It is influenced by surroundings. 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. 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. Any glassware, as well as the filer paper, must be dry in order to calculate an accurate concentration of IO 3 —. Rinse a mL pipet with two small portions of the saturated Ca IO 3 2 solution. You may discard any rinse solutions down the drain. Pipet In a titration an indicator is often used and these indicators exhibit vivid color in solution.
If we add excess I — to the solution done in this experiemnt by adding solid KI and excess acid in this case 3 M HCl will work just fine , then all of the IO 3 — aq will be oxidized to I 2 aq. We can verify that I 2 aq is present due to its brown color in solution. As the second step of the reaction sequence indicates, whenever thiosulfate S 2 O 3 2— is added to a solution of I 2 , the I 2 aq will be reduced to I — aq. Whenever a small amount of I 2 aq is in the presence of a starch indicator, a dark blue complex will form.
When the solution turns from blue or brown to colorless, we know that all of the I 2 aq has been reduced to I — aq.
In addition, add about 10 mL of 3 M HCl and swirl. This is converting all of the IO 3 — aq to I 2 aq , which will turn the solution brown. This is consistent with the following equation:. Now we are ready to perform the titration with standardized 0. Find the 0. Use this solution to rinse a mL buret twice, then perform three titrations.
In each of your titrations, fill the mL buret with 0. This constant is called solubility product constant or K sp.
Main menu Ksp solubility product Solubility basics Solubility of alcohol Solubility of salts Water solubility. What is Ksp solubility constant? The stoichiometry of the formula of the ionic compound dictates the form of the expression. For example the formula of calcium phosphate is Ca 3 PO 4 2. The dissociation equation and expression are shown below:. The Table below lists solubility product constants for some common nearly insoluble ionic compounds. Skip to main content.
Search for:. Perform calculations involving solubility product constants.
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