Answer:
0.16196 mEq of PO4^3- ions present in the solution
Step-by-step explanation:
To find the number of milliequivalents (mEq) of PO4^3- ions that must be present in the solution, we need to consider the charge of each ion and convert the moles of each ion to mEq.First, let's determine the equivalent weight (EW) for each ion. The equivalent weight is the molar mass of the ion divided by its charge.Ca^2+: The molar mass of Ca^2+ is approximately 40.08 g/mol, and it has a charge of 2. So, EW(Ca^2+) = 40.08 g/mol / 2 = 20.04 g/eq.NH4^+: The molar mass of NH4^+ is approximately 18.04 g/mol, and it has a charge of 1. So, EW(NH4^+) = 18.04 g/mol / 1 = 18.04 g/eq.HCO3^-: The molar mass of HCO3^- is approximately 61.02 g/mol, and it has a charge of 1. So, EW(HCO3^-) = 61.02 g/mol / 1 = 61.02 g/eq.Cl^-: The molar mass of Cl^- is approximately 35.45 g/mol, and it has a charge of 1. So, EW(Cl^-) = 35.45 g/mol / 1 = 35.45 g/eq.Now, we can calculate the mEq of each ion:mEq(Ca^2+) = 0.012 moles × 20.04 g/eq = 0.24048 mEqmEq(NH4^+) = 0.048 moles × 18.04 g/eq = 0.86736 mEqmEq(HCO3^-) = 0.015 moles × 61.02 g/eq = 0.9153 mEqmEq(Cl^-) = 0.010 moles × 35.45 g/eq = 0.3545 mEqTo maintain electrical neutrality in the solution, the total mEq of cations should equal the total mEq of anions. Therefore, the total mEq of PO4^3- ions must be equal to the difference between the total mEq of cations and anions:Total mEq of PO4^3- ions = (Total mEq of cations) - (Total mEq of anions)Total mEq of cations = mEq(Ca^2+) + mEq(NH4^+)
Total mEq of anions = mEq(HCO3^-) + mEq(Cl^-)Total mEq of cations = 0.24048 mEq + 0.86736 mEq = 1.10784 mEq
Total mEq of anions = 0.9153 mEq + 0.3545 mEq = 1.2698 mEqNow, calculate the total mEq of PO4^3- ions:Total mEq of PO4^3- ions = 1.10784 mEq - 1.2698 mEq = -0.16196 mEqTo maintain electrical neutrality, there should be approximately 0.16196 mEq of PO4^3- ions present in the solution