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Chapter 17: Problem 1

What is the difference between an ion product and an ion product constant?

Short Answer

Expert verified
The ion product varies with the concentrations of the ions in a solution and can change with different conditions. In contrast, the ion product constant (Ksp) is a specific value for a salt in a saturated solution at equilibrium and does not change unless conditions such as temperature change.

Step by step solution

01

Understanding Ion Product

The ion product refers to the product of the concentrations of the ions that form a salt in a solution. It is calculated by multiplying the molar concentrations of the cation and the anion that comprise the salt. This value can change depending on the conditions of the solution, such as temperature and concentrations.
02

Understanding Ion Product Constant (Ksp)

The ion product constant, often represented as Ksp (solubility product constant), is a specific value for a given salt at a particular temperature. It is the ion product at the point where the salt is in dynamic equilibrium with its dissolved ions in a saturated solution. Unlike the ion product, the Ksp is a fixed value under constant conditions.
03

Distinguishing Between Ion Product and Ksp

The main difference between the ion product and the ion product constant is that the ion product can vary with the immediate conditions of the solution, while Ksp is a constant that applies to a saturated solution of the salt at equilibrium under a given set of conditions (usually at a specific temperature). The ion product is used to determine the state of the solution (unsaturated, saturated, or supersaturated) by comparing it with the Ksp.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ion Product
When you mix a salt with water, it may start to dissolve, breaking apart into its positive and negative ions. The 'ion product' is a way of looking at the situation at any moment – it's like building a block tower and counting blocks along the way. You take the number of blocks (or molar concentrations) for the positive part of the salt, called the 'cation', and multiply it by the number of blocks for the negative part, the 'anion'. This number isn't always the same – it changes if you add more blocks, take some away, or even if you move from the living room to the kitchen (that's like changing the temperature).
Solubility Product Constant (Ksp)
But imagine if you learned the best way to build your block tower so it's just right – not falling over, but also not missing any pieces. That's the 'solubility product constant', or Ksp. It's like the perfect tower recipe for each salt in water. For each salt, when it's just starting to have bits left over and not dissolving anymore, that's when you use Ksp. It's a special, steady number that doesn't change unless you drastically change something like the thermostat (temperature). It's super important because it helps predict if you'll end up with leftover salt at the bottom of the glass (precipitate) or if it all mixes in.
Equilibrium Chemistry
Think about a dance party in a room where dancers (ions) come and go into and out from the dance floor (solution). The music (temperature) makes them move faster or slower. This party is hopping when an equal number of dancers enter and leave the dance floor. That's 'equilibrium' in science words. It's a special balance point and everything seems steady. For solubility, this means the amount of salt dissolving is the same as the amount coming back together. It’s a bit like magic, everything looks the same, but there's a lot of dancing (movement) going on that you can't see!
Molar Concentrations
Numbers are super handy, aren’t they? They help us describe how much stuff we’ve got. 'Molar concentrations' are kind of like telling how many apples are in your shopping bag, but for tiny, tiny things like ions. It's a count of how many ion 'apples' are packed into one liter of 'shopping bag' – or water in our case. The more you have, the stronger the taste, like a really sugary lemonade. Scientists use a cool unit, called a 'mole', to count these little particles because there are soooo many of them, and 'concentrations' is just how squished they are in a space. So, molar concentrations tell you how strong or weak your salt water is.

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Most popular questions from this chapter

Suppose two silver wires, one coated with silver chloride and the other coated with silver bromide, are placed in a beaker containing pure water. Over time, what if anything will happen to the compositions of the coatings on the two wires? Justify your answer.

Suppose that some dipositive cation, \(M^{2+},\) is able to form a complex ion with a ligand, \(L\), by the following balanced equation: \(M^{2+}+2 L \rightleftharpoons M(\mathrm{~L})_{2}^{2+} .\) The cation also forms a sparingly soluble salt, \(M \mathrm{Cl}_{2}\). In which of the following circumstances would a given quantity of ligand be more able to bring larger quantities of the salt into solution? Explain and justify the calculation involved: (a) \(K_{\text {form }}=1 \times 10^{2}\) and \(K_{\text {sp }}=1 \times 10^{-15}\), (b) \(K_{\text {form }}=1 \times 10^{10}\) and \(K_{\mathrm{sp}}=1 \times 10^{-20}\).

Write the equilibria that are associated with the equations for \(K_{\text {inst }}\) for each of the following complex ions. Write also the equations for the \(K_{\text {inst }}\) of each: (a) \(\mathrm{Hg}\left(\mathrm{NH}_{3}\right)_{4}^{2+},\) (b) \(\mathrm{SnF}_{6}^{2-}\), (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\).

Write the equilibria that are associated with the equations for \(K_{\text {form }}\) for each of the following complex ions. Write also the equations for the \(K_{\text {form }}\) of each: (a) \(\mathrm{Hg}\left(\mathrm{NH}_{3}\right)_{4}^{2+},\) (b) \(\mathrm{SnF}_{6}^{2-}\), (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\).

Why do we not use \(K_{\mathrm{sp}}\) values for soluble salts such as \(\mathrm{NaCl}\) ?
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