Write the formulas of the ions (including charges) present in aqueous solutions of the following:
K2CO3
NH4NO3
NA2Cr2O7
Mg(C2H3O2)2
Make sure it is both mass and charge balanced.
Here is a listing of many polyatomic ions. This should give you a start. Post with specific questions but tell us what you don't understand about it.
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To write the formulas of the ions present in aqueous solutions, we need to break down each compound into its individual ions.
1. K2CO3
The compound K2CO3 dissociates into two potassium ions (K+) and one carbonate ion (CO₃²⁻). Therefore, the formula for the ions present in aqueous solution is: 2K+ + CO₃²⁻.
2. NH4NO3
The compound NH4NO3 dissociates into one ammonium ion (NH₄+) and one nitrate ion (NO₃⁻). So the formula for the ions present in aqueous solution is: NH₄+ + NO₃⁻.
3. Na2Cr2O7
The compound Na2Cr2O7 dissociates into two sodium ions (Na+) and one dichromate ion (Cr2O7²⁻). The formula for the ions present in aqueous solution is: 2Na+ + Cr2O7²⁻.
4. Mg(C2H3O2)2
The compound Mg(C2H3O2)2 dissociates into one magnesium ion (Mg²⁺) and two acetate ions (C2H3O2⁻). Therefore, the formula for the ions present in aqueous solution is: Mg²⁺ + 2C2H3O2⁻.
It's important to note that these formulas are both mass and charge balanced. To verify this, you can check that the total number of positive charges equals the total number of negative charges in each compound.