Textbook Question
Pick the stronger base from each pair. a. F– or Cl– b. NO2– or NO3–
Ch.16 - Acids and Bases
Chapter 16, Problem 9
Determine the concentrations of OH-, pH, and pOH of a solution that is 0.125 M in CO32-.
Verified step by step guidance1
Identify the relevant equilibrium reactions for carbonate ion (\( \text{CO}_3^{2-} \)) in water: \( \text{CO}_3^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{HCO}_3^{-} + \text{OH}^- \).
Use the equilibrium constant expression for the reaction: \( K_b = \frac{[\text{HCO}_3^-][\text{OH}^-]}{[\text{CO}_3^{2-}]} \).
Assume initial concentration of \( \text{CO}_3^{2-} \) is 0.125 M and set up an ICE table to find changes in concentration at equilibrium.
Solve for \([\text{OH}^-]\) using the equilibrium expression and the known \( K_b \) value for carbonate ion.
Calculate pOH from \([\text{OH}^-]\) using the formula \( \text{pOH} = -\log[\text{OH}^-] \) and then find pH using \( \text{pH} = 14 - \text{pOH} \).
Related Practice
Open Question
Both HCO3- and HS- are amphoteric. Write an equation to show how each substance can act as an acid, and another equation to show how each can act as a base.
Open Question
A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka) for the acid.
Textbook Question
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. c. KOH(aq)
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Open Question
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base in aqueous solution according to the Arrhenius definition. a. NaOH(aq) b. H2SO4(aq) c. HBr(aq) d. Sr(OH)2(aq)
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH–(aq)
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