Advertisements
Advertisements
प्रश्न
What is the effect of temperature on solubility of solids in water? Give examples.
Advertisements
उत्तर
1. The effect of temperature on solubility of a substance depends on enthalpy of solution.
a. When the substance dissolves in water by an endothermic process, that is, with the absorption of heat, its solubility increases with an increase of temperature.
e.g. KCl dissolve in water by endothermic process.
b. On the other hand, when the substance dissolves in water by an exothermic process, that is, with the release of heat, its solubility decreases with an increase of temperature.
e.g. CaCl2 and Li2SO4.H2O dissolve in water releasing heat.
2. It is important to understand that there is no direct correlation between solubility and exothermicity or endothermicity. For example, dissolution of CaCl2 in water is exothermic and that of NH4NO3 is endothermic. However, the solubility of these substances increases with the temperature
APPEARS IN
संबंधित प्रश्न
The solubility of a gas in water ______.
The Henry’s law constant of a gas is 6.7 × 10–4 mol/(L bar). Its solubility when the partial pressure of the gas at 298 K is 0.65 bar is ______.
Which of the following 0.10 m aqueous solutions will have maximum ΔTf value?
The solubility of the following salts in water increases with increase in temperature, EXCEPT:
Which of the following is INCORRECT?
Which among the following is true for the value of Henry's law constant K?
The Henry's law constant for oxygen is 1.3 × 10-3 mol dm-3 atm-1. If partial pressure of oxygen is 0.46 atmosphere, what is the concentration of dissolved oxygen at 25°C and 1 atm pressure?
Solubility of a gas in liquid increases with ______.
Henry's law is a relation between ______.
Value of Henry’s constant KH ______.
Which of the following is strongest nucleophile?
What is Henry's law?
According to the Le-Chatelier principle, adding heat to a solid \[\ce{<=>}\] liquid equilibrium will cause the ______.
The solubility (in mol L−1) of AgCl (Ksp = 1.0 × 10−10) in a 0.1 M KCl solution will be ______.
The solubility of a gas in a liquid is directly proportional to the pressure of the over the solution is stated by ______.
`"K"_"sp"` for HgSO4 is `6.4 xx 10^-5`, what is the solubility of the salt?
How does entropy change in the following process? Explain.
Dissolving sugar in water
The solubility of N2 gas in water at 25° C and 1 bar is 6.85 × 10−4 mol L−1. Calculate KH (Henry’s law constant).
Depending on the states of solute and solvent there are ______ types of solutions.
Henry's constant for \[\ce{CH3Br_{(g)}}\] is 0.159 mol dm−3 bar−1 25°C. Calculate its solubility in water at 25°C, if its partial pressure is 0.164 bar.
Calculate the concentration of dissolved gas in water at 25°C if partial pressure of gas at same temperature is 0.15 atm. [KH = 0.15 mol dm-3 atm-1]
People living at high altitudes often reported with a problem of feeling weak and inability to think clearly. The reason for this is:
Which among the following salts dissolves in water with the absorption of heat?
Calculate Henry’s law constant if solubility of nitrogen gas in water at 25°C is 6.85 × 10–4 mol dm–3.
[Partial pressure of nitrogen gas = 0.9 bar]
