ChemCollective-Virtual-Labs/C3/Determination-of-Solubility-Product/English

Visual Cue	Narration
Slide Number 1 Title Slide	Welcome to this spoken tutorial on Determination of Solubility Product using Vlabs.
Slide Number 2 Learning Objectives	In this tutorial we will learn to, Determine Solubility of salts and Calculate Solubility Product of various sparingly soluble salts.
Slide Number 3 System Requirement	Here, I am using Mac OS version 10.10.5 ChemCollective Vlabs version 2.1.0 and Java version 8.0
Slide Number 4 Pre-requisites www.spoken-tutorial.org	To follow this tutorial you should be familiar with, Chemcollective vlabs interface. If not for relevant tutorials, please visit our website.
Point to the window.	Here, I have opened Virtual Chemistry labs application window.
Click on File >> Load Homework. Point at Default Lab Setup dialog-box. Double- click on Solubility and Solids option. Double- click on Determining the Solubility Product	Click on File menu and select Load Homework option. Default Lab Setup dialog-box opens. Double-click on Solubility and Solids option. From the sub-menu, double-click on Determining the solubility product option.
Cursor on chemicals, apparatus and Problem Description. Double click on Problem Description from Stockroom Explorer.	A workbench opens with required chemicals and Problem Description. Under the Stockroom Explorer double click on Problem Description.
Cursor on Problem Description window. Highlight relevant portions of Problem Description.	Problem Description window opens. The problem states that, using Virtual labs, We have to determine Solubility Products of Silver chloride Strontium Sulphate Silver Carbonate and Strontium Iodate. We have to also find the solubility of the above salts in Moles/Litre. Finally we have to compare the Solubility and Solubility Products for pairs of salts.
Click on 'x' on the top right corner of the window.	Close the Problem Description window.
Slide Number 5 Solubility Product	A substance's solubility product, is the mathematical product of its dissolved ion concentrations raised to the power of their stoichiometric coefficients.
Slide Number 6 Solubility Product: Equation 1 AgCl(s) ⇌ Ag+(aq) + Cl¯(aq) Stoichiometric Concentrations are [Ag+] : [Cl-] 1 : 1 [Ag+] = S, [Cl-] = S Ksp = [Ag+] [Cl¯] Solubility Product = S x S = S2	For Example: Solubility of Silver Chloride in its saturated solution is given as follows: For every one mole of silver chloride that dissolves, one mole of silver ion and one mole of chloride ion is produced. Let us assign a variable S to represent solubility of Silver and Chloride ions. Solubility Product of silver chloride is S squared.
Slide Number 7 Solubility Product: Equation 2 Ag2CO3 ⇌ 2Ag+ + CO3-2 [Ag+] : [CO3-2] 2 : 1 [Ag+] = 2S, [CO3-2] = S Ksp = [Ag+]2 [CO3-2] Solubility Product = (2S)2 x S = 4S3	Here is the solubility of Silver carbonate in its saturated solution. Stoichiometric concentrations of the ions are in the ratio of 2 : 1 In this equation, solubility of silver ion is two S and carbonate ion is S. Solubility Product of silver carbonate is four S cube.
Slide Number 8 Solubility Product: Significance	Significance of Solubility Product. Solubility Product applies to solutions where salts do not fully dissolve. Water is generally used as a solvent. Solubility Product changes with temperature.
Slide Number 9 Solubility Product: Significance	Solubility Product is a heterogeneous equilibrium constant. The smaller the Solubility Product of a substance, the lower is its solubility.
Slide Number 10 Solubility Product: Significance	Solubility Product values are useful in predicting, the precipitation in reactions. when the Ionic product is greater than Solubility Product, then precipitation will occur. when the Ionic product is smaller than Solubility Product, then precipitation will not occur.
Cursor on Vlabs workbench. From the Stockroom Explorer, double-click to select, Silver chloride Strontium Sulphate Silver Carbonate Strontium Iodate.	Back to the workbench. From the Stockroom Explorer, double-click to select, Silver chloride Silver Carbonate Strontium Sulphate and Strontium Iodate.
Click on Select tools icon. Click to select Scale Click on Select tools icon. Click to select Weighing Boat.	Click on Select tools icon. Click to select Scale and Weighing Boat.
Right-click on the Weighing Boat >> Duplicate option.	For this demonstration we require 4 copies of Weighing Boats. Right-click on the Weighing Boat. Select Duplicate option from the context menu. A new Weighing Boat appears. Similarly obtain other Weighing Boats. Rearrange the Weighing Boats on the workbench.
Right-click on Weighing Boat >> Rename option. Click on Ok. Rename the Weighing Boats as 1, 2, 3 and 4.	Let us assign names to each one of them. Right-click on the Weighing Boat. Select Rename option from the context menu. Rename the Weighing Boats as 1, 2, 3 and 4.
From the Stockroom Explorer, Double-click on 100 mL Distilled HspO flask. Right-click on the flask, use Duplicate option.	From the Stockroom Explorer, double-click on 100 mL Distilled water flask. 100 mL Distilled water flask appears on the workbench. Right-click on the flask. Use Duplicate option to make 4 copies. Rearrange 100 mL Distilled water flasks on the workbench.
Right-click on the flask, select Rename option from the context menu. Rename the flasks as 1, 2, 3 and 4.	Right-click on the flask, select Rename option from the context menu. Rename the flasks as 1, 2, 3 and 4.
Drag the Scale. Drag and place the boat on the scale. Press TARE.	Bring the Scale to a convenient position on the workbench. Place Weighing Boat 1 on the scale. Click TARE.
Type 5 in the Transfer amount input bar. Click on Pour.	Weigh 5 grams of Silver Chloride. Bring the Silver Chloride bottle near to the Weighing Boat 1. In the Transfer amount input bar , type 5. Click on Pour.
Drag the Silver Chloride bottle aside. Bring the Weighing Boat 1 to flask 1. Type 5 in the Transfer input bar. Click on Pour. Drag and place the Weighing Boat aside.	Keep the Silver Chloride bottle aside. Now let us transfer Silver Chloride to flask 1. Bring Weighing Boat 1 to flask 1. Type 5 in the Transfer amount input bar. Click on Pour. Keep Weighing Boat aside.
Click on Flask 1. Cursor on Solution Info Panel.	Click on Flask 1. Observe the Solution Info Panel.
Cursor on Aqueous radio button. Click on the black arrow, next to molarity. Point towards concentrations of Silver ion and Chloride ion.	By default Aqueous radio button is selected. Concentrations of all the ionic species present in the solution are given here. Click on the small black arrow, next to Molarity. Here we can express concentrations in grams, moles and Molarity. Note the concentrations of Silver ion and Chloride ion in terms of Molarity.
Show all the steps for Strontium Sulphate Silver Carbonate, and Strontium Iodate	Similarly, using weighing boat, weigh 5 gm each of, Silver Carbonate Strontium Sulphate, and Strontium Iodate Pour into flasks 2, 3 and 4 respectively.
Click on flasks 2, 3 and 4. Wait till equilibrium is reached.	Click on each flask. Wait till equilibrium is reached. Note the concentrations of ions at equilibrium. This value is the Solubility of that ion in its saturated solution.
Slide Number 11 Calculation Table	Note solubility values for each ion in table as shown here.
Slide Number 11 Calculation Table (with Ksp values)	Calculate Solubility product for each salt. Note in the table.
Cursor on slide number 10	Solubility products values for Strontium salts are more when compared to silver salts. This is because Strontium salts are more soluble in water when compared to silver salts.
Slide Number 12 Standard Values of Solubility Product	The experimental values of Solubility Product are comparable with known values.
Slide Number 13 Summary	Let us summarize. In this tutorial we have, Determined solubility of salts. Calculated Solubility Product of various sparingly soluble salts.
Slide Number 14 Assignment	As an assignment, For Strontium Sulphate and Strontium Iodate: Write dissociation equation and Solubility Product expression. Find Solubility Product of these salts at 35° C. Observe whether dissolution of these salts is exothermic or endothermic.
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Slide Number 18: Acknowledgement	Spoken Tutorial Project is funded by NMEICT, MHRD, Government of India. More information on this mission is available at this link.
	This tutorial is contributed by Snehalatha Kaliappan and Madhuri Ganapathi from IIT-Bombay. Thank you for joining.

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Snehalathak