Solutions (Formative check)

Ionic compounds produce ions in solution by

• Ionization

• dissociation

• evaporation

• solvation

Which of the following will NOT increase the rate at which a solute dissolves in a solvent?

• Increasing the surface area of the solute

• Stirring the solvent

• Increasing the temperature

• Increasing the particle size of the solute

Heating a solvent _______ the energy of its particles, making them move faster on average, and ________ the rate at which a solid solute can dissolve in the solvent.

• increases, increases

• increases, decreases

• decreases, decreases

• decreases, increases

Tags

NGSS.HS-PS1-5

NGSS.HS-PS3-2

A polar solvent dissolving a polar or ionic solute can best be described by:

• ionized H₃O⁺ molecules

• like dissolves like

• increased polarity increases the rate a solute dissolves in a solvent

Which substance is considered a homogeneous mixture? pay close attention to symbols...

• KBr_(s)

• NaCl_(s)

• LiNO_3(aq)

• H₂O_(l)

Which term correctly describes an aqueous solution of potassium chloride, KCl?

• water is the solute, KCl is the solvent

• KCl is the solute, water is the solvent

• NaBr is the solute, water is the solvent

• water is the solute, NaBr is the solvent

Which choice is an example of a supersaturated solution in 100 g of water? Use the Solubility Curve graph on your classwork practice if you cannot read this one.

• 90 g of NH₄Cl at 90 °C

• 5 g of SO₂ at 40 °C

• 100 g of KI at 10 °C

• 13 g of NH₃ at 80 °C

An unsaturated solution is created by dissolving 20 g of KClO₃ into 100 g of water at 70 °C. How many more grams of KClO₃ must be dissolved in order to saturate this solution? Use the solubility curve from classwork practice if you cannot read this one.

• 20g

• 24 g

• 16g

• 10 g

What must be the temperature of 100 g of water in order for 70 g of NH₄Cl to dissolve to form a saturated solution?

• 86 °C

• 81 °C

• 90 °C

• 95 °C

How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? Molarity = moles/liters

• 2

• 3

• 4

• 6