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# Consider the two acids $\mathrm{HCl}$ and $\mathrm{CH}_3 \mathrm{COOH}$. When in (separate) solutions they react in the following way: The $\mathrm{pH}$ of the $\mathrm{HCl}$ was measured at 1. The $\mathrm{pH}$ of the $\mathrm{CH}_3 \mathrm{COOH}$ was measured at $2.88$. $25 \mathrm{~mL} 0.1 \mathrm{~mol} / \mathrm{L}$ of each acid was reacted with an excess of sodium carbonate $\left(\mathrm{Na}_2 \mathrm{CO}_3\right)$. The reaction between $\mathrm{HCl}$ and $\mathrm{Na}_2 \mathrm{CO}_3$ was vigorous. The reaction between $\mathrm{CH}_3 \mathrm{COOH}$ and $\mathrm{Na}_2 \mathrm{CO}_3$ was much slower. Each reaction produced the same amount of $\mathrm{CO}_2$ gas. (a) Which acid has the greatest concentration of $\mathrm{H}^{+}$ions in solution?(b) Explain why the same amount of $\mathrm{CO}_2$ gas was produced despite the $\mathrm{pH}$ of the acids being different:

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Consider the two acids HCl and CH$_3$COOH. They dissociate in aqueous solutions individually:

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

$\mathrm{CH_3COOH \leftrightarrows H^+ + CH_3COO^-}$

The pH of HCl is 1 while for CH$_3$COOH is 2.88. 25 mL of 0.1 mol/L each acid reacted with excess of Na$_2$CO$_3$ forming the same amount of CO$_2$ gas. During the experiment, it was observed that:

• the reaction between HCl and Na$_2$CO$_3$ was intense
• the reaction between CH$_3$COOH and Na$_2$CO$_3$ progressed slowly

(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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