Enter ionic and net ionic equations : (nh4)2co3(aq)+mgcl2(aq) arrow (nh4cl)aq +mgco3(s)

ionic equation:

2NH4(+)(aq) + CO3(2-)(aq) + Mg(2+)(aq) + 2Cl(-)(aq) → NH4(+)(aq) + Cl(-)(aq) + MgCO3(s)

net ionic equation:

NH4(+)(aq) + CO3(2-)(aq) + Mg(2+)(aq) + Cl(-)(aq) →   MgCO3(s)

Explanation:

For ionic equations Start with a balanced molecular equation.  Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions . Indicate the correct formula and charge of each ion .Indicate the correct number of each ion . Write (aq) after each ion  and bring down all compounds with (s), (l), or (g) unchanged. The coefficients are given by the number of moles

(NH4)2CO3(aq)→ 2NH4(+) + CO3(2-). Then

2NH4(+)(aq) + CO3(2-)(aq) + Mg(2+)(aq) + 2Cl(-)(aq) → NH4(+)(aq) + Cl(-)(aq) + MgCO3(s)

For net ionic equations Write the balanced molecular equation.

Write the balanced complete ionic equation.  Cross out the spectator ions that are present, it means the repeated ions on both sides of the equation.  Write the "leftovers" as the net ionic equation.

NH4(+)(aq) + CO3(2-)(aq) + Mg(2+)(aq) + Cl(-)(aq) →   MgCO3(s)

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%