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Sagot :
To determine if [tex]\( H_2SO_4 \)[/tex] (sulfuric acid) is a strong or weak acid, we need to consider its behavior in water. Specifically, we need to look at its ionization, which is described by the balanced equations given:
1. First ionization step:
[tex]\[ H_2SO_4(\ell) + H_2O (\ell) \rightleftharpoons H_3O^+ (aq) + HSO_4^- (aq) \][/tex]
2. Second ionization step:
[tex]\[ HSO_4^- (aq) + H_2O (\ell) \rightleftharpoons H_3O^+ (aq) + SO_4^{2-} (aq) \][/tex]
### Analysis:
1. First Ionization Step:
In the first step, sulfuric acid ([tex]\( H_2SO_4 \)[/tex]) donates one proton ([tex]\( H^+ \)[/tex]) to water ([tex]\( H_2O \)[/tex]), forming hydronium ions ([tex]\( H_3O^+ \)[/tex]) and hydrogen sulfate ions ([tex]\( HSO_4^- \)[/tex]). This step occurs completely and is not in equilibrium, meaning that all [tex]\( H_2SO_4 \)[/tex] molecules ionize fully.
2. Second Ionization Step:
In the second step, the hydrogen sulfate ion ([tex]\( HSO_4^- \)[/tex]) can donate another proton to water to form more hydronium ions and sulfate ions ([tex]\( SO_4^{2-} \)[/tex]). This step is typically in equilibrium, indicating that it does not proceed to completion as the first step does. However, this does not diminish the overall significant contribution of [tex]\( H_2SO_4 \)[/tex] to the concentration of [tex]\( H^+ \)[/tex] ions in the solution.
### Conclusion:
Because [tex]\( H_2SO_4 \)[/tex] dissociates completely in the first ionization step, it produces a large number of [tex]\( H^+ \)[/tex] ions. This complete dissociation is a hallmark of strong acids. Furthermore, even though the second ionization step is in partial equilibrium, the first step's complete dissociation predominantly characterizes [tex]\( H_2SO_4 \)[/tex] as a strong acid.
Therefore, [tex]\( H_2SO_4 \)[/tex] is a STRONG acid because it dissociates completely in water, increasing the concentration of [tex]\( H^+ \)[/tex] ions significantly.
1. First ionization step:
[tex]\[ H_2SO_4(\ell) + H_2O (\ell) \rightleftharpoons H_3O^+ (aq) + HSO_4^- (aq) \][/tex]
2. Second ionization step:
[tex]\[ HSO_4^- (aq) + H_2O (\ell) \rightleftharpoons H_3O^+ (aq) + SO_4^{2-} (aq) \][/tex]
### Analysis:
1. First Ionization Step:
In the first step, sulfuric acid ([tex]\( H_2SO_4 \)[/tex]) donates one proton ([tex]\( H^+ \)[/tex]) to water ([tex]\( H_2O \)[/tex]), forming hydronium ions ([tex]\( H_3O^+ \)[/tex]) and hydrogen sulfate ions ([tex]\( HSO_4^- \)[/tex]). This step occurs completely and is not in equilibrium, meaning that all [tex]\( H_2SO_4 \)[/tex] molecules ionize fully.
2. Second Ionization Step:
In the second step, the hydrogen sulfate ion ([tex]\( HSO_4^- \)[/tex]) can donate another proton to water to form more hydronium ions and sulfate ions ([tex]\( SO_4^{2-} \)[/tex]). This step is typically in equilibrium, indicating that it does not proceed to completion as the first step does. However, this does not diminish the overall significant contribution of [tex]\( H_2SO_4 \)[/tex] to the concentration of [tex]\( H^+ \)[/tex] ions in the solution.
### Conclusion:
Because [tex]\( H_2SO_4 \)[/tex] dissociates completely in the first ionization step, it produces a large number of [tex]\( H^+ \)[/tex] ions. This complete dissociation is a hallmark of strong acids. Furthermore, even though the second ionization step is in partial equilibrium, the first step's complete dissociation predominantly characterizes [tex]\( H_2SO_4 \)[/tex] as a strong acid.
Therefore, [tex]\( H_2SO_4 \)[/tex] is a STRONG acid because it dissociates completely in water, increasing the concentration of [tex]\( H^+ \)[/tex] ions significantly.
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