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Which of the following statements are co...

Which of the following statements are correct ?

A

According to Bronsted Lowry concept, `H_(2)SO_(4)` can also act as a base

B

`SiF_(4)` is an acid according to Lewis concept

C

Stronger the acid, higher is its `pK_(a)` value

D

HCl, `HNO_(3) and H_(2)SO_(4)` act as equally strong acids in any solvent.

Text Solution

AI Generated Solution

The correct Answer is:
To determine which statements are correct, we will analyze each statement one by one based on the concepts of acid-base chemistry, specifically the Bronsted-Lowry and Lewis definitions. ### Step-by-Step Solution: 1. **Statement Analysis:** - **Statement 1:** "According to Bronsted-Lowry concept, H2SO4 can also act as a base." - **Analysis:** According to the Bronsted-Lowry theory, an acid is a proton donor and a base is a proton acceptor. H2SO4 is primarily known as a strong acid, but it can accept protons in certain reactions, thus acting as a base. This statement is **correct**. 2. **Statement Analysis:** - **Statement 2:** "SiF4 is an acid according to Lewis concept." - **Analysis:** The Lewis definition states that an acid is an electron pair acceptor. SiF4 can accept electron pairs due to the presence of an empty p-orbital on silicon. Therefore, SiF4 can be classified as a Lewis acid. This statement is **correct**. 3. **Statement Analysis:** - **Statement 3:** "Stronger the acid, higher is its pKa value." - **Analysis:** The pKa value is inversely related to the strength of an acid. A stronger acid has a lower pKa value. Therefore, this statement is **incorrect**. 4. **Statement Analysis:** - **Statement 4:** "HCl, HNO3, and H2SO4 act as equally strong acids in any solvent." - **Analysis:** While HCl, HNO3, and H2SO4 are strong acids in water, their strength can vary in different solvents. For example, in non-aqueous solvents, their acid strengths may differ. Thus, this statement is **incorrect**. ### Conclusion: From the analysis above, we conclude that: - Statement 1 is correct. - Statement 2 is correct. - Statement 3 is incorrect. - Statement 4 is incorrect. Therefore, the correct answers are **A and B**.
To determine which statements are correct, we will analyze each statement one by one based on the concepts of acid-base chemistry, specifically the Bronsted-Lowry and Lewis definitions. ### Step-by-Step Solution: 1. **Statement Analysis:** - **Statement 1:** "According to Bronsted-Lowry concept, H2SO4 can also act as a base." - **Analysis:** According to the Bronsted-Lowry theory, an acid is a proton donor and a base is a proton acceptor. H2SO4 is primarily known as a strong acid, but it can accept protons in certain reactions, thus acting as a base. This statement is **correct**. ...
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