First, we need to identify the ions that will be present in the solution when magnesium hydrogen phosphate (MgHPO4) is dissolved in water. Magnesium hydrogen phosphate is a salt and will dissociate into its constituent ions in water. The ions are:

1. Magnesium ion (Mg2+)
2. Hydrogen phosphate ion (HPO4 2-)

Next, we need to calculate the molar mass of MgHPO4 to find out how many moles of MgHPO4 are present in 23.4g. The molar mass of MgHPO4 is approximately 120.3 g/mol.

So, the number of moles of MgHPO4 = mass / molar mass = 23.4g / 120.3 g/mol = 0.194 mol

Since each formula unit of MgHPO4 produces one Mg2+ ion and one HPO4 2- ion, the number of moles of each ion is also 0.194 mol.

The volume of the solution is 4.80L.

The concentration of each ion in mol/L (Molarity) = number of moles / volume in L = 0.194 mol / 4.80L = 0.0404 M

To convert this to mEq/L, we need to multiply by the charge of the ion and by 1000 (since 1 Eq = 1 mol of charge, and 1 mEq = 1/1000 Eq).

For Mg2+, the concentration in mEq/L = 0.0404 M * 2 * 1000 = 80.8 mEq/L

For HPO4 2-, the concentration in mEq/L = 0.0404 M * 2 * 1000 = 80.8 mEq/L

So, the composition of the electrolyte solution is:

| Ion | Concentration (mEq/L) |
| --- | --------------------- |
| Mg2+ | 80.8 |
| HPO4 2- | 80.8 |

Question

First, we need to identify the ions that will be present in the solution when magnesium hydrogen phosphate (MgHPO4) is dissolved in water. Magnesium hydrogen phosphate is a salt and will dissociate into its constituent ions in water. The ions are:

1. Magnesium ion (Mg2+)
2. Hydrogen phosphate ion (HPO4 2-)

Next, we need to calculate the molar mass of MgHPO4 to find out how many moles of MgHPO4 are present in 23.4g. The molar mass of MgHPO4 is approximately 120.3 g/mol.

So, the number of moles of MgHPO4 = mass / molar mass = 23.4g / 120.3 g/mol = 0.194 mol

Since each formula unit of MgHPO4 produces one Mg2+ ion and one HPO4 2- ion, the number of moles of each ion is also 0.194 mol.

The volume of the solution is 4.80L.

The concentration of each ion in mol/L (Molarity) = number of moles / volume in L = 0.194 mol / 4.80L = 0.0404 M

To convert this to mEq/L, we need to multiply by the charge of the ion and by 1000 (since 1 Eq = 1 mol of charge, and 1 mEq = 1/1000 Eq).

For Mg2+, the concentration in mEq/L = 0.0404 M * 2 * 1000 = 80.8 mEq/L

For HPO4 2-, the concentration in mEq/L = 0.0404 M * 2 * 1000 = 80.8 mEq/L

So, the composition of the electrolyte solution is:

| Ion | Concentration (mEq/L) |
| --- | --------------------- |
| Mg2+ | 80.8 |
| HPO4 2- | 80.8 |

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