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2K3[Fe(CN)6] + 6Na2[PtCl6] 💧→ 3K2[PtCl6]↓ + 2FeCl3 + 12NaCN + 3PtCl4

2K₃[Fe(CN)₆] + 6Na₂[PtCl₆] 💧→ 3K₂[PtCl₆]↓ + 2FeCl₃ + 12NaCN + 3PtCl₄

Last updated: June 13, 2022

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 6Na₂[PtCl₆]Sodium hexachloridoplatinate(IV)
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3K₂[PtCl₆]↓Potassium hexachloridoplatinate(IV) + 2FeCl₃Iron(III) chloride + 12NaCNSodium cyanide + 3PtCl₄Platinum(IV) chloride

The reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV) yields potassium hexachloridoplatinate(IV), iron(III) chloride, sodium cyanide, and platinum(IV) chloride (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:

Precipitation reaction

Table of contents

Reaction data

Chemical equation

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Potassium hexacyanidoferrate(III) + 6Na₂[PtCl₆]Sodium hexachloridoplatinate(IV)
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3K₂[PtCl₆]↓Potassium hexachloridoplatinate(IV) + 2FeCl₃Iron(III) chloride + 12NaCNSodium cyanide + 3PtCl₄Platinum(IV) chloride

General equation

Precipitation reaction: Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
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Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV)

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
K₃[Fe(CN)₆]	Potassium hexacyanidoferrate(III)	2	Lewis acid	Very soluble in water
Na₂[PtCl₆]	Sodium hexachloridoplatinate(IV)	6	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
K₂[PtCl₆]	Potassium hexachloridoplatinate(IV)	3	Lewis conjugate	Slightly soluble in water
FeCl₃	Iron(III) chloride	2	Non-redox product	–
NaCN	Sodium cyanide	12	Non-redox product	–
PtCl₄	Platinum(IV) chloride	3	Non-redox product	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Crystalline solid + 6Na₂[PtCl₆]Crystalline solid
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3K₂[PtCl₆]↓Crystalline solid + 2FeCl₃Crystalline solid + 12NaCNCrystalline solidcubic + 3PtCl₄Crystalline solid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	962.8	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	481.4	–	–	–
per 1 mol of Sodium hexachloridoplatinate(IV)	160.5	–	–	–
per 1 mol of Potassium hexachloridoplatinate(IV)	320.9	–	–	–
per 1 mol of Iron(III) chloride	481.4	–	–	–
per 1 mol of Sodium cyanide	80.23	–	–	–
per 1 mol of Platinum(IV) chloride	320.9	–	–	–

Changes in standard condition (2)

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Crystalline solid + 6Na₂[PtCl₆]Crystalline solid
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3K₂[PtCl₆]↓Crystalline solid + 2FeCl₃Crystalline solid + 12NaCNCrystalline solidorthorhombic + 3PtCl₄Crystalline solid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	923.7	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	461.9	–	–	–
per 1 mol of Sodium hexachloridoplatinate(IV)	154.0	–	–	–
per 1 mol of Potassium hexachloridoplatinate(IV)	307.9	–	–	–
per 1 mol of Iron(III) chloride	461.9	–	–	–
per 1 mol of Sodium cyanide	76.98	–	–	–
per 1 mol of Platinum(IV) chloride	307.9	–	–	–

Changes in aqueous solution (1)

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Ionized aqueous solution + 6Na₂[PtCl₆]Crystalline solid
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3K₂[PtCl₆]↓Ionized aqueous solution + 2FeCl₃Un-ionized aqueous solution + 12NaCNIonized aqueous solution + 3PtCl₄Aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	–	–	–	–
per 1 mol of Sodium hexachloridoplatinate(IV)	–	–	–	–
per 1 mol of Potassium hexachloridoplatinate(IV)	–	–	–	–
per 1 mol of Iron(III) chloride	–	–	–	–
per 1 mol of Sodium cyanide	–	–	–	–
per 1 mol of Platinum(IV) chloride	–	–	–	–

Changes in aqueous solution (2)

Reaction of potassium hexacyanidoferrate(III) and sodium hexachloridoplatinate(IV): 2K₃[Fe(CN)₆]Ionized aqueous solution + 6Na₂[PtCl₆]Crystalline solid
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3K₂[PtCl₆]↓Ionized aqueous solution + 2FeCl₃Ionized aqueous solution + 12NaCNIonized aqueous solution + 3PtCl₄Aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	450.8	–	–	–
per 1 mol of Potassium hexacyanidoferrate(III)	225.4	–	–	–
per 1 mol of Sodium hexachloridoplatinate(IV)	75.13	–	–	–
per 1 mol of Potassium hexachloridoplatinate(IV)	150.3	–	–	–
per 1 mol of Iron(III) chloride	225.4	–	–	–
per 1 mol of Sodium cyanide	37.57	–	–	–
per 1 mol of Platinum(IV) chloride	150.3	–	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
K₃[Fe(CN)₆] (cr)	-249.8^[1]	-129.6^[1]	426.06^[1]	–
K₃[Fe(CN)₆] (ai)	-195.4^[1]	-120.4^[1]	577.8^[1]	–
Na₂[PtCl₆] (cr)	-1115.9^[1]	–	–	–
Na₂[PtCl₆] (cr) 2 hydrate	-1723.8^[1]	–	–	–
Na₂[PtCl₆] (cr) 6 hydrate	-2912.1^[1]	–	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
K₂[PtCl₆] (cr)	-1229.3^[1]	-1078.5^[1]	333.9^[1]	205.60^[1]
K₂[PtCl₆] (ai)	-1172.8^[1]	-1049.2^[1]	424.7^[1]	–
FeCl₃ (cr)	-399.49^[1]	-334.00^[1]	142.3^[1]	96.65^[1]
FeCl₃ (g)	-254.0^[1]	–	–	–
FeCl₃ (ai)	-550.2^[1]	-398.3^[1]	-146.4^[1]	–
FeCl₃ (ao)	–	-404.5^[1]	–	–
FeCl₃ (cr) 6 hydrate	-2223.8^[1]	–	–	–
NaCN (cr) cubic	-87.49^[1]	-76.43^[1]	115.60^[1]	70.37^[1]
NaCN (cr) orthorhombic	-90.75^[1]	–	–	–
NaCN (g)	109^[1]	79.94^[1]	249.43^[1]	51.17^[1]
NaCN (ai)	-89.5^[1]	-89.5^[1]	153.1^[1]	–
NaCN (cr) 1/2 hydrate	-235.77^[1]	–	–	–
NaCN (cr) 2 hydrate	-679.77^[1]	–	–	–
PtCl₄ (cr)	-231.8^[1]	–	–	–
PtCl₄ (aq)	-314.2^[1]	–	–	–
PtCl₄ (cr) 5 hydrate	-1752.7^[1]	–	–	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (aq):Aqueous solution

References

List of references

1
Janiel J. Reed (1989)
The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
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