well its because nak75321 is not compatible with KI. sorry for any inconvenience :)
To prepare a 0.1N Na2S2O3 solution, dissolve 24.98 grams of Na2S2O3·5H2O (sodium thiosulfate pentahydrate) in distilled water and dilute to 1 liter in a volumetric flask. This will give you a 0.1N (normal) solution of Na2S2O3.
Dissolve 2.0 grams of iodine and 6.0 grams of KI in 100.0 ml of H2O.
The molecular formula of sodium thiosulfate is Na2S2O3.
None. helium doesnt react with any other element
The molecular mass of sodium thiosulfate heptahydrate is 248,18 g.
It doesnt
Na2S2O3 does react with AgNO3, it is a reaction widely used in non-digital photography. The reaction is: 2AgNO3 + Na2S2O3 = Ag2S2o3 + 2 NaNo3 If hypo is taken in a limited amount, then this happens. The Ag thiosulphate thus formed goes through a change of colour (termed as 'play of colour'). Ag2S2O3 (white) --> yellow --> orange --> brown --> black (AgS ppt). But if hypo is taken in excess amount, then a complex [Ag(S2O3)2]3- , it is readily dissolved in water.
To prepare a 0.1N Na2S2O3 solution, dissolve 24.98 grams of Na2S2O3·5H2O (sodium thiosulfate pentahydrate) in distilled water and dilute to 1 liter in a volumetric flask. This will give you a 0.1N (normal) solution of Na2S2O3.
first we calculate the molecular weight M.W=158.11 mass of Na2S2O3=M.W*concentration*volume(in litter) for a concentration of 0.001 mass of Na2S2O3=158.11*0.001*1=0.15811 g so we use this mass and continue the volume to be 1 L
The blank titration requires more sodium thiosulfate (Na2S2O3) because it compensates for any residual iodine in the reaction mixture that didn't react with the analyte. This residual iodine can interfere with the accuracy of the titration results, so more Na2S2O3 is needed to completely neutralize it.
Na2S2O3(aq) + 2HCL(aq) => 2NaCl(aq) + S(s) + SO2(g) + H2O(l)
no it doesnt blow up
Resilient.
Gold is a metal that does not react with most acids or water.
Sodium thiosulfate
Na2S2O3
To find the amount of Na2S2O3 solution needed, first calculate the moles of AgBr using its molar mass. Then, use the stoichiometry of the balanced equation between AgBr and Na2S2O3 to determine the moles of Na2S2O3 required. Finally, use the molarity of Na2S2O3 to find the volume needed in milliliters.