Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee 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: 2K3PO4 (aq) + 3MgCl2 (aq) → Mg 3(PO4)2 (s) + 6KCl (aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine i

Solution: 2K3PO4 (aq) + 3MgCl2 (aq) → Mg 3(PO4)2 (s) + 6KCl (aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine i

Problem

2K3PO4 (aq) + 3MgCl2 (aq) → Mg 3(PO4)2 (s) + 6KCl (aq) 

The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine ions that would be present in solution. 

Be sure to consider both the coefficients and subscripts of the molecular equation, and then write this precipitation reaction in the form of a balanced complete ionic equation. 

Express your answer as a chemical equation including phases.