<p>Hello!</p>
<p>In a given water solvent, why increasing temperature increases solubility of solid solute in general while increasing temperature decreases solubility of gas solute? And why increasing pressure of container increases solubility of gas solute while pressure has almost no effect on solid solute?</p>
<p>Hello^^</p>
<p>So, basically, since gas particles are moving freely about, increasing temperature will make them move more and thus prevent them from dissolving (the added heat speeds them up, increasing kinetic energy). For a solid, increased heat helps break the bonds that hold the particles together, so that they can dissolve more easily.</p>
<p>Increase in pressure follows Henry’s Law: “The solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution.”
So when you increase pressure of container, the gas is forced to dissolve. This is how soda cans work, when you open them up, the pressure on top decreases and the gas gets out. It has no effect on solids since the molecules are not moving around much.</p>
<p>Thanks very much!</p>
<p>I have one more question…since increasing temperature in solution makes gaseous solute particles to move more freely, shouldn’t them collide much more with whole solution and dissolve faster due to collision?</p>