Consider the weak bases below and their Kb values: NH₃: Kb = 1.8 × 10⁻⁵ C₂H₅NH₂: Kb = 5.6 × 10⁻⁴ C₅H₅N: Kb = 1.7 × 10⁻⁹ Arrange the conjugate acids of these weak bases in order of increasing acid strength. Solution: The higher the Kb value, the stronger the base. The stronger the base, the weaker its conjugate acid is. Conjugate acid has one more hydrogen then the base, conjugate acids are C₂H₅NH₃⁺, NH₄⁺, C₅H₅NH⁺ The answer is: C₂H₅NH₃⁺<NH₄⁺<C₅H₅NH⁺

Calculate the pH of 250. mL of a 0.0205 M barium hydroxide solution at 25 °C. Solution: Barium hydroxide, Ba(OH) 2 is a strong base because it consists of a group 2 metal and OH. [OH-]=2* 0.0205 M = 0.041 pOH=-log[OH-]= -log( 0.041)= 1.387 pH=14-pOH=12.613 LINKS: General Chemistry Tutoring General Chemistry Study Guides LearnWithMayya