A solution is a mixture of two or more substances that is uniform throughout. You can keep track of what you're putting into a solution by measuring the number of particles. That said, we call the total number of particles the concentration of the solution, which is simply how densely saturated a solution is with something. (Example: how much hot chocolate powder is in a mug of hot water. More powder= higher concentration, more chocolateness. Less powder = lower concentration, less chocolateness. Ew.) Another, more science-y word for concentration is molarity, represented by the following equation:
Molarity (M) = number of moles (n) / Volume (L)
Problems:
1.) What does it mean when a solution is "uniform throughout"? This means that the solute. Has been thoroughly dissolved in a solvent and there are no random particles or "floaties" in the liquid.
5.) Put these three solutions in order of increasing molarity.
A.) 4.0 mol per 8.0 L: molarity is 0.5 mol/L
B.) 6.0 mol per 6.0 L: molarity is 1 mol/L
C.) 1.0 mol per10 L: molarity is 0.1 mol/L
Order: C, A, B.
1.) What does it mean when a solution is "uniform throughout"? This means that the solute. Has been thoroughly dissolved in a solvent and there are no random particles or "floaties" in the liquid.
5.) Put these three solutions in order of increasing molarity.
A.) 4.0 mol per 8.0 L: molarity is 0.5 mol/L
B.) 6.0 mol per 6.0 L: molarity is 1 mol/L
C.) 1.0 mol per10 L: molarity is 0.1 mol/L
Order: C, A, B.
Lesson 14:
In this lesson, we learned the relation of concentration to volume. The concentration does not change if the volume of the solution changes. If a solute is dissolved thoroughly and evenly in the solvent, the number of particles, or the molarity, should not change. Because of this, the equation mentioned in lesson 13 can be used to find molarity, volumes, and the moles in just about any solution.
Problems:
2.) How can you figure out how many moles of solute you have in a solution with a specific concentration? In the equation molarity = moles / volume, finding the number of moles requires multiplying both sides by the volume.
5.) Glucose and sucrose are two different types of sugar. Consider these aqueous solutions: 1.0 L of 1.0 M C6H12O6 (glucose), 1.0 L of 1.0 M C12H22O11 (sucrose), 500mL of 1.0 M C12H22O11 (sucrose):
A.) Which solution has the most molecules? Explain. The glucose solution, because it has the lowest molar mass for the given volume of solvent.
B.) Which solution is most concentrated? Explain. The glucose solution, because it has more molecules for a given volume and is more saturated with glucose.
C.) Which solution has the most mass? Explain. The first sucrose solution has the most mass, because it has a larger volume than the last sucrose solution and sucrose has a larger molar mass than glucose.
Problems:
2.) How can you figure out how many moles of solute you have in a solution with a specific concentration? In the equation molarity = moles / volume, finding the number of moles requires multiplying both sides by the volume.
5.) Glucose and sucrose are two different types of sugar. Consider these aqueous solutions: 1.0 L of 1.0 M C6H12O6 (glucose), 1.0 L of 1.0 M C12H22O11 (sucrose), 500mL of 1.0 M C12H22O11 (sucrose):
A.) Which solution has the most molecules? Explain. The glucose solution, because it has the lowest molar mass for the given volume of solvent.
B.) Which solution is most concentrated? Explain. The glucose solution, because it has more molecules for a given volume and is more saturated with glucose.
C.) Which solution has the most mass? Explain. The first sucrose solution has the most mass, because it has a larger volume than the last sucrose solution and sucrose has a larger molar mass than glucose.
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