moongazer
  • moongazer
Why substance dissolve?
Chemistry
  • Stacey Warren - Expert brainly.com
Hey! We 've verified this expert answer for you, click below to unlock the details :)
SOLVED
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.
jamiebookeater
  • jamiebookeater
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
mayankdevnani
  • mayankdevnani
you said that How does a substance dissolve in a solvent? right @moongazer
mayankdevnani
  • mayankdevnani
are you there? @moongazer
mayankdevnani
  • mayankdevnani
by diffusion of particles. The solute particles, which are moving randomly, collide with the solvent particles, break off and diffuse throughout the mixture. The process continues until the substance is spread evenly throughout the mixture. This is called diffusion.

Looking for something else?

Not the answer you are looking for? Search for more explanations.

More answers

moongazer
  • moongazer
@mayankdevnani I'm here now sorry for the late reply I'm doing something :)
moongazer
  • moongazer
Is that only the reason?
moongazer
  • moongazer
My teacher said there are three.
mayankdevnani
  • mayankdevnani
can i copy from my website
mayankdevnani
  • mayankdevnani
it takes much less time and you will get your answer sufficiently
mayankdevnani
  • mayankdevnani
can i?
mayankdevnani
  • mayankdevnani
@moongazer
moongazer
  • moongazer
What do you mean?
mayankdevnani
  • mayankdevnani
just copy and paste
moongazer
  • moongazer
This question is just for my notes so I think you can copy from your website. :) I'll just understand and summarize it. :)
mayankdevnani
  • mayankdevnani
no you will get your answer...plzz for your need
moongazer
  • moongazer
ok
mayankdevnani
  • mayankdevnani
plz wait
mayankdevnani
  • mayankdevnani
Let's consider the dissolving of an ionic substance, such as NaCl. The principles are the same for covalent substances such as sugar. There are edges and corners of the NaCl that are exposed to the solvent, let's say H2O. The dipole H2O is attracted to these areas where the atoms of Na+ and Cl- are sticking out. The water molecules cluster around the ions, hydrating (solvating) them as much as possible. The Heat of Hydration is exothermic, aiding in the breakdown of the ionic bond between the Na- and Cl-. Water molecules are doing the same thing to the Cl-, and with the Heat of Hydraation, the ions are being pulled apart, giving the water molecules a chance to sneak in behind them, further hydrating the ions. If enough water molecules get around the individual ions, they can pull it off from the crystal lattice, and completely surround the ions with concentric layers of waters of hydration. This reduces the effective charge on the ions, so they are not as attractive to the bulk of the remaining crystal lattice, and, due to kinteic energy of the water, are moved away from the lattice. Now more ions are exposed, and the process is repeated: solvation, heat of solvation, attractive forces of the solid being overcome by the solvent particles, as they cluster around solute particles. This process ties up a lot of H2O molecules, as they form the clusters of water around the solute particles, until there comes a situation where there is no more free H2O molecules, and the process appears to stop. This is "saturation", an equilibrium situation, where the ions return to the crystal at the same rate that other ions are leaving the crystal. If you heat the solution, the water particles have greater kinetic energy, and can smash into the undissolved solid with greater force, breaking attractive forces of the solute particles more easily. The Heat of Hydration is a major player in this process, and as more and more sloute particles are solvated, the leftover energy, leftover after the bonds of the crystal lattice have broken, may increase the temperature of the solution. If the Lattice Energy is greater than the Heat of Hydration, then the solution may become cold, or worse, the solute does not dissolve at all, or only a tiny bit. So, The Heat of Hydration provides the energy needed to disrupt attractive forces, and in ionic compounds, overcome the lattice energy, leading to each solute particle to be surrounded by layers and layers of solvent, which prevent the solute particle from rejoining the bulk of the solute.
mayankdevnani
  • mayankdevnani
n chemistry, a solution is a homogeneous mixture composed of two or more substances. In such a mixture, a solute is dissolved in another substance, known as a solvent. A common example is a solid, such as salt or sugar, dissolved in water, a liquid. Gases may dissolve in liquids, for example, carbon dioxide or oxygen in water. Liquids may dissolve in other liquids and gases always mix with other gases.[1] Examples of solid solutions are alloys, certain minerals and polymers containing plasticizers. The ability of one compound to dissolve in another compound is called solubility. The physical properties of compounds such as melting point and boiling point change when other compounds are added. Together they are called colligative properties. There are several ways to quantify the amount of one compound dissolved in the other compounds collectively called concentration. Examples include molarity, molality, and parts per million (ppm). Solutions should be distinguished from non-homogeneous mixtures such as colloids and suspension
mayankdevnani
  • mayankdevnani
ok @moongazer just read it and reply me soon

Looking for something else?

Not the answer you are looking for? Search for more explanations.