Part of NCSSM CORE collection: This video shows the collection of data to determine the K sp of Ca(OH)2 in water and a solution of CaCl2. http://www.dlt.ncssm.edu Please attribute this work as being created by the North Carolina School of Science and Mathematics. This work is licensed under Creative Commons CC-BY http://creativecommons.org/licenses/by/3.0 Help us caption & translate this video! http://amara.org/v/GAfu/
Views: 25946 North Carolina School of Science and Mathematics
Behold as I blow your minds with my awesome calculations!
Views: 17662 MrMrPhysics
Determining the Ksp of Calcium Hydroxide Calcium hydroxide is an ionic solid that is sparingly soluble in water. A saturated, aqueous, solution of Ca(OH)2 is represented in equation form as shown below. Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) The solubility product expression describes, in mathematical terms, the equilibrium that is established between the solid substance and its dissolved ions in an aqueous system. The equilibrium expression for calcium hydroxide is shown below. Ksp = [Ca2+][OH–]2 The constant that illustrates a substance’s solubility in water is called the Ksp. All compounds, even the highly soluble sodium chloride, have a Ksp. However, the Ksp of a compound is commonly considered only in cases where the compound is very slightly soluble and the amount of dissolved ions is not simple to measure.
Views: 1152 muhittin kelesli
This general chemistry video tutorial focuses on Ksp – the solubility product constant. It has plenty of examples and practice problems for you to work on to pass your next chemistry exam / test. Here is a list of topics: 1. How to Calculate Molar Solubility Using Ksp for AgCl and and Ca3(PO4)2 2. How to Convert Molar Solubility from M or mol/L to g/L 3. How to determine the concentration of the ions [Ag+], [Cl-], [Ca2+], [PO4 -3] 4. How To Find Ksp given molar solubility in moles per liter and grams per liter using PbCl2 and CuCl 5. Common Ion Effect – Calculating Molar solubility of CaF2 given Molarity of CaCl2 in a saturated solution 6. Calculating Molar Solubility of Al(OH)3 using Ksp and the pH of the solution 7. pH, pOH, [H+] and [OH-] equations and formulas 8. Le chatelier’s Principle – Chemical Equilibrium & Ksp – Reactant and Production Concentration 9. The effect of adding a common ion on solubility, dissolution, and precipitation 10. The effect of temperature on Ksp – Which way does the reaction shift? 11. The effect of adding CaCl2 to CaF2 on the pH of the solution 12. Solving for Ksp and Molar Solubility Using Ice Tables 13. How To Write The Equation or Equilibrium Expression For Ksp
Views: 188112 The Organic Chemistry Tutor
CHEM 1520L Experiment 007 (1) Standardization of Sodium Thiosulfate Through Titration with Iodate (2) Determining solubility "s" and Ksp of Calcium Iodate
Views: 2938 vijay antharam
We look at the method for determining the solubility product constant of a sparingly soluble salt, potassium acid tartrate, and how to collect lab data. (Recorded with https://screencast-o-matic.com)
Views: 1310 William Cunningham
This chemistry video tutorial explains how to calculate ksp from molar solubility. Ksp is known as the solubility product constant. This video contains plenty of examples and solubility equilibrium practice problems. It contains examples of calculating ksp from solubility in g/L and mol/L as well as from the concentration of one of the product ions. New Chemistry Video Playlist: https://www.youtube.com/watch?v=bka20Q9TN6M&t=25s&list=PL0o_zxa4K1BWziAvOKdqsMFSB_MyyLAqS&index=1 Access to Premium Videos: https://www.patreon.com/MathScienceTutor Facebook: https://www.facebook.com/MathScienceTutoring/
Views: 64253 The Organic Chemistry Tutor
Lab for determining the solubility product constant. http://www.BCLearningNetwork.com. 0:01determination of the solubility product 0:05constant in today's experiment we're 0:10going to be dealing with the production 0:13of a solid 0:15LED I'd we will remember that the 0:21solubility product constant or KSP is 0:24determined by taking the concentrations 0:28and in our case of PB 2 plus x the 0:34concentration of i minus remember that 0:39in the balanced equation the coefficient 0:41of x minus is too 0:45therefore when in the solubility product 0:49constant equation or the KSP equation we 0:53have to square it so the KSP becomes PB 0:572 plus x minus a squared will begin by 1:04taking potassium iodide and lead nitrate 1:11remember the net equation here or after 1:15the i- and the let the p2 plus when we 1:22mix the two solutions we will determine 1:25if a solid is formed or not the solid 1:30remember we call a precipitate we will 1:33do that for six test tubes and each of 1:39the one determining if a precipitate 1:43this form or not 1:44by doing this we're going to find the 1:48approximate KSP of land Ida now if you 1:54look at your table solubilities you'll 1:57notice there is a KSP for landed I'd 2:00what we're going to do is we're going to 2:03experimentally find the KSP or the 2:08approximate KSP for LED I'd so we'll 2:12take the first to where we have 10 mils 2:15of potassium iodide and 10 mils of lead 2:19nitrate we mix the two 2:21Lucian's together 2:29notice we get a yellow color and it's 2:34very milky so he knows precipitate has 2:36formed sometimes it's difficult to see 2:39whether or not it precipitates form but 2:42generally you'll notice that goes milky 2:45color and if we stood around we see the 2:47precipitate forming on the side 2:49let's just put that aside so precipitate 2:54form and remember that i will at the end 2:57of the lab pulse the results in a table 3:01the next two solutions are diluted 3:16we also see a reaction we notice the 3:20yellow color and there's also a 3:23precipitate formed 3:28the third test tubes are further noted 3:35six mills potassium iodide six mills and 3:40let nitrate dilated 10 mils of water 3:43remember we are varying the 3:45concentrations to see whether 3:47precipitate performed in essence we're 3:49doing the trial ksb if you've done some 3:53reading the trial Casspi if its larger 3:58than the Caspian precipitate before if 4:03it's smaller than the KSP precipitate 4:06wolf form when we vary the 4:09concentrations what we'll do is we'll 4:12find out the approximate concentrations 4:16at which the KSP does and doesn't form 4:19and our KSP value for the letter I'd i 4:22will fall in between move on to the 4:31fourth set of test tubes their 4:35concentrations are for Mills of each 4:38solution dilated to 10 mils of water 4:50fix it 4:55give it a moment we notice a precipitate 4:58has also formed so far the first four 5:03mix solutions have borne precipitates
Views: 6773 W CLN
Calculate the molar solubility of Ca(OH)2 in water. The Ksp of Ca(OH)2 = 6.5 x 10-6. Interviews 1) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part I” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-1 2) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part II” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-2
Views: 7069 Professor Heath's Chemistry Channel
Lead (II) sulfate has a solubility in water at 25 °C of 4.25 x 10-3 g/100.mL. What is the molar solubility of lead (II) sulfate? What is the Ksp of lead (II) sulfate? Interviews 1) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part I” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-1 2) Revell, K. (November 16, 2016) “An Interview with Heath Giesbrecht, Part II” The Macmillan Community https://community.macmillan.com/groups/flipped-chemistry/blog/2016/11/17/an-interview-with-heath-giesbrecht-part-2
Views: 2060 Professor Heath's Chemistry Channel
It is found that 1.1 x 10-2 g of SrF2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility product for SrF2.
Views: 2286 Professor Heath's Chemistry Channel
Titration of three different Ca(OH)2 solutions in NaOH, CaCL2 and water. This is basically also a good example of how it should not be done, or as some dude put it in the comments: "This is terrible". Here is a list of solubility product constants: http://www4.ncsu.edu/~franzen/public_html/CH201/data/Solubility_Product_Constants.pdf
Views: 1376 Kilian Demmel
From the graphical data generated when titrating hydrochloric acid into saturated calcium hydroxide solution, you can find the concentration of the hydroxide and calcium ions and then the Ksp of the base.
Views: 741 William Cunningham
DETERMINING THE KSP OF CALCIUM HYDROXIDE PART ONE PROF FOX
Views: 3 Andrew Symons
Part of NCSSM CORE collection: This video shows the collection of pH data to determine the Ksp of Ca(OH)2 and Mg(OH)2. Please attribute this work as being created by the North Carolina School of Science and Mathematics. This work is licensed under Creative Commons CC-BY http://creativecommons.org/licenses/by/3.0 Help us caption & translate this video! http://amara.org/v/GAfv/
Views: 4001 North Carolina School of Science and Mathematics
Explains how to calculate the Ksp for a slightly soluble ionic compound.
Views: 3624 storm808b
Dr. David Partyka, owner of PhDave LLC (http://www.phdave.com and http://www.test-boost.com), describes how to calculate the aqueous solubility of aluminum hydroxide, an ionic compound that has very low aqueous solubility. Test Boost now has a blog and a poll designed to create a database of information intended to help students (freely accessible) make more informed educational decisions. Visit http://www.test-boost.com/helpers/poll.php Please visit my other current project - CSSBurner (http://www.cssburner.com) - a rapid CSS optimization tool.
Views: 1305 TestBoost
The extent to which a sparingly soluble salt dissolves in water is often given in terms of the salt's equilibrium solubility product constant, K sp . The aim of this experiment is to determine the value of K sp for the salt silver acetate, and to demonstrate the common ion effect on the solubility of the salt.
Views: 2968 ProfessorAbud
A lot of ionic compounds dissolve in water, dissociating into individual ions. But when two ions find each other that form an insoluble compound, they suddenly fall out of solution in what's called a precipitation reaction. In this episode of Crash Course Chemistry, we learn about precipitation, precipitates, anions, cations, and how to describe and discuss ionic reactions. Table of Contents Precipitate Reactions 0:34 Determining Precipitates 1:35 Writing Precipitate Reactions 6:31 Calculating Molar Mass Equation 8:52 Want to find Crash Course elsewhere on the internet? Facebook - http://www.facebook.com/YouTubeCrashCourse Twitter - http://www.twitter.com/TheCrashCourse Tumblr - http://thecrashcourse.tumblr.com Support CrashCourse on Subbable: http://subbable.com/crashcourse
Views: 1390976 CrashCourse
Erika Tan explains how to solve common ion effect problems. TRANSCRIPT: The common ion effect is when you have a solid, and then you put it into a solution that already has dissolved ions in it. And this is going to lower the solubility of that solid. The solid in our case is Ca(OH)2, and it dissolves into Ca2+ and 2 moles of OH- ions. And we’re also given the Ksp here. We have the question, what is the solubility of Ca(OH)2 in a .2 M OH- solution? The common ion in this case is OH-, because OH- is present in the solution and Ca(OH)2 also can dissolve into OH- ions. What we have to do to find the solubility is first write out the Ksp equilibrium expression in regards to this whole equation here. Since Ca(OH)2 is a solid, we don’t include it in the expression. But since Ca2+ and OH- are ions, you can find the concentration of them. So we write [Ca2+] and [OH-]^2. Don’t forget that coefficient. What we can do is set up an ice chart (I stands for initial, C stands for change, E stands for equilibrium). We’re going to have initial Ca2+, which is 0, but the initial OH- is .2. Now change is going to be +x and +2x, so at equilibrium we’re going to have x and .2+x. So we have 5.5 x 10^-6 = (x)(.2 + 2x)^2. And we can drop the 2x because our Ksp value is very small. Remember, when anything is less than 1 x 10^-3, we can just drop the x value here. So now we have 5.5 x 10^-6 = (x)(.2)^2, which gives us 1.375 x 10^-4. That’s a really small value. As you can see, our solubility is really small because we already had OH- in the solution.
Views: 555 Tangerine Education