Textbook Question
Determine if each anion acts as a weak base in solution. For those anions that are basic, write an equation that shows how the anion acts as a base. a. Br– b. ClO– c. CN– d. Cl–
1124
views
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
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. c. NO3–
1243
views
Textbook Question
Determine the [OH–] and pH of a solution that is 0.140 M in F–.
1688
views
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+
657
views
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+
382
views
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+
672
views