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Chemistry - Week Five

Printable Version of this lesson board in PDF format

High School Chemistry

Week 5 May 4-May 8

Weekly Packet

Topic: Acid and Base pH Calculations
Science Objectives: Students will be able to:

  • calculate hydronium and hydroxide ion concentrations for a solution given either value.
  • calculate the pH of a solution given the hydronium ion concentration.
  • relate the hydronium or hydroxide ion concentration and pH to the acidity, basicity, or neutrality of a solution.

Guiding Questions

How do we measure the amount of hydronium ion concentration in solutions?

How do we calculate the pH of solutions?

Vocabulary

Acid: A compound which, when dissolved in water, gives a pH of less than 7.0, or donates a hydrogen ion.
Base: A substance that accepts a proton and has a pH above 7.0. A common example is sodium hydroxide (NaOH).
pH: A logarithmic scale used to specify the acidity or basicity of an aqueous solution. The pH scale approximates the negative of the base-10 logarithm of the molar concentration of hydrogen ions in a solution. At room temperature, pure water is neutral (pH = 7); solutions with a pH less than 7 are acidic and those with a pH greater than 7 are basic.
Concentration: The abundance of a constituent of a mixture divided by the total volume of the mixture. Several different definitions of concentration are widely used in chemistry, including mass concentration, volume concentration, and molar concentration.
Molarity: A measure of the concentration of a chemical species, especially of a solute in a solution, in terms of the amount of the species per unit volume of solution. Molarity is typically expressed in units of moles per liter (mol/L); a solution with a concentration of exactly 1 mol/L is commonly said to be 1 molar, symbolized as 1 M. Contrast molality.

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