Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Some kidney stones form by the precipitation of calcium oxalate monohydrate (CaC2O4·H2O, Ksp = 2.3 × 10−9). The pH of urine varies from 5.5 to 7.0, and the average [Ca 2+] in urine is 2.6 × 10−3 M.(a)

Problem

Some kidney stones form by the precipitation of calcium oxalate monohydrate (CaC2O4·H2O, Ksp = 2.3 × 10−9). The pH of urine varies from 5.5 to 7.0, and the average [Ca 2+] in urine is 2.6 × 10−3 M.

(a) If the [oxalic acid] in urine is 3.0 × 10−13 M, will kidney stones form at pH = 5.5?