Search results “Determining solubility product constant calcium hydroxide solubility”
Ksp Ca(OH)2 with Common Ion Effect Lab
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/
Determining the solubility of calcium hydroxide via titration
Behold as I blow your minds with my awesome calculations!
Views: 13931 MrMrPhysics
CHEM 1520L Experiment 007 A Solubility Product Constant
CHEM 1520L Experiment 007 (1) Standardization of Sodium Thiosulfate Through Titration with Iodate (2) Determining solubility "s" and Ksp of Calcium Iodate
Views: 1374 vijay antharam
Calculating Ksp From Molar Solubility - Solubility Equilibrium Problems - Chemistry
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/
Determining the Ksp of Calcium Hydroxide AP Lab with vernier
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: 830 muhittin kelesli
What is Ksp? (Solubility Product Constant)
Ksp is really just an equilibrium constant (Keq), but it's for a solid dissolving in water. This is special, since all of the reactants are solid, and so they AREN'T included in the equilibrium expression.
Views: 259807 chemistNATE
Calculating the Solubility Product Constant of KHTartrate
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: 400 William Cunningham
Ksp Determination
Lab 11: Ksp Determination Pd 2 Hi Ms. Paik!!!
Views: 2506 Vivian Zhou
Titration and solubility with Ca(OH)2 (how not to do it)
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: 984 Kilian Demmel
Solubility Products
Views: 15 Massimo Bozzi
Mg(OH)2 molar solubility Ksp
I created this video with the YouTube Video Editor (http://www.youtube.com/editor)
Views: 1490 Kayla Pyper
A2 Chem:Solubility Product
This video is about Ksp calculations
Views: 871 Bilal Hameed
WCLN - Determination of solubility product constant - Chemistry
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: 4977 W CLN
Determining the Ksp of Calcium Hydroxide
Determining the Ksp of Calcium Hydroxide
Views: 31 Kristin Smart
Lab 4 Solubility Product Constants
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: 2860 ProfessorAbud
Analyzing Data from the Vernier Ksp of Calcium Hydroxide lab
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: 565 William Cunningham
Soluble and Insoluble Compounds Chart - Solubility Rules Table - List of Salts & Substances
This chemistry video tutorial focuses the difference between soluble and insoluble compounds. It contains a table or chart of the solubility rules and it provides a list of salts and substances - some of which are soluble while others are insoluble. This video contains a worksheet of examples and problems toward the end of the video including answers and solutions. Here is a list of topics: 1. Understanding The Solubility Rules Table 2. Ions that are always soluble - Na+, K+, Li+, NH4+, C2H3O2-, Cs+, Rb+, ClO4-, ClO3-, and HCO3- 3. Ions that are generally soluble - Cl-, Br-, I- (halides) - Exceptions - Pb2+, Ag+, Hg2 2+ 4. Sulfates are generally soluble except with Ba2+, Ca+2, and Sr2+ 5. The difference between soluble and insoluble compounds - aqueous vs solid phases 6. Substances that are generally insoluble - Hydroxides, carbonates, sulfides, and phosphates
Explains how to calculate the Ksp for a slightly soluble ionic compound.
Views: 3554 storm808b
Determination of Ksp in Calcium Hydroxide
Jesse Fox Class
Views: 65 Shivam Bembalkar
Calculate Molar Solubility of Ca(OH)2 From Ksp 002
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
Precipitation Reactions: Crash Course Chemistry #9
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: 1259972 CrashCourse
ksp of calcium hydroxide
This video is about ksp of calcium hydroxide
Views: 31 Brittani Young
WCLN - Altering Solubility Review - Chemistry
Altering Solubility Review Question http://www.BCLearningNetwork.com. 0:00that here's a question that will help you review how the solubility 0:06the compound can be altered rest to consider a saturated solution a 0:10calcium hydroxide a and were given its solubility equilibrium equation here 0:15various things are added to the saturated calcium hydroxide solution 0:19and rest to fill in the table to show what would happen pause the video now 0:23and try to fill this on your own first 0:26and then resumed video we'll start with Kayleigh 0:30which is an alkali metal compound so it dissociates completely and decay plus 0:35no age minus science que pases a spectator I N 0:38so we omit sweating Kooh will initially increase the concentration 0:44avoid minus so we can write this in here is no initial change in the 0:48concentration ca2+ plus 0:50increasing the concentration avoid minus will cause the equilibrium 0:55to shift to the left which would produce more solid and decrease the solubility 1:00it calcium hydroxide 1:01next we'll look at a quiz sodium oxalate 1:05sodium oxalate and alkali metal compound 1:08dissociates completely into sodium and oxalate I N 1:12sodium ions are spectators so we can discard them the oxalate INC to you all 1:17for two-minus 1:18is a negative by in so we can see if it forms a precipitate 1:22with positive calcium ions mechanic ASP table 1:27we see that calcium oxalate has a low key sp 1:30this means the Oxley I and does former precipitate 1:33with the ca2+ besides this would initially 1:37decrease the concentration of ca2+ plus there's no initial change in the 1:42hydroxide ion concentration 1:44decreasing the concentration of ca2+ plus 1:47will cause the equilibrium to shift to the right a shift to the right 1:52will increase the solubility have calcium hydroxide 1:55next we'll look at a quiz calcium I had a 1:59go see my dad is soluble & Associates the calcium 2:02and I and II this would cause an initial increase in the concentration of calcium 2:08mines 2:08so right that increase here there's no initial change in the concentration 2:14hydroxide nine's an initial increase in the concentration accounts in mind 2:19would cause the equilibrium to ship to the left which would cause a solubility 2:24accounts in hydroxide to decrease 2:26remember this is called the common ion effect the low solubility compound CaOH 2:322 2:33and the added salt CA I to have the cows into plus I am in common 2:39next we'll consider adding he or increasing the temperature 2:43adding heat will have no initial effect on the concentration of calcium lines 2:48or on the concentration of hydroxide ions 2:51because the heater is on the left side of the equation adding he 2:55will cause the equilibrium to shift to the right a shift to the right 3:00will cause the solubility of calcium hydroxide 3:03to increase next we'll consider the addition a bakery s make an easy in a 3:08tree 3:08make on a tree compounds magnesium a tree is soluble 3:13so it dissociates into magnesium in a trade in's 3:16nitrate ions are spectators so we can discard them 3:20now we have to check and see if the positive magnesium ions 3:24form a precipitate with negative hydroxide ions that are in the solution 3:28looking on the KSP table we see that magnesium hydroxide 3:33has a low key sp so this means magnesium I N 3:37do former precipitate with hydroxide magnesium ions 3:41will react with some other hydroxide ions and cause their concentration to 3:45decrease 3:46adding magnesium nitrate would have no initial effect on the concentration 3:51Kelsey mines decreasing the hydroxide ion concentration 3:56will cause the equilibrium to ship to the right shift to the right 4:00will increase the solubility calcium hydroxide 4:04next we'll consider the addition a bakery s hno3 4:08which is called nitric acid nature cassidy hno3 4:12has a strong acid so it completely ionized 4:15Cindy age plus in a trade nitrate and your spectators so we can discard them 4:21nitric acid supplies age by science 4:24and it is known that age by science react at all wage minus science 4:29department water 4:30as shown by the net ionic equation inside the yellow arrow 4:35the reaction a page plus with oooh minus is called neutralization 4:39age prices in acid no age minus is a base 4:43this will use up hydroxide ions 4:46and make their concentration decrease there will be no initial change in the 4:51concentration accounts in mind 4:53a game decreasing the concentration of hydroxide ions 4:57because this equilibrium to ship to the right 5:00which will cause the solubility of calcium hydroxide
Views: 1067 W CLN
Calculate Molar Solubility In Solution of Common Ion From Ksp 001
Calculate the molar solubility of Ca(OH)2 in 0.10 M Ca(NO3)2. The Ksp of Ca(OH)2 = 6.5 x 10-6.
Ksp precipitate lab
We are doing a serial dilution of Calcium and hydroxide ions do see when the solution stops preciptating. Then we'll calculate a range for ksp
Views: 1161 Kim Kaufman
writing Ksp expression
Views: 1384 Bhavna Rawal
Thermodynamics of Borax Dissolution | Intro & Theory
Experiment 21 in CHEM 1212K is titled "Thermodynamics of Borax Dissolution." The purpose of the experiment is to use titration of a saturated solution of the borate anion to determine the solubility products of sodium borate (borax) in water at three different temperatures. From these Ksp's, thermodynamic parameters can be determined.
Views: 2518 Michael Evans
Titration of HCl and Ca(OH)2
**Moles of HCl should be round to 0.00857 mol Video assignment for Chem 1201 - John Hopkins
Views: 2827 Nicole Ravey
Ksp Determination Lab
Views: 1556 Flak153
Lab 12 Ksp Determination
Lab 12 Paik 7, 8 Members: Kevin Zhao, Shantanu Jha, Nick Ng 6.11.17
Views: 34 Kevin Zhao
AP Chemistry Ksp Lab
Ksp Lab performed by Kevin, Chrissy, & The Junior.
Views: 193 Ksp Lab
WCLN - Increasing solubility - Chemistry
Solubility equilibrium equations will show how the solubility of a compound can be increased. http://www.BCLearningNetwork.com. 0:03here we'll look at how we can increase the solubility of a compound 0:06we'll start with a saturated solution the low solubility compound 0:11calcium carbonate here's the solubility equilibrium equation for it 0:16if we could somehow make this equilibrium shift to the right 0:20then some other CACO 3 percent but a 0:23would dissolve which means the solubility of calcium carbonate 0:28would increase question now is how do we make this shift to the right 0:33the shit ellios principal tells us that we can make the equilibrium chip tray 0:38by decreasing the concentration at the due to calcium 0:42or the carbonate I N the question is how do we decrease the concentration 0:47the Zions in cantwell 0:50we all learned two ways that decrease in the concentration of the dissolved I N 0:54one is to add a reagent which will form a new purse epic eight with the in- 0:59and the second method is if the in- is a babys 1:03make hydroxide or carbonate I N then we can at an acid to neutralize it 1:09let's say we want to decrease the concentration of calcium ions 1:14by adding something to precipitate them to find out what we can add 1:18we look at the solubility table or the KSP table 1:22in this section calcium ions are included in the low solubility category 1:27so for example the compound calcium phosphate 1:31will have low solubility so in other words 1:34phosphate ions will form a precipitate with Kelsey minds 1:38a soluble compound a phosphate 1:41is sodium phosphate so we obtain a pipe at 1:44with sodium phosphate solution in it sodium mines are spectators 1:49so we will include them here we had some %uh this solution to the beaker 1:54by doing this we are adding phosphate ions to the beaker 1:57these phosphate ions 2:01move toward somebody free calcium ions and calcium and phosphate mines 2:08become attached to each other forming the precipitate 2:12calcium phosphate the net ionic equation 2:16for this precipitation reaction is three see a two-plus 2:20bus to PO 43 miners form solid calcium phosphate 2:25c8 repeal 40 this reaction has consumed 2:30somebody free calcium mines that were in the solution 2:33so now there are less free calcium to class signs 2:37in the solution so we can say that the concentration 2:41see a two-plus has decreased we'll start with the original saturated calcium 2:47carbonate solution 2:48will include graphs showing how the mass of solid calcium carbonate 2:53and the concentrations at the ions in solution change 2:57we'll start by looking what happens before we add anything 3:02to the regional solution we can see that the massive solid and the concentrations 3:09at the in's 3:10have not changed yet at this point 3:13will add sodium phosphate to the beaker precipitates medi-cal sea mines 3:18and we can see that the concentration of ca2+ plus 3:22quickly decreases in order to counteract the low concentration and Kelsey mines 3:28disequilibrium which shift to the right make this 3:39noticed that during his shift the massive solid calcium carbonate 3:43decreased 3:44well the concentrations up the dissolved diane's 3:47increased after this year a new equilibrium has been established 3:52and the massive the solid and the concentrations at the ions remain 3:56constant 3:57we see that from the very beginning to the very end of the process 4:02there was a net decrease in the mass up the solid calcium carbonate 4:06because the massive the solid went down 4:09it means more a bit bizarre so we can save that the solubility of calcium 4:14carbonate 4:14was increased 4:17looking at the graph under the ca2+ plus I N 4:19we see that from the very beginning to the very end there was a small net 4:24decrease in the concentration of ca2+ plus 4:27whenever we decrease the concentration oven i and unique living next year 4:32the equilibrium a shift and only partially increase it 4:36so there will still be a small net decrease we see that there was a net 4:40increase in the concentration of carbon E 4:43nine's now will go back to the original solubility equilibrium 4:48this time will decrease the concentration at the carbonate I N 4:52acids all contribute age plus signs 4:56when they're added to a solution when an acid our age plus 4:59is added to the carbonate I N it is known that 5:03forms liquid water and carbon dioxide gas 5:07because carbon dioxide is a gas it bubbles out at the solution
Views: 2779 W CLN
Solubility product (Ksp) and molar solubility (10)
Chemistry: Dissolution and precipitation reactions. Solubility product (Ksp) and ion product (Q). Application of ICE tables to dissolution reactions. Molar solubility. How to find the solubility from the Ksp; how to find the Ksp from the solubility. Common ion effect This is a recording of a tutoring session, posted with the student's permission. These videos are offered on a "pay-what-you-like" basis. You can pay for the use of the videos at my website: http://www.freelance-teacher.com/videos.htm For a printable handout covering the material discussed in this video series, go to my website. For a list of all the available video series, arranged in suggested viewing order, go to my website. For a playlist containing all the videos in this series, click here: http://www.youtube.com/watch?v=fhFSu_Ssp54&feature=PlayList&p=1BB04DB5FECD1701&index=0&playnext=1 (1) Dissolution and precipitation reactions. Aqueous ("aq") phase (2) "Completely soluble" vs. "slightly soluble" salts. Solubility product (Ksp) and ion product (Q) (3) Continued (4) Application of ICE tables to dissolution reactions (5) Continued (6) Solubility (7) General method for solving solubility problems. An example in which we are given the solubility and have to find the Ksp (8) Continued (9) An example in which we are given the Ksp and have to find the molar solubility (10) Continued (11) Common ion effect. An example (12) Continued (13) Continued tags: education college student students university exam test educational study campus school class
Views: 4943 freelanceteach
Ksp of Mg(OH)2 and Ca(OH)2 Lab
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/