Problem 128
Question
Phosphorus on reaction with conc. \(\mathrm{HNO}_{3}\) gives an acid A which can also be formed by the action of dil. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) on powdered phosphorite rock, the acid \(\mathrm{A}\) is (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{2}\) (d) \(\mathrm{HPO}_{3}\)
Step-by-Step Solution
Verified Answer
The acid is \\(\mathrm{H}_3\mathrm{PO}_4\\) (b).
1Step 1: Identify the Reaction Products
Identify the products formed when phosphorus reacts with concentrated \(\mathrm{HNO}_3\). One of the expected products is phosphoric acid (\(\mathrm{H}_3\mathrm{PO}_4\)).
2Step 2: Understand Secondary Reaction
Phosphoric acid (\(\mathrm{H}_3\mathrm{PO}_4\)) can also be produced by reacting dilute sulfuric acid (\(\mathrm{H}_2\mathrm{SO}_4\)) with phosphorite rock, which suggests that this is the acid in question.
3Step 3: Select the Correct Acid
From the given options, identify that acid \(\mathrm{A\) is phosphoric acid, which matches the molecular formula \(\mathrm{H}_3\mathrm{PO}_4\). The correct choice is (b) \(\mathrm{H}_3\mathrm{PO}_4\).
Key Concepts
Chemical ReactionsAcid Base ChemistryInorganic Chemistry
Chemical Reactions
In the study of chemistry, chemical reactions are central to understanding how different substances interact with each other. A chemical reaction involves the rearrangement of atoms or ions to form new substances. Typically, this encompasses a change in the chemical composition.
Phosphorus, when reacting with concentrated nitric acid ( \( \mathrm{HNO}_3 \) ), undergoes such a transformation. In this reaction, phosphorus is oxidized by nitric acid, leading to the formation of phosphoric acid.
The general form of the reaction can be represented as: \[ \text{P} + \text{Conc. } \mathrm{HNO}_3 \rightarrow \mathrm{H}_3\mathrm{PO}_4 + \text{other products}\]
Understanding these responses helps comprehend not just the formation of substances like phosphoric acid, but also the broader interactions that take place at the molecular level. Chemical reactions such as this are essential in producing a wide range of materials crucial for various applications in industry and research.
This example also emphasizes the importance of oxidation and reduction reactions, where the transfer of electrons involves changes in the oxidation state of reactants.
Phosphorus, when reacting with concentrated nitric acid ( \( \mathrm{HNO}_3 \) ), undergoes such a transformation. In this reaction, phosphorus is oxidized by nitric acid, leading to the formation of phosphoric acid.
The general form of the reaction can be represented as: \[ \text{P} + \text{Conc. } \mathrm{HNO}_3 \rightarrow \mathrm{H}_3\mathrm{PO}_4 + \text{other products}\]
Understanding these responses helps comprehend not just the formation of substances like phosphoric acid, but also the broader interactions that take place at the molecular level. Chemical reactions such as this are essential in producing a wide range of materials crucial for various applications in industry and research.
This example also emphasizes the importance of oxidation and reduction reactions, where the transfer of electrons involves changes in the oxidation state of reactants.
Acid Base Chemistry
Acid-base chemistry deals with the properties and interactions of acids and bases. These substances are fundamental in chemistry, influencing reactions and being crucial in different contexts, from biology to industry.
Phosphoric acid ( \( \mathrm{H}_3\mathrm{PO}_4 \) ) is a triprotic acid, which means it can donate up to three protons ( \( \mathrm{H}^+ \) ions) in solution. This characteristic makes it versatile in creating acid-base reactions. In this context, the acidic behavior of phosphoric acid can be represented, highlighting its ability to undergo multiple deprotonations:
These reactions demonstrate how phosphoric acid can gradually release its hydrogen ions. This feature is significant for applications that require controlled pH levels. Understanding acid-base chemistry is crucial for predicting the behavior of acids and bases under different conditions.
Phosphoric acid ( \( \mathrm{H}_3\mathrm{PO}_4 \) ) is a triprotic acid, which means it can donate up to three protons ( \( \mathrm{H}^+ \) ions) in solution. This characteristic makes it versatile in creating acid-base reactions. In this context, the acidic behavior of phosphoric acid can be represented, highlighting its ability to undergo multiple deprotonations:
- First ionization: \( \mathrm{H}_3\mathrm{PO}_4 \rightarrow \mathrm{H}^+ + \mathrm{H}_2\mathrm{PO}_4^- \)
- Second ionization: \( \mathrm{H}_2\mathrm{PO}_4^- \rightarrow \mathrm{H}^+ + \mathrm{HPO}_4^{2-} \)
- Third ionization: \( \mathrm{HPO}_4^{2-} \rightarrow \mathrm{H}^+ + \mathrm{PO}_4^{3-} \)
These reactions demonstrate how phosphoric acid can gradually release its hydrogen ions. This feature is significant for applications that require controlled pH levels. Understanding acid-base chemistry is crucial for predicting the behavior of acids and bases under different conditions.
Inorganic Chemistry
Inorganic chemistry encompasses the study of minerals, metals, and non-organic compounds. Phosphoric acid, being an inorganic compound, is vital in multiple chemical processes and industries.
The preparation of phosphoric acid through the treatment of phosphorite rock with dilute sulfuric acid involves the reaction:\[\text{Phosphorite (Ca} \cdot \mathrm{PO}_4 \text{)} + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{H}_3\mathrm{PO}_4 + \text{other products}\]
This process highlights the application of inorganic chemistry in producing phosphoric acid, which is integral to fertilizers, food additives, and cleaning agents, among others.
Inorganic compounds like phosphoric acid often exhibit diverse reactivity due to their different functional groups and structural arrangements. This section of chemistry further explores the periodic table to explain the origins and interactions of all elements except those classified as organic compounds. By understanding inorganic chemistry principles, one appreciates the chemical processes essential to various industries and environmental applications.
The preparation of phosphoric acid through the treatment of phosphorite rock with dilute sulfuric acid involves the reaction:\[\text{Phosphorite (Ca} \cdot \mathrm{PO}_4 \text{)} + \mathrm{H}_2\mathrm{SO}_4 \rightarrow \mathrm{H}_3\mathrm{PO}_4 + \text{other products}\]
This process highlights the application of inorganic chemistry in producing phosphoric acid, which is integral to fertilizers, food additives, and cleaning agents, among others.
Inorganic compounds like phosphoric acid often exhibit diverse reactivity due to their different functional groups and structural arrangements. This section of chemistry further explores the periodic table to explain the origins and interactions of all elements except those classified as organic compounds. By understanding inorganic chemistry principles, one appreciates the chemical processes essential to various industries and environmental applications.
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