You’d need ##”3.1 g”## of sodium thiosulfate pentahydrate.
The molecular formula for sodium thiosulfate pentahydrate is ##Na_2S_2O_3*5H_2O##, which means that the molar mass of the compound will include the 5 water molecules.
##”molar mass” = 2*23 + 2*32.1 + 3* 16 + 5*18 = “248.2 g/mol”##
is defined as moles of per liter of solution; in this case, the solute includes the 5 water molecules per molecule of ##Na_2S_2O_3##. The number of moles of thiosulfate pentahydrate you’ll need is
##C = n/V => n = C * V##
##n = “0.025 mol/L” * 500*10^(-3)”L” = 12.5*10^(-3)”moles”##
Use the calculated molar weight of the hydrate to determine how much of it you need in grams
##12.5 * 10^(-3)”moles” * (“248.2 g”)/(“1 mole”) = “3.1 g”##
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