- Oxidation–reduction (redox) reactions
- Worked example: Using oxidation numbers to identify oxidation and reduction
- Balancing redox equations
- Dissolution and precipitation
- Precipitation reactions
- Double replacement reactions
- Single replacement reactions
- Molecular, complete ionic, and net ionic equations
- Molecular, complete ionic, and net ionic equations
- 2015 AP Chemistry free response 3a
Dissolution and precipitation
Defining solute, solvent, hydration, dissolution, precipitation, net ionic equation, and spectator ions. Looking at the molecular level interactions between water and ions in NaCl. Created by Jay.
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- How do you know that the ionic crystal is AgCl(s). How come the solid is not NaNO3?(95 votes)
- solubility rules: AgCl will always be insoluble, but all alkali metal salts are soluble(97 votes)
- 1. Why does NaCl dissolve in water?. Isn't the electrostatic force to keep the ionic lattice greater than the attraction of the water molecules for the ions?
2. If all four compounds (NaCl, Ag(NO)3, AgCl and Na(NO)3) are ionic, why do NaCl, Ag(NO)3, Na(NO)3 all soluble in water but not AgCl?(29 votes)
- The exact reason is not simple and involves quantum mechanics. That said, many ionic solids, such as silver chloride (AgCl) do not dissolve in water because the forces holding the solid AgCl lattice together are too strong to be overcome by the forces favoring the formation of the hydrated ions, Ag+(aq) and Cl-(aq). Other salts and compounds that you mention will have different binding strength in a lattice, so some will dissolve, and others won't.(14 votes)
- why does he write 8- when he writes that Oxygen is partially negative and 8+ when he writes that Hydrogen is partially positive?(6 votes)
- It's really a lower-case Greek letter delta (δ). δ⁻ means "partially negative", and δ⁺ means "partially positive".(39 votes)
- What is a dipole at1:45?(6 votes)
- A dipole is a molecule in which a concentration of positive electric charge is separated from a concentration of negative charge.
Water is a dipole because it has a partially negative oxygen end, while the hydrogen atoms are at the positive end.(22 votes)
- When NaCl is dissolved in water, it dissociates into Na+ and Cl-. Does this mean, that Na and Cl are attracted more to water than to itself? Isn't ionic bond strong..? I understand that polar molecules dissolves in water, but the fact that ionic compound dissolves,, is not intuitive to me...(11 votes)
- Some ionic bonds are stronger than others - they're not all of equal strength. Thus the ionic bond between Ag+ and Cl- is stronger than between Na+ and Cl-.(11 votes)
- When NaCl bonds are broken in the solution, is any energy needed to do so? If yes,shouldn't the water/solution become colder?(8 votes)
- Nice point and for NaCl this will happen (although only by an extremely small amount, barely if at all noticeable)! If it takes more energy to separate the particles of the solute than is released when the water molecules bond to the particles, then the temperature goes down (endothermic).(8 votes)
- How come Ag+ and Cl- form AgCl but Na+ and NO3- do not form NaNO3?
Sodium and nitrate are also charged oppositely, shouldn't they attract?(7 votes)
- Some salts are soluble in water, and some salts aren't soluble in water. Added to which there are degrees of solubility, with some salts being more soluble than other salts.
It all depends on whether the ionic crystal state (AgCl or NaNO3) is more thermodynamically favoured than the solvated ions (Ag+ and Cl- or Na+ and NO3-). By solvated, I mean that water molecules surround the ions and stabilise them so that they prefer to be in solution rather than sitting as a crystals at the bottom of the beaker.
If ionic substances never dissolved in water then there would be no life as we know it.(8 votes)
- At1:27, they bring up the concept of water splitting Sodium Chloride into their individual parts. If this is the case, why does salt water still taste salty, if in fact you are tasting Chlorine and Sodium separately?(4 votes)
- Because it's the sodium ions that our tongues detect as being salty.(4 votes)
- At7:28, what does spontaneously mean?(3 votes)
- With no additional energy / it will naturally just happen.
This will also mean that delta G (change in free energy) is negative(8 votes)
- My friend has told me dissolution is the same as ionization. Is this true?(2 votes)
- Technically no they are different processes. Dissolution refers to a solute dissolving into a solvent to create a solution. While ionization means when an atom or molecule acquires a positive or negative charge by gaining or losing an electron.
I can ionize sodium metal by bombarding it with high energy radiation. The radiation removes sodium's valence electron to turn it into a sodium cation, Na+, which I was able to do without involving dissolution.
I an also dissolve something that is soluble in water without creating ions. Table sugar, or sucrose, easily dissolves into a polar solvent like water, but still remains a neutral molecule of sugar in solution.
Even dissolving a salt like sodium chloride, NaCl, into water technically doesn't count as ionization since the sodium cations and chloride anions are already present in a salt crystal. Dissolution only serves to separate those ions from each other by surrounding them with water molecules. Hope this helps.(5 votes)
- [Voiceover] Let's say we have some solid sodium chloride, so some salt. And that right there is supposed to be our pile of salt. We're going to put our salt into some water. We have a beaker containing H2O. The sodium chloride is going to dissolve in the water. So the sodium chloride is our solute and the water will be our solvent. This is the process of dissolution. If you look more closely at sodium chloride, solid sodium chloride is an ionic crystal. It's held together by the ionic bonds, right? So the sodium cation, or the positive charge, is attracted to the chloride anion with a negative charge. That's holding together our ionic crystal. When you put the solid sodium chloride into water, remember, water is a polar molecule. The oxygen is more electronegative than the hydrogens here. So the oxygen gets a partial negative charge and these hydrogens get a partial positive charge. So we have a polar molecule here. The negative charge on the oxygen is going to interact with the positive charge on the sodium. Right? Opposite charges attract. We have one water molecule here attracted to this sodium cation, and this water molecule would do the same, right? So partial negative charge attracted to the positive charge on the sodium. So the water molecules are going to pull off the sodium cations and eventually give you this situation over here. We have the partial negative oxygens, right? Partial negative oxygens are going to interact with the sodium cation, right? So the water is a dipole and the sodium cation is an ion. So we could call this an ion-dipole interaction. The water molecules break the ionic bonds, pull off the sodium cations, surround the sodium cation. We call this process hydration. This is the process of hydration, where the ion is surrounded and stabilized by a shell of our solvent molecules. The same thing would happen with the chloride anions. Right up here, the chloride anion is negatively charged. But this time, the negative charge would be attracted to the positive part of our polar molecule, right? The oxygen is partially negative and this hydrogen here would be partially positive. Opposite charges attract, the positive charge is going to interact with the negative charge. Same for this molecule of water, partially positive hydrogen. Once again, this interaction is going to pull off that chloride anion and move it into solution. So we have our partial positive hydrogens interacting with our negatively-charged chloride anions here. Once again, we get ion-dipole interactions. The chloride anion is surrounded by our water molecules, so once again, the process of hydration. The end result is, each sodium cation is surrounded by water molecules and each chloride anion is surrounded by water molecules. The sodium chloride has dissolved in water. We formed a solution, an aqueous solution, of sodium chloride. The way that you see that written, you would write, here we have solid sodium chloride, which we put into water, our solvent, and the water molecules surrounded our ions. Now we have sodium ions in solution, so we write an aq here for aqueous sodium ions, and we have chloride anions also in solution, so we write an aq here. So we have an aqueous solution of sodium chloride. The sodium chloride has dissolved in water. Now let's say we have one beaker that contains a solution of NaCl, so an aqueous solution of NaCl has sodium cations in solution and chloride anions in solution. Let's say we have another beaker that contains a solution of silver nitrate, which is AgNo3. So an aqueous solution of silver nitrate means we have silver cations in solution, Ag+, and nitrate anions, No3-. Now let's say we add the contents of one beaker to the other beaker. Let's pour the contents of, let's say, this beaker into this beaker. We're combining our two solutions. We would notice a few things. We would notice the volume to increase, obviously, since we're pouring the contents of one into the other. We would also notice a white solid form. A white solid is going to form down here. That white solid forms when the silver cations interact with the cloride anions. We get a solid forming that is silver chloride, AgCl. We would write AgCl here. We put a subscript s, indicating that a solid formed. This solid is called a precipitate. This solid spontaneously falls out of solution. This is the process of precipitation, which is the opposite of dissolution. In dissolution, we put a solid into water and we formed ions, right? In precipitation, the ions come together to form a solid, and that solid spontaneously falls out of solution. Silver chloride is our precipitate. We would still have some ions in solution. We would still have sodium cations and nitrate anions. In here, we would have sodium cations in solution and nitrate anions in solution. We could add them into here. We could say, NaNo3, aqueous, meaning those ions are present in solution. Let's look in more detail about what's happening with the formation of our precipitate. We know that we had silver cations in solution. Here's our silver cation over here. We know that this ion is being surrounded by water molecules in the process of hydration, right? So these oxygens are partially negative right here. Since opposites attract, there's a force that's holding that ion in our solution, the forces of hydration. Same thing for the chloride anion, right? The partial positive charge on the hydrogen, opposite charges attract, right? So those water molecules are stabilizing the chloride anion in solution. But when we pour those two solutions together, we form our precipitate. We form silver chloride. We form this ionic crystal down here. Once again, opposite charges attract. So the positively-charged silver cation is attracted to the negatively-charged chloride anion here. Since we notice this solid to form, the electrostatic attractions of our ionic crystal must be stronger than the forces of hydration. This chloride anion would move into here, and then this silver cation would move into here. So the ions come out of solution and a precipitate spontaneously forms. We form our solid, silver chloride. This is one way to represent what's going on here. We could have also drawn out all of the ions, right? Instead of writing that, another way to represent what's happening would be to say, a solution of sodium chloride would be sodium cations in solution, so we write our sodium cations here, chloride anions, so Cl-. We added to that our solution of silver nitrate, which had silver ions in solution, so Ag+, and nitrate anions, so NO3-. And we saw a precipitate form. We formed AgCl, which is our solid. We write AgCl here, which is our precipitate. Then we also had sodium cations and nitrate anions. We had sodium cations, Na+, and we had nitrate anions, NO3-. That's a lot of writing. Either one tells you the same amount of information. This one down here just shows you all of the ions. Really, only some of the ions are reacting. The silver cation and the chloride anion are coming together to form silver chloride. We could write a net ionic equation showing what's happening to form our precipitate. We could show the silver cations here, Ag+. We could show our silver cations and our chloride anions combining to form our precipitate, AgCl. This is the net ionic equation. This is the net ionic equation because some of our ions aren't taking part in this reaction. They're just observing what's happening. This sodium cation is on the left side. It's also on the right side. It's an ion in solution. Same thing with the nitrate anion. It's over here on the left side as a ion in solution. It's over here on the right side as a ion in solution. The sodium cation and the nitrate anion are called spectator ions. These are called spectator ions because they're not taking part in what's happening. They're just watching. They're watching as the silver chloride precipitates out of solution. That's why we call them spectator ions. So this is the idea of precipitation.