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Chapter 4: Problem 63

The average adult human male has a total blood volume of 5.0 L. If the concentration of sodium ion in this average individual is \(0.135 \mathrm{M}\), what is the mass of sodium ion circulating in the blood?

Short Answer

Expert verified
The mass of sodium ions circulating in the average adult human male's blood is approximately 15.5 g. This calculation is based on a blood volume of 5.0 L and a sodium ion concentration of \(0.135 \mathrm{M}\).

Step by step solution

01

Calculate moles of sodium ions in the blood

To determine the moles of sodium ions in the blood, we can use the formula: Moles of solute = Molarity × Volume of solution Here, the Molarity of sodium ions is \(0.135 \mathrm{M}\) and the volume of the blood is 5.0 L.
02

Convert volume to liters

The volume of blood is given in liters, so we don't need to make any conversion. We can directly use the given volume: Volume of blood = 5.0 L
03

Calculate moles of sodium ions

Now, we can calculate the moles of sodium ions using the molarity and volume: Moles of sodium ions = \(0.135 \mathrm{M} \times 5.0\, \mathrm{L}\) Moles of sodium ions = \(0.675 \, \mathrm{moles}\)
04

Calculate the mass of sodium ions

To calculate the mass of sodium ions, we can use the formula: Mass = Moles × Molar mass The molar mass of sodium ion (Na+) is approximately \(23 \, \mathrm{g/mol}\) (we consider only the sodium part of the ion, ignoring the charge). So, the mass of sodium ions in the blood: Mass of sodium ions = \(0.675 \, \mathrm{moles} \times 23\, \mathrm{g/mol}\) Mass of sodium ions = \(15.525 \, \mathrm{g}\)
05

Round the answer to the appropriate decimal place

The mass of sodium ions circulating in the blood is approximately 15.5 g, after rounding off to one decimal place.

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Most popular questions from this chapter

Predict whether each of the following compounds is solu- ble in water: (a) $\mathrm{MgS},(\mathbf{b}) \mathrm{Cr}(\mathrm{OH})_{3},(\mathbf{c}) \mathrm{Zn} \mathrm{Cl}_{2}$ (d) \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) (e) \(\mathrm{Sr}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\)

We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) \(\mathrm{Hg}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{NH}_{4} \mathrm{OH}\), (c) \(\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\) (d) \(\mathrm{AgNO}_{3}\), (e) FeCO \(_{3}\)

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: $$ \begin{array}{c} \mathrm{Br}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q) \\ \mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q) \end{array} $$ (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides? (b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed. (c) Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

Acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3},\) is a nonelectrolyte; hypochlorous acid, \(\mathrm{HClO},\) is a weak electrolyte; and ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? (b) If $0.1 \mathrm{~mol}$ of each compound is dissolved in solution, which one contains \(0.2 \mathrm{~mol}\) of solute particles, which contains \(0.1 \mathrm{~mol}\) of solute particles, and which contains somewhere between 0.1 and 0,2 mol of solute particles?
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