the formula for the sulfate ion is so₄²⁻. based on this information, which two formulas below represent…

Explanation:

Step1: Determine ion charges

Magnesium ($Mg$) has a charge of $Mg^{2 +}$, potassium ($K$) has a charge of $K^{+}$, and sulfate ion has a charge of $SO_{4}^{2 -}$.

Step2: Check charge - neutrality for each option

For option A ($MgSO_{4}$): The $2+$ charge of $Mg$ balances the $2 -$ charge of $SO_{4}^{2 -}$. So the overall charge of the compound is $+ 2+( - 2)=0$. For option B ($Mg_{2}SO_{4}$): The total positive charge from two $Mg^{2 +}$ ions is $2\times(+2) = + 4$, and the negative charge from one $SO_{4}^{2 -}$ ion is $-2$. The overall charge is $+4+( - 2)=+2$, so it is not neutral. For option C ($KSO_{4}$): The positive charge of $K^{+}$ is $+1$ and the negative charge of $SO_{4}^{2 -}$ is $-2$. The overall charge is $+1+( - 2)=-1$, so it is not neutral. For option D ($K_{2}SO_{4}$): The total positive charge from two $K^{+}$ ions is $2\times(+1)=+2$, and the negative charge from one $SO_{4}^{2 -}$ ion is $-2$. The overall charge is $+2+( - 2)=0$.

Answer:

A. $MgSO_{4}$, D. $K_{2}SO_{4}$