Map A General Chemistry 4th Edition University Science Books e Rock presented by

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Map A General Chemistry 4th Edition University Science Books e Rock presented by Sapling Leaming e quantity of atmospheric SO2(g) can be determined by reaction with H202(aq), according to the balanced chemical equation shown below. So, a H,O, aal+ SO, The amount of sulfuric acid produced can be determined by titration with sodium hydroxide of known concentration. An 888.0 gram sample of an air that is known to contain sulfur dioxide was reacted with excess hydrogen peroxide. Given that 18.50 mL of a 0.00250 M NaOH(aq) were required to neutralize the H2SO4(aq) produced, calculate the mass percentage of SO2(g) in the air sample. Number SO, 1.91 x 10 There is a hint available! View the hint by clicking on the divider bar again to hide the hint. Close O Previous ® Give Up & View Solution Check Answer Next H Ext Hint

Explanation / Answer

mol of NaOH reacted =    M*V

= 0.00250 M * 18.50 mL

= 0.04625 mmol

Since H2SO4 is diprotic acid,

mol of H2SO4 = mol of NaOH / 2

= 0.04625 / 2 mmol

= 0.023125 mmol

from reaction,

mol of SO2= mol of H2SO4

so,

mol of SO2 required = 0.023125 mmol

= 2.3125*10^-5 mol

molar mass of SO2 = 64 g/mol

mass of SO2 = number of mol * molar mass

= 2.3125*10^-5 mol * 64 g/mol

= 1.48*10^-3 g

= 0.00148 g

mass % SO2 = mass of SO2 * 100 / total mass

= 0.00148 * 100 / 888

= 1.67*10^-4 %

Answer: 1.67*10^-4 %

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