The diagram shows the enthalpy changes when sodium chloride is dissolved in water. Define the term enthalpy change of solution.

The enthalpy change of solution, ∆ H f is the energy absorbed or released when one mole of an ionic solid dissolves in sufficient water to form a very dilute solution.

The diagram shows the enthalpy changes when sodium chloride is dissolved in water. Define the term enthalpy change of hydration.

The enthalpy change of hydration is the enthalpy change when one mole of aqueous ions are formed from one mole of ions in the gaseous state. The enthalpy change of hydration is always exothermic.

The diagram shows the enthalpy changes when sodium chloride is dissolved in water. Write symbol equation that describe the enthalpy change of solution of sodium chloride.

The enthalpy change of solution for zinc chloride is described by the thermochemical equation given below: NaCl ( s ) + aq → NaCl ( aq ) ∆ H = + 3 . 9 kJ mol - 1 Or, NaCl ( s ) + aq → Na + ( aq ) + Cl - ( aq ) ∆ H = + 3 . 9 kJ mol - 1 Note:- The symbol 'aq' represents the very large amount of water used. A compound is likely to be soluble in water only if ∆ H is negative or has a small positive value. The substances with large positive values of ∆ H are relatively insoluble.

The diagram shows the enthalpy changes when sodium chloride is dissolved in water. Write symbol equation that describe the enthalpy change of hydration of the chloride ion.

The enthalpy change of hydration for a chloride ion is described by the equation below: Cl - ( g ) + aq → Cl - ( aq ) ∆ H hyd ⊝ = - 364 kJ mol - 1 Note:- The standard enthalpy change of hydration, ∆ H sol ⊝ is the enthalpy change when one mole of a specified gaseous ion dissolves in sufficient water to form a very dilute solution under standard conditions.

The diagram shows the enthalpy changes when sodium chloride is dissolved in water. Name the enthalpy changes labelled A, B and C.

In step A, gaseous ions are combining to form an ionic solid crystal. Therefore, the equation represents the lattice enthalpy, ∆ H latt for NaCl . Na + ( g ) + Cl - ( g ) → NaCl ( s ) In step B, gaseous ions Na + and Cl - dissolves in sufficient water to form a very dilute solution. Therefore, the equation represents the enthalpy change of hydration, ∆ H hyd . Na + ( g ) + Cl - ( g ) + aq → Na + ( aq ) + Cl - ( aq ) In step C, 1 mole of ionic solid, NaCl dissolves in sufficient water to form a very dilute solution. Therefore, the equation represents the standard enthalpy change of solution, ∆ H sol for NaCl . NaCl ( s ) → Na + ( aq ) + Cl - ( aq )

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Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 5

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Use ideas about ion polarisation to explain why barium carbonate is more stable to thermal decomposition than magnesium carbonate.

Important Questions on Lattice Energy

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AS and A Level

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Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

The diagram shows the enthalpy changes when sodium chloride is dissolved in water.

Question Image

Define the term enthalpy change of solution.

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

The diagram shows the enthalpy changes when sodium chloride is dissolved in water.

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Define the term enthalpy change of hydration.

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

The diagram shows the enthalpy changes when sodium chloride is dissolved in water.

Question Image

Write symbol equation that describe the enthalpy change of solution of sodium chloride.

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

The diagram shows the enthalpy changes when sodium chloride is dissolved in water.

Question Image

Write symbol equation that describe the enthalpy change of hydration of the chloride ion.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

The diagram shows the enthalpy changes when sodium chloride is dissolved in water.

Question Image

Name the enthalpy changes labelled A, B and C.

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

Draw the water molecules around magnesium ions and sulfate ions in a solution of magnesium sulfate.

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 19 - Lattice Energy>EXAM-STYLE QUESTIONS>Q 6

Explain, in terms of differences of lattice energies and enthalpy changes of hydration, why magnesium sulfate is more soluble in water than calcium sulfate.

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