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: Calcium ion present in water supplies is easily precipitated as calcite (CaCO 3):Ca2+(aq) + CO32−(aq) ⇌ CaCO3(s)Because the Ksp decreases with temperature, heating hard water forms a calcite “scale,” which clogs pipes and water heaters. Find the solubility of calcite in water (b) at 30°C (Ksp = 3.1 × 10−9)

Problem

Calcium ion present in water supplies is easily precipitated as calcite (CaCO 3):

Ca2+(aq) + CO32−(aq) ⇌ CaCO3(s)

Because the Ksp decreases with temperature, heating hard water forms a calcite “scale,” which clogs pipes and water heaters. Find the solubility of calcite in water 

(b) at 30°C (Ksp = 3.1 × 10−9)