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Crystal growing kit not dissolving completely - used correct amount of water; fear temperature of the water may have dropped how can I safely resolve this?

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Thomas Stromgren

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  • 166 Answers

This is usually caused by using a solution that isn't saturated. The cure is to dissolve more solute into the liquid. Stirring and applying heat can help to get solute into solution. Keep adding solute until you start to see some accumulate at the bottom of your container. Let it settle out of solution, then pour or siphon the solution off, being careful not to pick up undissolved solute. If you don't have any more solute to use, you can take some comfort in knowing that the solution will become more concentrated over time, as evaporation removes some of the solvent. You can speed this process by increasing the temperature where your crystals are growing or by increasing air circulation. Remember, your solution should be loosely covered with a cloth or paper to prevent contamination, not sealed. See this link for detailshttp://chemistry.about.com/cs/growingcrystals/a/aa012804.htm

Posted on Jan 28, 2016

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Anonymous

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SOURCE: Totallt tubular science, crystal growing kit

www.smithsonianstore.com/assets/product_files/pdf/12074_me


Try this site. I saw instructions for a crystal growing product they have that also has a packet of citrine powder. See if you have the same ingredients as this 'recipe' calls for. :)

Posted on Sep 02, 2008

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Anonymous

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SOURCE: Missing instruction manual for Crystal growing kit.

www.toyday.co.uk/shop/crystal-growing-kit-instructions/info_12.html - 33k -

try this url--it is pretty much similar to all the kits.

cindy

Posted on Feb 23, 2009

Anonymous

  • 1 Answer

SOURCE: NEED INSTRUCTIONS TO GROW LOST THEM.

there is a link to the instruction manual on this page: http://www.discoverthis.com/smitcrystal.html

Posted on Apr 04, 2009

Anonymous

  • 1 Answer

SOURCE: I lost my space age crystal growing kit instructions

i lost my space age crystal growing kit instructions...

Posted on Sep 04, 2009

Anonymous

  • 1 Answer

SOURCE: My Discovery Kids Crystals growing kit is missing instructions

DISCOVERY KIDS INVENTIVE DISCOVERY KIDS LAB 9+ 8 UNIQUE CRYSTAL FORMATIONS WITH 12 CRYSTAL GROWING ACTIVITIES. NO INSTRUCTIONS. WOULD SOMEONE PLEASE POST INSTRUCTIONS TO 1 OR MORE GLOW IN THE DARK GEODE, SQUISHY CRYSTALS, SPIKEY CLEAR CRYSTALS, RED GEODE, COLORFUL STALACTITES? THANK YOU, THE COUSINS!

Posted on Nov 04, 2010

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How to get crystals fast


A supersaturated solution of the desired crystal id the best way! Try heating the water to boiling point so that more solute dissolves into the water.
Keep adding more solute until no more will dissolve and leave it to cool.
After it cools, you will see crystals growing in the solution. If you select a large crystal. place it into a cup and pour over it the super-saturated (cool) solution, the crystal will grow very fast. This is due to the molecular bonding (strong nuclear force) between the crystal and the solution.

Enjoy!

Dec 31, 2014 | Fast Computers & Internet

3 Answers

I just bought a small crystal growing kit and the instructions are missing.


I had one as a Kid. Pour enough water to fill the jar about 3/4 into a pot and add powder. Heat till dissolved. Pour into jar and place rock in the bottom. The crystals should start to grow in about a week or less... good luck

Jan 11, 2012 | Toys

1 Answer

The soap dispenser opens & the soap tablet (power ball) drops to the bottom but doesn't dissolve


1. Water temp is wrong should be 140-145
2. spray arms clogged with food
3. water valve is not letter the correct amount of water in

after it fill's check to see water amount in bottom , dose it sound like it is starving for water ? it would sound like it was surging

Dec 01, 2011 | Whirlpool GU2400XTP Built-in Dishwasher

2 Answers

If you have this crystal growing kit, please help. I lost, or didn't get containers a, b, and c. what can I use to replace them? I need to see what they look like. I did experiment #2 in the manual,...


This product is manufactured by poof-slinky. Go to poof-slinky.com/instructions for a list of products. Look under "Scientific Explorer" for Ultimate Crystal Growing Kit. Clink on it for a pdf of the instruction manual to download. Good luck!

Sep 06, 2011 | Scientific Explorer Ultimate Crystal...

1 Answer

Do & Discover Crystal Growing kit came with 2 spanish ONLY directions...How do we get the right dirsctions so my son can Do & Discover?!


I patiently used Google Translate and got this. The instructions may not be in perfect English, but it's good enough to understand. Good luck :)

GROWING CRYSTALS
1.
experiments require a large measurement cup (at least 32fl oz / 0.9 1) Heat resistant glass mix the powder and boiling water. The vessel measures must be glass or plastic Resistant to heat. You also need a medium saucepan (at least 32 fl oz / 0, 9 1) to boil water. Separate carefully cut molds, as pictured. Make sure to leave a border around each mold. Also remove sharp edges from the edges with scissors.
2.
Use a large glass measure (at least 32 fl oz / 0, 9 1) (not included) to measure 0.68 liters of water and pour into a medium-size saucepan. Heat the pan until the water boils.
3.
Open the bag of potassium sulfate 10 (diamond frosting) with chemical crystal growth and pour the contents into the glass of measures.
4.
Pour boiling water in medium saucepan shot glass with the contents of the bag 10.
5.
Stir the mixture with the big stick until all the grains are completely dissolved chemicals. NOTE: Let the mixture cool for 5 minutes after the grains have dissolved.
6.
placed 2 rocks on the bottom base of the 5-sized plastic molds "C" of growth. These basement rocks should rise only about 3 / 4 "(2cm) from the bottom of mold growth.
7.
Pour the chemical solution / water shot glass molds in size 5 "C" for crystal growth. Make sure to fill each mold in the same way, leave an inch (8mm) of space between the liquid and the edge.
8.
After removing the bottle cap coloring dye, carefully cut with scissors (not included) the tip of the boat. Individual drops slowly drops of dye into the mold of crystal growth. see diagram following Mercedes to mix colors. Once you add the dye mixture solution with the small mixing stick. NOTE: Do not add dye to the mold of a glass. transparent crystals are better for the electronic.
9.
Place the mold of crystal growth in a place where not disturbed by movements or changes in temperature. crystals begin to grow in a matter of hours. let the crystals grow for three or four days without disturbing them. You can then remove the crystals from the solution. For best results, wash the crystals abundantly in the sink to remove excess dye and place on a newspaper or paper towel for a day to dry.
10.
if the mass of rock crystal and the base have been a square shape due to the structure of the mold growth, you can break the remaining crystals that form the block so that the crystalline mass display look more natural from the geological point of view. to expose the glass, LED lights the base by pressing the button on the bottom. transparent glass placed at the base and see how it changes color. if you are not using the base, be sure to extinguish by pressing the button again. to replace the battery, remove the cover with a screwdriver as shown below. NOTE: with the help of a magnifying glass, look closely at the detailed crystal structure of the crystals finalized.
Beak-shaped crystals: follow steps 2-10 with the following changes: In step 2, only 0.34 a boil water. In step 3, use the contents of the bag 11.
In step 6 uses the five molds size "D" of growth of crystals with a single rock in each base.
In step 8 uses color guidelines mold "D" (crystals spike) in the diagram below.
NOTES: replacement of the battery base. Place the base upside down. Now you can remove the battery cover to access it, as shown in the image below.

Jan 10, 2011 | Edu-Science Toys

1 Answer

We bought an grow colossal chrystals kit but no instruction manual included


Hi, cats92357,

Please allow me to give you some general instructions that might serve you well despite not having your instruction manual. I have had a lot of experience growing crystals, starting way back when I was a high school sophomore, and later after my college days when I was a chemical researcher often needing to purify chemical compounds. There were many different methods I used, but crystallization has always been one of my favorite ways, especially when my lab was in my childhood home's kitchen. Back then I followed detailed recipes (like you are probably expecting) from library books, but I always found them so tedious because of their many steps.

I think you might appreciate a simpler set of instructions that'll give you the general ideas behind successful crytal growing that you could apply to almost any inorganic chemicals ("salts") you have available in your chemistry kit or in your home.

The General Method (no details at first to give you just the overview - for details see the very bottom of this posted message.)
  1. Prepare a saturated solution of the chemical compound (the "solute") in water (the "solvent") at room temperature.
  2. Decant off most of the clear solution into another container, a process that allows you to separate the liquid from the excess solid on the bottom, so the liquid is particle-free.
  3. Add slightly more of the solid chemical to the saturated solution, keeping a record of how much you added.
  4. Heat the heterogeneous mixture (liquid + undissolved solid) to dissolve all of the solid.
  5. Filter out any undissolved solids particles to produce a perfectly clear solution still at the elevated temperature.
  6. Cover the top of the clear hot solution (loosely wrapped aluminum foil or paper towel) and let it cool slowly back down to room temperature. At this point you will have made what is called a supersaturated solution. That is what you need for successful crystal growing.
OK, now while the solution is cooling down, you can get different and interesting results depending on what you do next.

You could do one or more of the following steps:
  • Let the solution continue to cool down slowly undisturbed and let crystals begin to form spontaneously. This could take minutes, hours, or days, depending on a) the solute, b) the amount of chemical you added in step 2, and/or c) on how fast the solution cools. YOUR CRYSTALS WILL BE LARGER IF THEY FORM SLOWLY. THE FASTER THEY FORM, THE SMALLER THEY WILL BE. There's a lot of experimentation you could do to obtain optimum results! Just keep a record of how much chemical used, and every step of your procedure, so you can reproduce what you did, and so you can have a reference upon which to make small measurable changes in your scientific investigations.
  • Gently scratch the inside of the container (preferably made of glass) just below the surface of the room-temperature liquid with a glass stirring rod. Do this if you get impatient, since this technique often speeds up the crystallization process. The scratched surface, if you could see it under a high-powered microscope, would reveal broken silicon oxide bonds (from the molecular structure of glass) that would attract ions from your solute and initiate the crystallization process. You would see tiny crystals forming at the freshly scratced surface. They would become the nucleus or center for crystal growth. If you are using an glass container that has had a lot of use, there will already be enough scratched surfaces to do the job without your using a stirring rod. If you want more control on the rate of crystallization, I recommend that you use a brand new unused glass container.
  • Suspend your best tiny seed crystal (of the same substance) inside the cooling solution. This will cause most of the solute to grow only on your seed crystal and not so much on the glass surfaces. You can get really big crystals this way! The seed crytal would have to be large enough to allow tying with sewing thread. The seed crystal can be made by pouring a small volume of the still hot solution into a petri dish or some other small container like a saucer or dessert bowl or cup, etc, to have a shallow liquid level. Cover very loosely with paper towel and let the water evaporate. You want it to evaporate faster than your main solution above, but slow enough to allow crystals large enough to tie with thread. BE CAREFUL NOT TO SUSPEND THE SEED CRYSTAL IN THE SOLUTION WHILE IT IS STILL HOT ENOUGH TO DISSOLVE IT. Let the solution cool some first. Keep trying until your seed crystal does not dissolve; it's no big deal if it does, just tie another one and try again until you succeed. It will take some practice.
Salts that are often used for successful crystallization experiments are:
  • copper sulfate pentahydrate, CuSO4*5H2O. I'm using the asterisk to indicate that the water molecules are bonded to the metal. You can probably buy this salt at gardening shops, because it is used as a fungicide and also as a root killer to control tree root growth. It also is sometimes called "blue vitriol" or "bluestone." You probably guessed it, this hydrate is a beautiful blue crystalline solid.
  • aluminum potassium sulfate, KAl(SO4)2*12H2O, also known as potash alum (icolorless), and can be bought in a grocery store, because it is used in pickling.
  • chromium potassium sulfate, KCr(SO4)2*12H2O, also known as chrom alum (dark violet), and is used in tanning leather.
More details regarding the "General Method" described at the top:
  • Step 1 - Add enough chemical until the solid no longer dissolves but instead just falls to the bottom of the container. Add, stir, add, stir, etc, until you get a small layer of solid on the bottom of the container. This process allows you to form the needed saturated solution. It can hold only a certain amount of the chemical at a given temperature.
  • Step 2 - You could omit this decantation step if you were satisfied with the amount of solid on the bottom of the container.
  • Step 3 - You could also omit this step if you decided to use the solid already placed on the bottom of the container during step 1. However, using steps 2 and 3 as originally listed at the top might be better if you would like to be able to measure the amount of extra solid used.
  • Step 4 - This heating step necessary to convert the saturated solution into an unsaturated solution, that is a solution that has not reached its maximum level of dissolved solute. For most solutes, their ability to dissolve in water increases with temperature. The higher the temperature, the more salt can dissolve in a given volume of solvent.
  • Step 5 - This filtering step is needed to remove impurities, including dust, which could interfere with the crystallization process. You could use an oven mit to hold the container while you tilt it and pour the liquid into another (clean) container. Or, fold some paper towels together to use as an insulating strap to wrap around the neck of the container with both hands as you pour. DO THIS QUICKLY TO AVOID RAPID AND UNCONTROLLED COOLING. Too fast cooling will almost always result in the formation of small crystals.
  • Step 6 - Place the still hot container of clear solution on top of a dry insulated surface to avoid a rapid transfer of heat and uncontrolled cooling.
Good luck!

###

Dec 26, 2010 | Scientific Explorer My First Chemistry Kit

1 Answer

What are the insructoins of grow colossal crystals kit


Hi, Plantmasterz,

Here's something I hope you will find useful until you can find your chemistry kit's instructions manual.

Please allow me to give you some general instructions that might serve you well despite not having your instruction manual. I have had a lot of experience growing crystals, starting way back when I was a high school sophomore, and later after my college days when I was a chemical researcher often needing to purify chemical compounds. There were many different methods I used, but crystallization has always been one of my favorite ways, especially when my lab was in my childhood home's kitchen. Back then I followed detailed recipes (like you are probably expecting) from library books, but I always found them so tedious because of their many steps.

I think you might appreciate a simpler set of instructions that'll give you the general ideas behind successful crytal growing that you could apply to almost any inorganic chemicals ("salts") you have available in your chemistry kit or in your home.

The General Method (no details at first to give you just the overview - for details see the very bottom of this posted message.)

  1. Prepare a saturated solution of the chemical compound (the "solute") in water (the "solvent") at room temperature.
  2. Decant (pour off) most of the clear solution into another container, a process that allows you to separate the liquid from the excess solid on the bottom, so the liquid is particle-free.
  3. Add slightly more of the solid chemical to the saturated solution, keeping a record of how much you added.
  4. Heat the heterogeneous mixture (liquid + undissolved solid) to dissolve all of the solid.
  5. Filter out any undissolved solids particles to produce a perfectly clear (no noticeable particles) solution, still at the elevated temperature. If the chemical compound is colored, the solution should be that color, but clear.
  6. Cover the top of the clear hot solution (loosely wrapped aluminum foil or paper towel) and let it cool slowly back down to room temperature. At this point you will have made what is called a supersaturated solution. That is what you need for successful crystal growing.
OK, now while the solution is cooling down, you can get different and interesting results depending on what you do next.

You could do one or more of the following steps:

  • Let the solution continue to cool down slowly undisturbed and let crystals begin to form spontaneously. This could take minutes, hours, or days, depending on a) the solute, b) the amount of chemical you added in step 2, and/or c) on how fast the solution cools. YOUR CRYSTALS WILL BE LARGER IF THEY FORM SLOWLY. THE FASTER THEY FORM, THE SMALLER THEY WILL BE. There's a lot of experimentation you could do to obtain optimum results! Just keep a record of how much chemical used, and every step of your procedure, so you can reproduce what you did, and so you can have a reference upon which to make small measurable changes in your scientific investigations.
  • Gently scratch the inside of the container (preferably made of glass) just below the surface of the room-temperature liquid with a glass stirring rod. Do this if you get impatient, since this technique often speeds up the crystallization process. The scratched surface, if you could see it under a high-powered microscope, would reveal broken silicon oxide bonds (from the molecular structure of glass) that would attract ions from your solute and initiate the crystallization process. You would see tiny crystals forming at the freshly scratced surface. They would become the nucleus or center for crystal growth. If you are using an glass container that has had a lot of use, there will already be enough scratched surfaces to do the job without your using a stirring rod. If you want more control on the rate of crystallization, I recommend that you use a brand new unused glass container.
  • Suspend your best tiny seed crystal (of the same substance) inside the cooling solution. Tie it with a length of sewing thread tied to the end of a pencil or other rod-shaped support. Hang the seed crystal away from the sides and bottom of the container. This will cause most of the solute to grow only on your seed crystal and not so much on the glass surfaces. You can get really big crystals this way! The seed crytal would have to be large enough to allow tying with sewing thread.
  • How to grow a seed crystal and successfully position it: The seed crystal can be made by pouring a small volume of the still hot solution into a petri dish or some other small container like a saucer or dessert bowl or cup, etc, to have a shallow liquid level. Cover very loosely with paper towel and let the water evaporate. You want it to evaporate faster than your main solution above, but slow enough to allow crystals large enough to tie with thread. BE CAREFUL NOT TO SUSPEND THE SEED CRYSTAL IN THE SOLUTION WHILE IT IS STILL HOT ENOUGH TO DISSOLVE IT. Let the solution cool just a little. Keep trying until your seed crystal does not dissolve; it's no big thing if it does, just tie another one and try again until you succeed. It will take some practice.
Salts that are often used for successful crystallization experiments are:

  • copper sulfate pentahydrate, CuSO4*5H2O. I'm using the asterisk to indicate that the water molecules are bonded to the metal. You can probably buy this salt at gardening shops, because it is used as a fungicide and also as a root killer to control tree root growth. It also is sometimes called "blue vitriol" or "bluestone." You probably guessed it, this hydrate is a beautiful blue crystalline solid.
  • aluminum potassium sulfate, KAl(SO4)2*12H2O, also known as potash alum (icolorless), and can be bought in a grocery store, because it is used in pickling.
  • chromium potassium sulfate, KCr(SO4)2*12H2O, also known as chrom alum (dark violet), and is used in tanning leather.
More details regarding the "General Method" described at the top: (the step numbers refer to the same steps listed above.)

  • Step 1 - Add enough chemical until the solid no longer dissolves but instead just falls to the bottom of the container. Add, stir, add, stir, etc, until you get a small layer of solid on the bottom of the container. This process allows you to form the needed saturated solution. It can hold only a certain amount of the chemical at a given temperature.
  • Step 2 - You could omit this decantation step if you were satisfied with the amount of solid on the bottom of the container.
  • Step 3 - You could also omit this step if you decided to use the solid already placed on the bottom of the container during step 1. However, using steps 2 and 3 as originally listed at the top might be better if you would like to be able to measure the amount of extra solid used.
  • Step 4 - This heating step necessary to convert the saturated solution into an unsaturated solution, that is a solution that has not reached its maximum level of dissolved solute. For most solutes, their ability to dissolve in water increases with temperature. The higher the temperature, the more salt can dissolve in a given volume of solvent.
  • Step 5 - This filtering step is needed to remove impurities, including dust, which could interfere with the crystallization process. You could use an oven mit to hold the container while you tilt it and pour the liquid into another (clean) container. Or, fold some paper towels together to use as an insulating strap to wrap around the neck of the container with both hands as you pour. DO THIS QUICKLY TO AVOID RAPID AND UNCONTROLLED COOLING. Too fast cooling will almost always result in the formation of small crystals.
  • Step 6 - Place the still hot container of clear solution on top of a dry insulated surface to avoid a rapid transfer of heat and uncontrolled cooling.
Good luck!

###

Dec 11, 2010 | Scientific Explorer My First Chemistry Kit

1 Answer

What is crystillization?


Hi, Sajidalidud,

Crystallization is a simple, yet powerful method for purifying solid substances, whether or not they are molecular or ionic. The main idea of the method is to dissolve the solid to make a solution of it, then causing it to fall back out of solution without its impurities. You'd just have to filter the solution away from the recovered, but purified solid. Before drying the purified solid you would "wash" it, while it is still on top of the filter paper, with 2 or 3 small portions of cold solvent (usually water). Finally, you would dry it by either letting it dry in the air, or by oven-drying it (that's quicker, but only advisable if the pure solid is stable to heat, or if the heat is set low enough to prevent melting).

The trick to successful crystallization is using a satisfactory solvent, one in which the solid is not excessively soluble (you'd never get it to fall back out as a solid if it is too soluble). The solvent has to be "good" enough, or course, to dissolve the solid. Depending on your chemical intuition or knowledge, you could narrow down the long list of possible solvents to a reasonable first choice. If the solid is polar (for example, like one of the thousands of salts), you would know to use only polar solvents, like water. Most ionic solids would not dissolve in anything except water, or some mixture of water and another polar solvent like ethanol or methanol - just how much alcohol would require some trial and error (experimentation).

If your solid were an organic compound, you would probably want to avoid using water; instead use something like alcohol, or alcohol-ether, etc. If your organic compound were a very polar organic compound, you might be able to use a small amount of water mixed with alcohol.

How does the desired solid crystalize free of the impurities?
Separation of desired solid from impurities is not merely a matter of differential solubility.
What allows the solid to crystallize pure is its particles' (ions or molecules) greatly selective attraction for other particles in solution like themselves. A solid's natural pure state is a crystalline matrix, which is very stable, and naturally "preferred" - something that can be explained best by thermodynamics theory - a topic best discussed in advanced chemistry courses.

Impurities that are present would not satisfy the most stable state, and would only interfere with it. The growing crystals of the pure solid can grow only by its natural attraction for other ions of the desired substance. The different ions of an ionic compound stack in well-defined ways, creating the most stable angles, patterns, and layers (the geometry) that are characteristic for the solid substance. This process would also probably be occurring much faster than the impurities could interfere.

The impurities, even if they could bind to the growing crystal's ions, would not be attracted as strongly; so as they momentarily drifted away from the crystal, the ions in higher concentration surrounding the growing sites on the crystal would stick and further block the interference of the impurities. So after a few hours of growing, the set of pure crystals of the solid would have formed on the sufaces of the container, and the impurities would still be dissolved in the solution.

Some practical considerations
If you have a low yield of crystals of the solid, how do you recover the rest of the solid in pure form?
You can recover much of it by processing the "mother liquor," a term going back to the days of alchemy. That's what you call the solution above the crystals, or the filtrate that goes through the filter paper. You could concentrate it to a smaller volume and allow crystallization to go further. So, it's best not to discard this solution after the first crop of crystals. I have usually obtained 2 or 3 crops of crystals, but generally, the second and third crops are not as pure. To increase their purity you could redissove the crystals in minimum solvent and repeat the usual process of crystallization ("recrystallization").

How to test the purity of your crystals
Take a melting point. If the melting point range is narrow, that is a good indicator of solid's purity. For example, suppose you had a solid that melted at 103.1 - 103.3 0C, that would indicate high purity. On the otherhand, if the range were, say, 103 - 106 0C, that would indicate low to moderate purity. A minimum acceptable purity depends on what application you have in mind for the solid. Often a 2-degree range is acceptable.

If you are lucky, you will have a sample of the pure crystalline solid as a reference. This will probably be the case, if your purpose is only to purify a sample of the solid that is a known substance, and not a new substance from your research. To prove the purity of your crystalline solid, take a melting point of it side by side with the reference sample. Their melting points should be very close to each other. If you don't have a sample of the commercial pure solid, you could just refer to the mp in a reference manual.

I hope my description is useful to you. Good luck in using crystallization!

###

Jul 14, 2010 | Scientific Explorer My First Chemistry Kit

4 Answers

MIssing Edu Science Crystal Growing Kit Instructions


We lost the directions to EduScience Crystal Kit we from Toys-R-Us--here's a site from the company that actually puts the kits together. Lists directions for all there kits
http://www.nsi-intonline.com/prin.html

Aug 22, 2009 | Toys

5 Answers

Missing instruction manual for Crystal growing kit.


www.toyday.co.uk/shop/crystal-growing-kit-instructions/info_12.html - 33k -

try this url--it is pretty much similar to all the kits.

cindy

Dec 12, 2008 | Toys

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