CALCULATE THE OSMOLARITY OF THE FOLLOWING
).1M KNO3 & ).35M Na3PO4
& 0.35
To calculate the osmolarity, we need to find the total number of moles of solute particles in the given solutions, and then divide by the total volume of the solution.
Let's start with the first solution, 0.1 M KNO3.
In KNO3, there is one K+ ion and one NO3- ion. That means there are a total of 2 moles of solute particles for every mole of KNO3.
So, 0.1 M KNO3 means that there are 0.1 moles of KNO3 for every liter of solution. Since we know that there are 2 moles of solute particles for every mole of KNO3, we can say that there are 0.1 x 2 = 0.2 moles of solute particles for every liter of solution.
Now let's move on to the second solution, 0.35 M Na3PO4.
In Na3PO4, there are three Na+ ions and one PO4-3 ion. That means there are a total of 4 moles of solute particles for every mole of Na3PO4.
So, 0.35 M Na3PO4 means that there are 0.35 moles of Na3PO4 for every liter of solution. Since we know that there are 4 moles of solute particles for every mole of Na3PO4, we can say that there are 0.35 x 4 = 1.4 moles of solute particles for every liter of solution.
Finally, let's calculate the osmolarity of the third solution, 0.35.
Since there are no units given, we assume it is referring to 0.35 M. This means that there are 0.35 moles of solute particles for every liter of solution. Since there are no additional solute particles mentioned, we can consider this as the total number of moles of solute particles for every liter of solution.
So, the osmolarity of the third solution is 0.35 moles/L.
Therefore, to find the total osmolarity of all the solutions, we add up the osmolarities of each solution:
Total Osmolarity = Osmolarity of KNO3 solution + Osmolarity of Na3PO4 solution + Osmolarity of 0.35 solution
= 0.2 moles/L + 1.4 moles/L + 0.35 moles/L
= 1.95 moles/L
The total osmolarity of all the solutions is 1.95 moles/L.
To calculate the osmolarity of a solution, you need to know the concentration of each solute and the number of particles that each solute will dissociate into when dissolved in water.
Let's begin with the first solution, 0.1M KNO3. This represents 0.1 moles of KNO3 per liter of solution. KNO3 dissociates into two particles: one K+ ion and one NO3- ion.
Therefore, the effective osmolarity contributed by KNO3 is calculated as follows:
Osmolarity of KNO3 = (0.1 M KNO3) × (2 particles/molecule)
= 0.2 Osm
Next, let's move on to the second solution, 0.35M Na3PO4. This represents 0.35 moles of Na3PO4 per liter of solution. Na3PO4 dissociates into four particles: three Na+ ions and one PO4^3- ion.
Hence, the effective osmolarity contributed by Na3PO4 is calculated as follows:
Osmolarity of Na3PO4 = (0.35 M Na3PO4) × (4 particles/molecule)
= 1.4 Osm
Lastly, you mentioned "0.35" without specifying the unit or solute. If you provide more details, I can assist you in calculating its osmolarity as well.
To determine the total osmolarity of a solution containing multiple solutes, you sum the individual osmolarities of each solute. In this case, the total osmolarity would be the sum of the osmolarities of KNO3 and Na3PO4.
Total Osmolarity = Osmolarity of KNO3 + Osmolarity of Na3PO4
= 0.2 Osm + 1.4 Osm
= 1.6 Osm