What do ksp values tell you

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How to Write an Amazing College Essay. A Comprehensive Guide. Choose Your Test. For these equations: A and B represent different ions and solids. In these equations, they are also referred to as "products". So [AgCl] represents the molar concentration of AgCl.

First, we need to write out the two equations. In this section, we discuss the main factors that affect the value of the solubility constant. Temperature Most solutes become more soluble in a liquid as the temperature is increased. Pressure Pressure can also affect solubility, but only for gases that are in liquids.

A saturated solution is in a state of equilibrium between the dissolved, dissociated, undissolved solid, and the ionic compound. Austin State University with contributing authors. Introduction Recall that the definition of solubility is the maximum possible concentration of a solute in a solution at a given temperature and pressure. Calculation of K sp from Equilibrium Concentrations We began the chapter with an informal discussion of how the mineral fluorite is formed.

Solution The solubility product constant of copper I bromide is 6. Summary Solubility is defined as the maximum amount of solute that can be dissolved in a solvent at equilibrium. You should observe a white precipitate. Note: These volume measurements do not need to be exact, so you can use a graduated cylinder to add the solutions to the beaker.

To do this we must separate or filter them from the solid Ca IO 3 2. The magnitude of the K sp is proportional to how much solid Ca IO 3 2 will dissolve. Similar to Figure 2, assemble a ring, clay triangle, and funel with filter in order to perform a gravity filtration. Fold a piece of filter paper in half, then fold it in half again. In order to fit the filter paper snugly inside the funnel, tear off a small part of the corner as shown in the video below.

Open the filter paper so that one side of the funnel is in contact with a single layer of the filter paper and the other side of the funnel is in contact with three layers of the filter paper. It seems to work best if the side with the tear has three layers. The paper should be in smooth contact with the funnel at the top, but not near the point. Squirting in water with a wash bottle sometimes helps to keep the filter paper in place.

Take the mL beaker from Step 1 and pour as much supernatant liquid through the filter paper as possible, trying your best not to disturb the precipitate. Use a wash bottle filled with distilled water to wash down the sides of the beaker.

Swirl the wash water with the solid and quickly pour the mixture on the filter paper. Rinse any remaining solid onto the filter paper with a small amount of water from your wash bottle.

Wash the solid Ca IO 3 2 on the filter paper with three small portions of distilled water. Leave the left over precipitate on the filter paper. You will only use the precipitate on the filter paper if you mess up one of your trials. Rinse your mL graduated cylinder with distilled water and use it to add 80 mL of distilled water to the beaker containing the wet precipitate.

Acquire a stirring motor from the balance room and a stir bar from your TA. Place the stir bar into the beaker containing your 80 mL of water and your Ca IO 3 2 precipitate. Place your beaker on the stirring motor and turn the stirrer on to its lowest speed setting and allow it to stir in order to obtain a saturated solution.

While you are waiting for your solution to reach equilibrium complete the following problems in your lab notebook, which must be checked off by your TA before you continue. Note: the following problems were taken from Quiz I given during the past two quarters. Example Problem 3. The solubility product constant for Cu IO 3 2 is 1. What volume of 0. Example Problem 4. The solubility product constant for Sr IO 3 2 is 1. Example Problem 5. A titration was performed to determine the solubility product constant K sp of lead iodide.

The first step of the reaction sequence was performed and a starch indicator was added to the solution turning it blue. After 1. From the results of this experiment, calculate the K sp of lead iodide. Once you get your TA to check off these example problems, you are finished with Day 1 of this lab. Write your name on the Erlenmeyer Flask containing your saturated solution with a Sharpie, place Parafilm over the top of the flask, and hand it to your TA.

You will start by filtering this solution at the beginning of the next lab period. In order to ensure you have a saturated solution of Ca IO 3 2 , the mixtures set aside from Step 8 must not contain any solid. Filter the saturated solution in the same manner as Step 2, but for this step use a clean, dry mL Erlenmeyer flask to catch the filtrate.