) (hypophosphorous acid). This is because the number of \( OH \) groups and the oxidation state of phosphorus influence acidity. More \( OH \) groups generally lead to stronger acids due to increased ability to donate protons. ...
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