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Question

Consider the two acids HCl\mathrm{HCl} and CH3COOH\mathrm{CH}_3 \mathrm{COOH}. When in (separate) solutions they react in the following way:

  • The pH\mathrm{pH} of the HCl\mathrm{HCl} was measured at 1. The pH\mathrm{pH} of the CH3COOH\mathrm{CH}_3 \mathrm{COOH} was measured at 2.882.88.
  • 25 mL0.1 mol/L25 \mathrm{~mL} 0.1 \mathrm{~mol} / \mathrm{L} of each acid was reacted with an excess of sodium carbonate (Na2CO3)\left(\mathrm{Na}_2 \mathrm{CO}_3\right). The reaction between HCl\mathrm{HCl} and Na2CO3\mathrm{Na}_2 \mathrm{CO}_3 was vigorous. The reaction between CH3COOH\mathrm{CH}_3 \mathrm{COOH} and Na2CO3\mathrm{Na}_2 \mathrm{CO}_3 was much slower.
  • Each reaction produced the same amount of CO2\mathrm{CO}_2 gas.

(a) Which acid has the greatest concentration of H+\mathrm{H}^{+}ions in solution?

(b) Explain why the same amount of CO2\mathrm{CO}_2 gas was produced despite the pH\mathrm{pH} of the acids being different:

Solution

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Consider the two acids HCl and CH3_3COOH. They dissociate in aqueous solutions individually:

HClH++Cl\mathrm{HCl \rightarrow H^+ + Cl^-}

CH3COOHH++CH3COO\mathrm{CH_3COOH \leftrightarrows H^+ + CH_3COO^-}

The pH of HCl is 1 while for CH3_3COOH is 2.88. 25 mL of 0.1 mol/L each acid reacted with excess of Na2_2CO3_3 forming the same amount of CO2_2 gas. During the experiment, it was observed that:

  • the reaction between HCl and Na2_2CO3_3 was intense
  • the reaction between CH3_3COOH and Na2_2CO3_3 progressed slowly

Based on this information, answer:

(a) indicate which acid has the greatest concentration of H+^+ ions in solution

(b) why both acids produced the same amount of gas given the different vales in pH

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