How much does sodium thiosulfate weigh?
I know this is a broad question, but how much would the average 1 mL of sodium thiosulfate weigh?
Asked by Wesley Hoenig 2 years ago.
According to the Wikipedia article on sodium thiosulfate, the density of Na2S2O3 is 1.667 g/cm^3. This appears to be the density for the pure substance, rather than a commonly observed pentahydrate (Na2S2O3 dot 5H2O). Since you ask about a "milliliter," you may be asking about sodium thiosulfate in solution rather than in its crystalline form. Again using the Wikipedia article, the solubility of Na2S2O3 in water is given as 76.4 g per 100 grams of H2O, at 20 Celsius. Since a gram of pure water occupies one milliliter, it seems the most a milliliter of sodium thiosulfate solution (in water) could weigh would be 176 grams. Answered by Tashia Ivers 2 years ago.
What is the equation for water + sodium thiosulfate?
What is the word equation for: Water + sodium thiosulfate And what is the chemical equation for: H20 + Na2S2O3 Thanks in advance
Asked by Sigrid Mccraney 2 years ago.
Na2S2O3 + H2O is sodium thiosulfate + water. The chemical equation is simple. It's a double replacement reaction, the hydrogen and sodium swap places. Hydrogen and Sodium have the same charge, so don't worry about oxidation numbers. Na2S2O3 + H2O --> H2S2O3 + Na2O notice in this equation the product is the same thing as the reactants only with the H and Na switched, I didn't have to change any other numbers, since H and Na have the same charge of +1. Answered by Leslee Folks 2 years ago.
wrong answer 2 NaOH + 2SO2 Answered by Lacresha Aoki 2 years ago.
Theoretical yield of sodium thiosulfate pentahydrate (Na2S2O3 * 5H2O)?
I have 12.6g (.099m) of NaSO3 and 3.5g (.109m) of S. I'm not asking for an answer, I just need to know how to find it myself. How do I find the theoretical yield of sodium thiosulfate pentahydrate?
Asked by Karole Demyers 2 years ago.
Theoretical Yield: Given mass of 1st reactant * molar mass of sodium thiosulfate pentahydrate (multiply total by number of moles if any) / molar mass of reactant 1 (multiply total by number of moles if any) Given mass of 2nd reactant * molar mass of sodium thiosulfate pentahydrate (multiply total by number of moles if any) / molar mass of reactant 2 (multiply total by number of moles if any) Out of the both numbers you get, the smaller number is your theoretical yield because you can only make as much as your limiting reagent lets you. Answered by Corina Farquhar 2 years ago.
You have a solution that is 16.2% sodium thiosulfate...?
you have a solution that is 16.2% sodium thiosulfate,Na2S2O3, by mass.a)what mass of sodium thiosulfate is in 80.0 g of solution?b) How many moles of sodium thiosulfate are in 80.0 g of solution?c) if 80.0 g of sodium thiosulfate solution is diluted to 250.0 mL with water, what is the molarity of the...
Asked by Adriana Galaz 2 years ago.
you have a solution that is 16.2% sodium thiosulfate,Na2S2O3, by mass. a)what mass of sodium thiosulfate is in 80.0 g of solution? b) How many moles of sodium thiosulfate are in 80.0 g of solution? c) if 80.0 g of sodium thiosulfate solution is diluted to 250.0 mL with water, what is the molarity of the resulting solution? please show me how to do each part step by step. thank you! Answered by Lang Ziek 2 years ago.
a.) 16.2% = .162 .162 = mass of sodium thiosulfate / (80g of solution) The equation used above is simply mass of solute / total mass of solution, you can use it to determine the percentage of something by mass. So solve for mass of sodium thiosulfate, and you get 12.96g. b.) First find the molar mass of Sodium Thiosulfate you have. The molar mass of it is (22.990x2 + 32.06 x 2 + 16 x 3) = 158.1g Now you can simply convert the grams of sodium thiosulfate (which you calculated from part a) to moles. 12.96g x (1mole / 158.1g ) = .082 moles c.) Molarity = moles of solute / Liters of solution You have moles of solute from part b (.082moles). Therefore, change 250.0 mL to Liters, 250.0 mL x (1 L / 1000 mL) = .25 L Then you can use your molarity formula and: .082 moles / .25 L = .328 M (molarity) Answered by Aracelis Leavy 2 years ago.
Sodium Thiosulfate Solution Answered by Antionette Jesperson 2 years ago.
1) Calculate the molar mass of sodium thiosulfate 1 mol Na2S2O3 weighs X grams 2) If you dissolve X grams in 1000 mL you will have a 1 M solution thus for a 0.25 M solution you need Y grams Calculate Y 3) You don't need to prepare 1000 mL but only 500mL thus for preparing 500 mL you need Z grams Calculate Z. Z is what you need Now do your homework. Answered by Chara Goertz 2 years ago.
Calculate to the nearest 0.01 gram the amount of sodium thiosulfate pentahydrate needed to prepare 2000 mL of a 0.11 M solution.?
Asked by Gina Fabus 2 years ago.
sodium thiosulfate pentahydrate --> H10Na2O8S2 (add their total molar masses) molar mass = 248.1841 g per mol molarity = mol solute / liter solution 0.11 M = mol solute / 2 L mol solute = 0.11 M x 2 L mol solute = 0.22 mol solute convert mole to gram: 0.22 mol x 248.1841 g/mol = 54.60 g sodium thiosulfate pentahydrate Answered by June Sylvester 2 years ago.
find the molar mass. 2000 mL = 2 L (0.11 mole / L) x (2 L) X molar mass ---- this gives the answer Answered by Easter Holshovser 2 years ago.
Explain in detail how the calculated average percent of NaOCl change if some sodium thiosulfate droplets...?
Explain in detail how the calculated average percent of NaOCl change if some sodium thiosulfate droplets adhered to the inside of the buret during the titration.
Asked by Caterina Kreitner 2 years ago.
the issue is that the droplets on the inside of the buret will cause the volume of added thiosulfate to appear to be more than it actually is. if you added 10ml thiosulfate but drops of thiosulfate remain on the sides of the buret, did you actually add 10ml or less than 10ml? you will have added less than 10ml since part of the 10ml that the buret says you added are still adhered to the side of the buret. as for the hypochlorite concentration, if you added less than 10ml thiosulfate but the buret says that you added 10 ml, your calculated hypochlorite concentration will be off. you will have calculated the number of moles of thiosulfate as being higher than the moles you actually added. therefore, the titration tells you that you have more hypochlorite in solution than you actually do have. 0.01L x 0.1M thiosulfate = 0.001moles added thiosulfate binds hypochlorite in a 1:2 ratio so this will tell you that you have 0.002moles hypochlorite if you actually added only 9.5ml: 0.0095L x 0.1M thiosulfate = 0.0095moles added therefore, the actual moles of hypochlorite would be 0.0195moles the droplets adhering to the inside of the buret will cause you to 'think' you used more thiosulfate than you actually did, thereby increasing the concentration of hypochlorite as well. Answered by Vinnie Kinsler 2 years ago.
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Why is it important in the iodine clock reaction that there is only a small quantity of sodium thiosulfate?
Asked by Lilliam Mcnelley 2 years ago.
with out any sodium thiosulfate, the oxidizer would produce iodine & it would turn the dark color almost immediately so we add some sodium thiosulfate, for it destoys the I2 as fast as the oxidizer produces it... once the sodium thiosulfate is depleted, then the I2 remains & the color of it with starch appears add too much sodium thiosulfate, & we have too long of a wait... to destroy the large amount of sodium thiosulfate.... too much added... I have seen it take hours Answered by Avelina Lourence 2 years ago.
How do i convert 24.5 mL of sodium thiosulfate into grams?
a) how do i convert 24.5 mL of sodium thiosulfate into grams?
Asked by Hester Rico 2 years ago.
Sodium Thiosulfate Wiki Answered by Rachael Reistad 2 years ago.