Textbook Question
Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. a. C7H5O2– b. I– d. F–
Ch.16 - Acids and Bases
Chapter 16, Problem 98
Determine the [OH-] and pH of a solution that is 0.250 M in HCO3⁻.
Verified step by step guidance1
Identify the relevant equilibrium reaction for bicarbonate ion (HCO₃⁻) in water: HCO₃⁻ + H₂O ⇌ H₂CO₃ + OH⁻.
Write the expression for the equilibrium constant (K_b) for the reaction: K_b = [H₂CO₃][OH⁻]/[HCO₃⁻].
Use the relationship between K_w, K_a, and K_b to find K_b for HCO₃⁻: K_b = K_w / K_a, where K_w is the ion-product constant of water (1.0 x 10⁻¹⁴) and K_a is the acid dissociation constant for H₂CO₃.
Set up an ICE (Initial, Change, Equilibrium) table to determine the changes in concentration of HCO₃⁻, H₂CO₃, and OH⁻ at equilibrium.
Solve for [OH⁻] using the K_b expression and the values from the ICE table, then calculate pH using the relationship pH + pOH = 14.
Related Practice
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