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Determining the solubility of calcium hydroxide via titration
 
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Behold as I blow your minds with my awesome calculations!
Views: 15125 MrMrPhysics
Ksp Ca(OH)2 with Common Ion Effect Lab
 
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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 Ksp of Calcium Hydroxide AP Lab with vernier
 
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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: 948 muhittin kelesli
Calculating Ksp From Molar Solubility - Solubility Equilibrium Problems - Chemistry
 
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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/
What is Ksp? (Solubility Product Constant)
 
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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: 270769 chemistNATE
ksp of calcium hydroxide
 
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This video is about ksp of calcium hydroxide
Views: 35 Brittani Young
Analyzing Data from the Vernier Ksp of Calcium Hydroxide lab
 
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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: 623 William Cunningham
Stoichiometry Problem, Precipitation of Calcium Hydroxide
 
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New Visions Charter High School for the Humanities
Views: 130 Logan Cawley
WCLN - Ksp from Solubility Data - Chemistry
 
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Ksp from Solubility Data http://www.BCLearningNetwork.com. 0:00do dull 0:06in this video we'll show you how do you sell your ability data 0:09to determine the KSP for a given compound 0:13well illustrate a little experiment we start with an MP evaporating dish 0:17now we put the anti dapper in dish 0:21on electronic ballots and the balance read 70 8.5 22 grams 0:27so we record that here in the data table 0:30for the massive the empty evaporating dish replace the anti evaporating dish 0:36and a hot plate that hasn't been turned on yet 0:39now we carefully measured fifty milliliters 0:42and saturated be af2 solution and at it today that green dish 0:47me make sure this sample has no I'm dissolve solid in it 0:51and we record this as fifty milliliters 0:55a volume here in the data table now we turn the hot plate on 1:00a low setting and let it warm up and the water slowly evaporate 1:08leaving a small amount of solid residue in need operating dish 1:12we turn the hot plate of 1:15and let the dish cool down after its cool 1:20replace the evaporating dish with the solid residue back on the electronic 1:25balance 1:25and the reading is seventy 8.5 53 grams 1:30this is the total mass the evaporating dish and a solid be a apt to you that 1:35was originally dissolved in the 50 milliliter sample 1:38the saturated solution so 1:41we record that appear in the data table were asked to use the given data 1:47to determine the KSP 3b af2 1:50at the temperature the original saturated solution 1:53we can do this in two major steps first 1:56we used a given data to determine the molar solubility 2:00a BF two once we have the molar solubility 2:04then we can use it to determine the dalai a PSP 2:08for barium chloride we start by calculating the mass 2:12up solid be af2 in the that green dish 2:15this is the message be af2 that was dissolved in the 50 no sample 2:20have the original saturated solution to do this we take the mass 2:25the that bringing dish and solid be af2 2:28and subtract the mass at the Mt apprehended 2:32and we get .0 31 grams 2:35have solid be a FT so will add a line to our data table 2:40and record this value their now we have enough information to calculate the 2:45molar solubility 2:46be af2 we start out with the gramm to be a f2 2:51then we convert to moles IBAF to 2:54next we divide the moles by the volume 2:57have our sample in leaders in order to get 3:00the molar concentration or molarity the saturated solution 3:04which is the molar solubility so to calculate the molar solubility 3:10we start with the massive be af2 which is .0 31 grams 3:16and we multiply it by the conversion factor one mall IBAF to 3:21270 5.3 Graham to be a f2 3:24it's more mass if we stopped here 3:27we would be able to calculate the malls however we use another conversion factor 3:33to go to the molar concentration in order to find a molar concentration 3:38normal air D 3:39we divide the malls by the leaders of solution up in the data table we see 3:45that the volume of the solution is fifty milliliters 3:48to change fifty milliliters two leaders we divide by eight thousand so fifty 3:53milliliters is equal 2.05 meters 3:56dividing by years is the same as multiplying 4:01by one overeaters so we multiplied by the conversion factor 4:06one over point zero five leaders we can cancel the unit Graham to be a f2 4:14never left with malls to be a f2 4:17over leaders in the af2 which is the same as molarity 4:21unit we need for concentration 4:24defined in value from a lower concentration we take .0 31 4:29divided by one 75.3 invited by .0 4:335 and we get 3.54 4:37times tend to the -3 moles per liter 4:40or we can say the molar solubility 4:43his 3.54 times 10 the native third molar 4:47notes that this answer has three significant figures 4:51one more than a two significant figures in the massive solid be af2 4:57however since the molar solubility is only the first step in this problem 5:02will lead it to one extra significant figure and round 5:05two significant figures at the very end to the problem 5:09so we can summarize up here the molar solubility
Views: 1770 W CLN
Ksp Determination
 
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Lab 11: Ksp Determination Pd 2 Hi Ms. Paik!!!
Views: 2649 Vivian Zhou
Mg(OH)2 molar solubility Ksp
 
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I created this video with the YouTube Video Editor (http://www.youtube.com/editor)
Views: 1771 Kayla Pyper
Titration of HCl and Ca(OH)2
 
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**Moles of HCl should be round to 0.00857 mol Video assignment for Chem 1201 - John Hopkins
Views: 3555 Nicole Ravey
Equation for Calcium Hydroxide Dissolving in Water   | Ca(OH)2 + H2O
 
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In this video we will describe the equation Ca(OH)2 + H2O and write what happens when Ca(OH)2 is dissolved in water. Note: Calcium hydroxide is not very soluble in water (15 mg/L at 25°C). So only a small amount would dissolve. When Ca(OH)2 is dissolved in H2O (water) it will dissociate (dissolve) into Ca +2 and Cl- ions. To show that they are dissolved in water we can write (aq) after each. The (aq) shows that they are aqueous – dissolved in water. The equation for Ca(OH)2 (Calcium hydroxide) and H2O sometimes isn’t considered a chemical reaction since it is easy to change the Ca 2+ and OH- back to Ca(OH)2 (just let the H2O evaporate). At the same time, the Ca(OH)2 is a very different substance than Ca 2+ and OH-. If you need to know how to balance chemical reactions, see my complete tutorial on balancing all types of chemical equations: Balancing Equations in 5 Easy Steps: https://youtu.be/zmdxMlb88Fs More Practice Balancing: https://youtu.be/Qci7hiBy7EQ Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).
Views: 1870 Wayne Breslyn
Calculate Molar Solubility of Ca(OH)2 From Ksp 002
 
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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
Soluble and Insoluble Compounds Chart - Solubility Rules Table - List of Salts & Substances
 
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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
How to do back titrations - also known as indirect titrations.
 
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I use a writing frame to take you through three separate back titrations, teaching you the 5 basic steps that are generally involved. The first determines the percentage purity of a sample of Magnesium Oxide.The second determines the percenatge of Calcium Carbonate in chalk. The third finds the concentration of Ammonia in a domestic cleaner. Note that the result of a back titration will be inaccurate if chemical A is contaminated with a chemical that would also react with chemical B.
Views: 49169 FranklyChemistry
Calcium hydroxide titrated in hydrochloric acid
 
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This is my video submission for hopkins
Views: 307 Kevin Nguyen
AP Ksp and pH Calculations
 
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Calculating Ksp from pH values and calculating pH from Ksp values.
Views: 12491 Victor Senn
ksp equilibrium
 
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1) Compound Formula Ksp Silver bromide AgBr 5.35×10−13 Iron(II) hydroxide Fe(OH)2 4.87×10−17 Calcium fluoride CaF2 1.46×10−10 Use the Ksp value in the table to calculate the molar solubility of AgBr in pure water. Use the Ksp value in the table to calculate the molar solubility of CaF2 in pure water. 2)Use the given molar solubilities in pure water to calculate Ksp for each compound: PbF2; molar solubility = 5.63×10−3M
Views: 463 Alek Chongris
Precipitation Reactions: Crash Course Chemistry #9
 
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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: 1302553 CrashCourse
pH Saturated CaOH2
 
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Part of NCSSM CORE collection: This video shows the reading the pH of saturated solution of calcium hydroxide. 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/GAfz/
How to make Calcium Hydroxide (Ca(OH)2)
 
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Note: It is much cheaper to just buy CaOH2. This video is more for informational purposes if you don't want to buy it. It is extremely cheap stuff to buy. In this video we will make calcium hydroxide. I am producing this to use in a future video on how to make potassium chlorate from calcium hydroxide and chlorine gas.
Views: 92850 NileRed
Calcium-EDTA titration
 
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This video demonstrates the titration of calcium with an EDTA titrant. The indicator used is another chelating agent, Eriochrome Black T. The color transition can be very difficult to see due to the very gradual change in color of the indicator over the course of the titration.
Views: 171722 crharrison
WCLN - Altering Solubility Review - Chemistry
 
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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: 1145 W CLN
How To Find Concentration Of A Base (OH-) When Given pH
 
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How to find the concentration of a hydroxide when given the pH How to find a concentration of base Includes concentration formula, and how to find a pH with a pOH Ca(OH)2, calcium hydroxide Polyatomics with subscripts Chemistry and Math
Views: 1152 Academic Aesthetic
making calcium cyanamide
 
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Making calcium cyanamide via pyrolysis of calcium cyanurate at high temperature. firstly we made calcium cyanurate using pool stabilizer cyanuric acid in a large solution nad added sodium hydroxide to form sodium cyanurate and finally used a slight excess of calcium chloride to form the targeted product with sodium chloride as a side product. the calcium cyanurate is somewhat soluble in hot water but further precipitates on cooling. We washed and decanted several times to remove all traces of alkali metal contamination- This step MUST be done otherwise dangerous sodium cyanide may form during the heating which will be bad news when the cyanamide is used later in an acidic solution to make Aminoguanidine bicarbonate in a later preparation. The identity test was nitric acid/cyanamide in a solution with a second solution added of ammoniacal silver nitrate to precipitate a very vibrant yellow salt of silver cyanamide. This test can also be used to determine the purity of the product however i ran out of nitric acid. the theoretical yield vs actual yield are calculated to determine % and a nitrogen percentage Music credit goes to bensound.com royalty free music.
Views: 2542 AllChemystery
Quicklime and Water Exothermic Reaction
 
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We will measure the heat produced when quicklime (calcium oxide) reacts with water. The reaction is exothermic, because it releases heat.
Views: 48383 mopatin
Ca(OH)2 + HBr - Calcium Hydroxide and Hydrobromic Acid: Balanced Chemical Equation
 
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This video shows you how to write a balanced chemical equation for the reaction between calcium hydroxide Ca(OH)2 and hydrobromic acid (HBr). It also includes the total ionic and the net ionic equation as well.
Views: 5777 Math & Science 2024
Chemistry Experiment How To Make Calcium Carbonate Full HD video
 
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In this experiment I will show you how to make Calcium Carbonate. This compound is present in many rocks because they are remains of prehistoric sea living animals with shells, living hundred millions years ago. But it's available for free in quite pure form in the thing that we normally throw away to trashcan. Eggshells. It has mass approximately 5-6 grams. Therefor there is needed approximately 200 eggshells to receive 1 kg of Calcium Carbonate. My videos are often watched by people from India, Pakistan, and other 3rd world countries. You can make job from this process. Buy eggshells from people and convert them to Calcium Carbonate, Calcium Oxide, Calcium Hydroxide and sell ready product. First I will use coffee mixer like this one and mix shells. Press button and release multiple times until you have dust. Then use mortar and pestle to mash it up even more. Once you have dust place it in container and add water. Calcium Carbonate is slightly soluble in water. Whatever is insoluble and lighter than water will gather on the surface of water. Wait a day and throw it away. Repeat multiple times with more eggshells. At the bottom of tank there is our product. I have here product made couple days ago. Get rid of water and you have Calcium Carbonate. In future I will show how to make from it Calcium Oxide, Calcium Hydroxide and other Calcium compounds. Thank you for watching. ps. Use dry eggshells. Fresh one are a bit wet. Wait at least day or two prior mixing them in coffee mixer. ps2. You can convert it even more, by dissolving entire eggshells permanently in water (there is needed plentiful of water). Then heat water to vaporize it (use Sun to minimize cost). Remains will be looking nothing like original material.
Views: 20712 Przemysław Gruchała
Make Calcium Hydroxide
 
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In this video we explore one way of making calcium hydroxide using easy to find Sodium Hydroxide (NaOH) and Calcium Chloride (CaCl2). Sodium hydroxide can be sound as Lye or in many crystal drain openers. If using a drain opener first verify it is truly pure sodium hydroxide. Calcium Chloride is sold as DampRid, but can be found in many other moisture absorbing products as well. In this experiment solutions containing 60g Calcium Chloride and 40g Sodium Hydroxide are reacted to precipitate Calcium Hydroxide Ca(OH)2 This will eventually be used to attempt isolating Calcium metal for an element collection as well as other various experiments.
Views: 20285 ElementalMaker
The Reaction of Calcium Metal and Water
 
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The Reaction of Calcium Metal and Water: This highly exothermic reaction produces bubbles of hydrogen gas. A small amount of the calcium hydroxide product is dissolved in the aqueous solution, but the majority precipates due to its low solubility. Ca (s) + 2H2O (l) → Ca(OH)2 (aq, s) + H2 (g) Video created and uploaded by Tom's Photo Log http://www.tomsphotolog.com
Views: 897 Toms Photos
Titration (using phenolphthalein)
 
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*** For those who have not noticed the previous comments about the accuracy in the video: This video was made as a quick guide for one of my classes about what a titration is and it wasn't meant to be an exact representation since that would have taken longer and I wanted to get to the end point faster so they could see what happens. I explained to them that it would need to be done more accurately if they were ever to do one themselves. *** ---------- A titration experiment is used to calculate an unknown concentration of acid (or alkali) using a neutralisation reaction. In this titration an alkali (with a known concentration) is carefully added to the acid (of unknown concentration) using a burette. The volume of alkali used in the experiment is needed in order to perform a calculation to work out the concentration of the acid. The acid used in this titration is hydrochloric acid (HCl, 25ml volume, unknown concentration) and the alkali used is sodium hydroxide (NaOH, 0.1M concentration). ----- Useful equations to calculate the unknown concentration of acid: number of moles = concentration x volume concentration = number of moles ÷ volume Concentration is measured in moles per litre (moldm-3) Volume is measured in litres (decimetre cubed: dm3) ----- The equation for this reaction is: hydrochloric acid + sodium hydroxide ---- sodium chloride + water HCl + NaOH ---- NaCl + H2O (using subscript for the 2 in H2O)
Views: 1088098 Science Xperiments | sXp
What mass will Dissolve in 1 L of Water? (Use Ksp)
 
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How to Calculate how much PbI2 will dissolve in 1 L of water? I use PbI2 as an example....you can do this for any solid as long as you have its solubility product constant (Ksp)!
Views: 18230 chemistNATE
How to Balance HF + Ca(OH)2 = CaF2 + H2O (Hydrofluoric Acid plus Calcium Hydroxide)
 
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In this video we'll balance the equation HF + Ca(OH)2 = CaF2 + H2O and provide the correct coefficients for each compound. To balance HF + Ca(OH)2 = CaF2 + H2O you'll need to be sure to count all of atoms on each side of the chemical equation. Once you know how many of each type of atom you can only change the coefficients (the numbers in front of atoms or compounds) to balance the equation for Hydrofluoric Acid plus Calcium Hydroxide. Important tips for balancing chemical equations: Only change the numbers in front of compounds (the coefficients). Never change the numbers after atoms (the subscripts). The number of each atom on both sides of the equation must be the same for the equation to be balanced. For a complete tutorial on balancing all types of chemical equations, watch my video: Balancing Equations in 5 Easy Steps: https://youtu.be/zmdxMlb88Fs More Practice Balancing: https://youtu.be/Qci7hiBy7EQ Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).
Views: 494 Wayne Breslyn
CO2 + Ca(OH)2 Carbon dioxide and Calcium Hydroxide פחמן דו חמצני ומי סיד צלולים
 
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CO2 + Ca(OH)2 Carbon dioxide and Calcium Hydroxide פחמן דו חמצני ומי סיד צלולים צפייה בסמארטפונים והסבר מלא בקישור: http://goo.gl/GdpdN הסרט הוא חלק מסדרה של ניסויים אינטראקטיבים בנושא "חומצה בסיס", הסידרה כוללת את כל תגובות החומצה-בסיס הנלמדות במסגרת הבגרות בכימיה בתיכון בישראל -- ליחצו על ההערות המופיעות במהלך הסרט כדי לעבור בין הסרטים והניסויים המצולמים רעיון: ד"ר אבי סאייג - מכון דוידסון לחינוך מדעי, מכון ויצמן למדע פיתוח והפקה: ד"ר אבי סאייג, ד"ר מלכה יאיון, מרכז מורי הכימיה הארצי, המחלקה להוראת המדעים, מכון ויצמן למדע מציגים: ד"ר אבי סאייג, שלי רפּ - המחלקה להוראת המדעים, מכון ויצמן למדע צילום: שגיא בר און עריכה: צילה ביטרמן מוזיקה: Amazing Plan; Hustle. Kevin MacLeod - Creative Commons license, http://incompetech.com/m/c/royalty-free/
Solubility product Kₛₚ problem: AX₂
 
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00:07 Solubility of lead (II) iodide 01:24 Kₛₚ expression for PbI₂ 04:08 Let x = [Pb⁺² (aq)] 04:58 Let 2x = [I⁻ (aq)], charge balance 05:29 Substitute x and 2x into Kₛₚ expression 07:56 Solve for x 10:58 Molar solubility Calculation of the molar solubility of the sparsely soluble salt lead (II) iodide (PbI₂). Don't forget to like and subscribe!
Views: 115 lseinjr1
ChemCast 14.7 - Calculating Solubility from Ksp.mp4
 
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ChemCast 14.7 - Calculating Solubility from Ksp.mp4
Views: 25766 CarringtonChemCast
Dissolving Calcium Chloride: An Exothermic Process
 
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A demonstration of the exothermic nature of the dissolving process for calcium chloride. *Note - This and all demonstrations should only be performed by qualified personnel. Proper safety precautions should be observed at all times.*
Views: 61639 mreisley
Solubilities
 
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In which I describe the concept of solubility through the eyes of the chemist. All references can be found in any general chemistry text book. Calcium Hydroxide and Sodium Hydroxide Solubility (downloaded from): http://www.google.com/url?sa=t&source=web&cd=5&ved=0CEUQFjAE&url=http%3A%2F%2Fwww.lime.org%2Fdocuments%2Flime_basics%2Flime-physical-chemical.pdf&rct=j&q=Solubility%20sodium%20hydroxide%20100%20degrees&ei=4vx0TsCINoTmiAKFw5CzAg&usg=AFQjCNG1PJjRnAPl4YQkiNKTIfFSMWsOww&sig2=-vOGv5dcA_KJCs7fuXoBQg&cad=rja I also realize that I switched the scenes for rule 2 and rule 3. I apologize for that.
Views: 229 The Science Of Life
Primitive Technology: Wood Ash Cement
 
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Primitive Technology: Wood Ash Cement - Creating wood ash cement from scratch Subscribe: http://bit.ly/subPT | Never miss a video! Enable ‘ALL’ Notifications! More videos, watch me cultivate and cook yams from scratch: http://bit.ly/2L5HmqY Follow Primitive Technology: Wordpress: https://primitivetechnology.wordpress.com/ Patreon: https://patreon.com/user?u=2945881 Watch More Primitive Technology: Latest Uploads: https://youtube.com/playlist?list=PLGnWLXjIDnpBR4xqf3FO-xFFwE-ucq4Fj Pyrotechnology: https://youtube.com/playlist?list=PLGnWLXjIDnpBVRqu5lz5JGaQxjPs7q3CJ Shelter: https://youtube.com/playlist?list=PLGnWLXjIDnpBBsdKZb-vy30o88SIxItp2 Weapons: https://youtube.com/playlist?list=PLGnWLXjIDnpA-XGDrrmVgBnSXx15i2Awp Popular Videos: https://youtube.com/playlist?list=PLGnWLXjIDnpAb29Lrdki5BPjTpMon8zla Partial credit for this idea goes to James Keane who I discussed this with on my wordpress site (see conversation): https://primitivetechnology.wordpress.com/2018/03/06/lime/#comment-9736 I developed an experimental cement from made only from re-fired wood ash as its cementitious material. It was mixed with crushed terracotta as an aggregate and formed into a cube. The cement set hard after 3 days and did not dissolve in water after this period. Process: First I burnt bark and leaves in a kiln at high temperatures to produce well burnt, mostly white wood ash. The ash was then mixed into water and stirred well. The excess water was poured off and the resulting paste was made into pellets and allowed to dry. A pellet was then re-heated in the forge until it glowed about orange hot. This was then taken out, cooled and dropped in a pot of water. The pellet dissolved and boiled due to a chemical reaction with the water. The paste was stirred and crushed terracotta (old tiles from previous projects) was added and mixed to form a mouldable mortar. This was formed into a cube and allowed to set for three days (in the video, a cube made exactly the same way 3 days previously was used due to time constraints). The resultant cube was strong and made a slight ringing sound when tapped with a finger nail. It was placed in water for 24 hours to simulate a very heavy rain event and did not dissolve or release residues into the water. My current theory: The main component of wood ash consists of calcium in some form (e.g. calcium carbonate, calcium oxide). This can be up to 45% from my research. Calcium is in higher concentration in the bark and leaves of a tree. When the ash is mixed with water, the soluble component of wood ash (10% pot ash) dissolves into the water. But seeing that it does nothing for the cementing process, it is drained off leaving the insoluble calcium (and other components) in the paste. Doing this probably raises the relative percentage of calcium in the paste to about 50% or more. Most of the other 50 % consists of silica and alumina which are pozzolans, materials that chemically react with calcium hydroxide to increase the durability of the cement product. The paste was then made into a pellet and fired again to high temperature to convert all the calcium compounds to calcium oxide. It also reduces any charcoal in the pellet to ash if it hadn’t already been burnt the first time. This step seemed important as un-fired ash pellets only partially hardened and would fall apart in water, though retaining a weak undissolved 5mm thick crust. I can only surmise that re-firing the ash just gave a greater conversion of the calcium components to calcium oxide. The pellet is slaked in water converting the calcium oxide to calcium hydroxide. This cement was mixed with crushed terracotta which may also help in some way that I’m not aware of as I only did this one experiment and did not test other aggregates yet (e.g. sand, gravel etc.). Terracotta is porous and might hold together better than other materials. The mixture is allowed to set in air where carbon dioxide reacts with calcium hydroxide to form calcium carbonate cementing the aggregate together. After this, the cement will not dissolve in water. Use: I think this material might have a potential use as a mortar holding rocks or bricks together in wet environments where limestone or snail shells are unavailable for making cement. Wood ash is a pretty ubiquitous material to most natural environments inhabited by people using biomass fuels. Wood ash cement turns a waste product into a valuable building material. From my research, wood ash is already being used as a partial replacement for cement in the building industry without decreases in strength of the final product. But I’ve only just started experimenting with it and don’t know its full capabilities and limitations. Calcium content of wood ash differs depending on the species of tree, the part of the tree burnt and the soil it’s grown on. Cautious experimentation is still required before committing to a hut built from this material.
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Calculate Molar Solubility of Ba(IO3)2 From Ksp 003
 
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The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What is the molar solubility (mol/L) of Ba(IO3)2?

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