Westonci.ca is the premier destination for reliable answers to your questions, provided by a community of experts. Discover detailed answers to your questions from a wide network of experts on our comprehensive Q&A platform. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.
Sagot :
To determine the correct balanced hydration equation for the dissociation of sodium sulfate [tex]\((\text{Na}_2\text{SO}_4)\)[/tex] in water, we need to analyze the given equations and compare them to the typical dissociation behavior of this compound in aqueous solution.
### Equation 1:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} \text{Na}^+(aq) + 2 \text{SO}_4^{2-}(aq) \][/tex]
- Upon examining this equation, we see that it suggests [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into one [tex]\(\text{Na}^+\)[/tex] ion and two [tex]\(\text{SO}_4^{2-}\)[/tex] ions.
- However, this is incorrect because [tex]\(\text{Na}_2\text{SO}_4\)[/tex] should produce two [tex]\(\text{Na}^+\)[/tex] ions and one [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
### Equation 2:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^{2+}(aq) + \text{S}^{2-}(aq) + \text{O}_4^{2-}(aq) \][/tex]
- This equation suggests [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] dissociates into ions with unusual oxidation states: two [tex]\(\text{Na}^{2+}\)[/tex] ions (instead of [tex]\(\text{Na}^+\)[/tex] ions), one [tex]\(\text{S}^{2-}\)[/tex] ion, and one [tex]\(\text{O}_4^{2-}\)[/tex] ion.
- These species are not typical products of [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociation and are chemically unrealistic.
### Equation 3:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} \text{Na}_2^{2+}(aq) + \text{SO}_4^{2-}(aq) \][/tex]
- This equation proposes that [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into a [tex]\(\text{Na}_2^{2+}\)[/tex] ion and a [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
- A [tex]\(\text{Na}_2^{2+}\)[/tex] ion is not a recognized or stable species in aqueous solution.
### Equation 4:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^+(aq) + \text{SO}_4^{2-}(aq) \][/tex]
- This equation correctly indicates that [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into two [tex]\(\text{Na}^+\)[/tex] ions and one [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
- This is consistent with known chemical behavior and balances both mass and charge.
Thus, the correct balanced hydration equation for [tex]\(\text{Na}_2\text{SO}_4\)[/tex] in water is:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^+(aq) + \text{SO}_4^{2-}(aq) \][/tex]
Therefore, the correct equation is given by option 4.
### Equation 1:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} \text{Na}^+(aq) + 2 \text{SO}_4^{2-}(aq) \][/tex]
- Upon examining this equation, we see that it suggests [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into one [tex]\(\text{Na}^+\)[/tex] ion and two [tex]\(\text{SO}_4^{2-}\)[/tex] ions.
- However, this is incorrect because [tex]\(\text{Na}_2\text{SO}_4\)[/tex] should produce two [tex]\(\text{Na}^+\)[/tex] ions and one [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
### Equation 2:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^{2+}(aq) + \text{S}^{2-}(aq) + \text{O}_4^{2-}(aq) \][/tex]
- This equation suggests [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] dissociates into ions with unusual oxidation states: two [tex]\(\text{Na}^{2+}\)[/tex] ions (instead of [tex]\(\text{Na}^+\)[/tex] ions), one [tex]\(\text{S}^{2-}\)[/tex] ion, and one [tex]\(\text{O}_4^{2-}\)[/tex] ion.
- These species are not typical products of [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociation and are chemically unrealistic.
### Equation 3:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} \text{Na}_2^{2+}(aq) + \text{SO}_4^{2-}(aq) \][/tex]
- This equation proposes that [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into a [tex]\(\text{Na}_2^{2+}\)[/tex] ion and a [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
- A [tex]\(\text{Na}_2^{2+}\)[/tex] ion is not a recognized or stable species in aqueous solution.
### Equation 4:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^+(aq) + \text{SO}_4^{2-}(aq) \][/tex]
- This equation correctly indicates that [tex]\(\text{Na}_2\text{SO}_4\)[/tex] dissociates into two [tex]\(\text{Na}^+\)[/tex] ions and one [tex]\(\text{SO}_4^{2-}\)[/tex] ion.
- This is consistent with known chemical behavior and balances both mass and charge.
Thus, the correct balanced hydration equation for [tex]\(\text{Na}_2\text{SO}_4\)[/tex] in water is:
[tex]\[ \text{Na}_2\text{SO}_4(s) \xrightarrow{H_2O} 2 \text{Na}^+(aq) + \text{SO}_4^{2-}(aq) \][/tex]
Therefore, the correct equation is given by option 4.
We appreciate your time on our site. Don't hesitate to return whenever you have more questions or need further clarification. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Westonci.ca is your go-to source for reliable answers. Return soon for more expert insights.
