pH of Acids and Bases

Arrhenius Acid Base Acids = H+, Bases = OH-

Modified Arrhenius Uses the idea that the substance will react with water to form H3O+ instead of just H+ Acids = H3O+, Bases = OH-

[H3O+][OH-] = 1.00x10-14

Example 1 What Is the hydroxide ion concentration in a solution with a hydronium ion concentration of 2.59x10-4M?

Example 2 If 2.50g of NaOH was dissolved in water to produce 500mL of solution, what would be the concentration of hydronium and hydroxide ions in solution?

Sig Figs and pH The number of significant digits in the concentration is the number of decimal places in the pH

Example 3 What is the pH of a solution of 0.159M HCl?

Example 4 What is the hydronium and hydroxide ion concentration of a solution with a pH of 2.42?

pOH Potency power of hydroxide!!! Used for BASES!! pOH = -log [OH-] [OH-] = 10-pOH

pH + pOH = 14.00

Example 5 A solution has a pH of 5.750. What are the hydronium ion and hydroxide ion concentrations?

Example 6 A solution has a hydronium ion concentration of 1.95x10-4M. What are the pH, pOH and [OH-] values? pH = 3.710 pOH = 10.290 [OH-] = 5.13x10-11M

Example 7 A solution of Calcium hydoxide was created using 5.673g of solid in 250.00mL of solution. What is the pH, pOH, [OH-] and [H3O+]??? [OH-] = 0.6124M pOH = 0.2130 pH = 13.7870 [H3O+] = 1.633x10-14M