Heat of Dilution
Chemistry ⇒ Thermochemistry and Energetics
Heat of Dilution starts at 11 and continues till grade 12.
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Describe how you would experimentally determine the heat of dilution for a salt solution.
Describe what happens to the heat of dilution as the concentration of a solution approaches zero.
Explain the difference between heat of solution and heat of dilution.
Explain why the heat of dilution approaches zero as the solution becomes very dilute.
A 1 M solution of HCl is diluted to 0.1 M. If the molar heat of dilution is -1.7 kJ/mol, how much heat is released when 0.2 mol HCl is diluted?
A solution of KNO3 absorbs heat when diluted. Is the heat of dilution positive or negative?
A student adds 100 mL of water to 100 mL of 2 M NaOH solution. If the molar heat of dilution is -2.0 kJ/mol, how much heat is released?
A student observes that the temperature of a solution increases upon dilution. What can be inferred about the heat of dilution?
The heat of dilution is generally greater for (1) strong electrolytes, (2) weak electrolytes, (3) non-electrolytes, (4) all are equal.
The heat of dilution is generally more significant for which type of solute? (1) Ionic compounds, (2) Covalent compounds, (3) Gases, (4) Metals
The heat of dilution is important in which of the following industries? (1) Chemical manufacturing, (2) Food processing, (3) Pharmaceuticals, (4) All of the above
The heat of dilution is measured in which unit? (1) Joules, (2) Calories, (3) kJ/mol, (4) All of the above
If the heat of dilution is positive, the process is ________.
The heat of dilution for a solution is zero when the solution is ________.
The heat of dilution is a type of ________ change.
The heat of dilution is always measured at constant ________.
State whether the following statement is true or false: The heat of dilution is always negative.
True or False: The heat of dilution can be determined using a calorimeter.
True or False: The heat of dilution is a state function.
True or False: The heat of dilution is always measured per mole of solute.
