Unit 11 (Ch 15) Review

Define a solution.

• A homogeneous mixture of two or more substances.

• A heterogeneous mixture of two or more substances.

• A pure substance.

• A compound.

How does a molecular solid such as sugar dissolve in water?

• portions of sugar molecules are attracted to water molecules

• sugar molecules form covalent bonds with water molecules

• sugar molecules form ionic bonds with water molecules

• sugar molecules split into separate ions to dissolve in water

How does an ionic solute such as NaCl dissolve in water?

• portions of NaCl crystals for hydrogen bonds with water molecules

• NaCl crystals form covalent bonds with water molecules

• NaCl crystals form ionic bonds with water molecules

• NaCl crystals split into separate ions to dissolve in water

What are three ways to increase the rate of dissolution of a solute?

• heat the solution

• stir the solution

• increase the surface area of the solute

• increase the number of solute particles

Tags

NGSS.HS-PS1-5

Match the following statements correctly with a saturated solution, an unsaturated solution, and a supersaturated solution?

• supersaturated solution

• more solute is dissolved than is normally possible at a particular

  temperature

• saturated solution

• contains less solute

  than can dissolve at a particular temperature

• unsaturated solution

• contains as much solute as can dissolve at a

  particular temperature

Match the terms to the definitions

• Percent by mass

  (or mass percent)

• the number of equivalents per liter of solution

• Normality

• (mass of solute) × 100%

  ---

  (mass of solution)

• Molarity

• the number of moles of solute per liter of solution

One equivalent of an acid can furnish ​ (a)   of ​ (b)   ions.

One equivalent of a base can furnish ​ (c)   of​ (d)   ions.

• one mole
• H+
• OH–
• positive
• negative
• one kilogram
• one gram

The normality of a solution is defined as

• equivalents of solute

  ---

  liter of solution

• equivalents of solvent

  ---

  liter of solution

• moles of solute

  ---

  liter of solution

• moles of solvent

  ---

  liter of solution

A 12.5-g sample of glucose (C₆H₁₂O₆) is dissolved in 225 g of water. Calculate the percent by mass of glucose in the solution.

• 4.8%

• 5.3%

• 6.3%

• 5.8%

Answer explanation

A chemist prepares some standard solutions for use in the lab using 500.0-mL volumetric flasks to contain the solutions. If the following masses of solutes are used, calculate the resulting molarity of a solution with 4.865 g NaCl. (The molar mass of NaCl is 58.44 g/mol)

• 0.167 M

• 0.132 M

• 0.244 M

• 0.929 M

Answer explanation