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Chapter 6: Problem 28

Which of the following cannot show acidic nature? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{CaCO}_{3}\) (c) \(\mathrm{HCl}\) (d) \(\mathrm{HSO}_{4}^{-}\)

Short Answer

Expert verified
a) H2CO3 b) CaCO3 c) HCl d) HSO4- Answer: b) CaCO3

Step by step solution

01

Identify substance's characteristics

For each substance, we need to analyze its formula and determine if it can dissociate to produce H+ ions when in an aqueous solution. Let's examine each substance: (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) - Carbonic acid: It has H+ ions and can therefore show acidic nature. (b) \(\mathrm{CaCO}_{3}\) - Calcium carbonate: It does not have H+ ions in its structure and cannot dissociate into H+ ions in the solution. (c) \(\mathrm{HCl}\) - Hydrochloric acid: It has H+ ions in its structure and can dissociate into H+ ions in the solution, thus it can show acidic nature. (d) \(\mathrm{HSO}_{4}^{-}\) - Bisulfate ion: It has H+ ions and can dissociate into H+ ions in the solution, therefore it can show acidic nature.
02

Identify the substance that cannot show acidic nature

As we have analyzed the chemical formulas of each substance, we have determined that option (b) \(\mathrm{CaCO}_{3}\) (Calcium carbonate) is the substance that cannot show acidic nature as it does not have H+ ions in its structure and cannot dissociate into H+ ions in the solution. So, the correct answer is \(\mathrm{CaCO}_{3}\) (option b).

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