6.5 Concentration of Aqueous Solution

Concentration of a solution is a measurement that shows the _________________ dissolved in a unit volume of solution.

• quantity of solute

• quantity of solvent

• quantity of solution

What is the formula for concentration?

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• 
• 

The higher the quantity of solute, ________________.

• the lower the concentration of the solution

• the higher the concentration of the solution

How to convert

MOLARITY (mol dm^–3) to CONCENTRATION (g dm^–3)?

• x Molar mass

• / Molar mass

The molarity of KOH solution is 2 mol dm^–3. What is the concentration of the solution?

[RAM: K, 39; O,16; H ,1]

• 28 g dm^–3

• 56 g dm^–3

• 112 g dm^–3

The concentration of HCl is 77 g dm^–3. What is the molarity of the solution?

[RAM: H ,1; Cl, 35.5]

• 0.8 mol dm^-3

• 2.1 mol dm^-3

• 28 mol dm^-3

• 281 mol dm^-3

What is the correct formula to solve for the Molarity of a solution that has 0.4 moles of HCl in 9.5 L of solution?

[1 dm³ = 1L]

• M = 9.5 L / 0.4 mol

• M₁V₁=M₂V₂

• M = 0.4 mol / 9.5 L

• none of the other choices

A questions asks, "what volume of 0.125 M KMnO₄ is required to yield 0.180 mol of potassium permanganate,

KMnO₄?" What is the correct formula set up to solve for this problem?

• 0.125 M = 0.180 mol / volume of solution

• M₁ V₁ = M₂ V₂

• 0.125 M = volume of solution /0.180 mol

• none of the choices listed

What is the molarity of a solution containing 4 moles of KCl in 2.5 dm³ of solution?

• 1.6 M

• 0.63 M

• 10 M

• 2.6 M

What is the number of moles of solute in 550 cm³ of a 0.2M solution?

• 0.11mol

• 110mol

• 27.5mol

• 0.36mol