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A chemist adds 225.0 mL of a 8.0x10-5 mmol/L solution of silver (II) oxide solution to...

A chemist adds 225.0 mL of a 8.0x10-5 mmol/L solution of silver (II) oxide solution to a reaction flask. Calculate the mass of micrograms in silver (II) oxide the chemist has added to the flask..Please answer using two significant figures.

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Expert Solution

AgO miili moles = M x V ( in L)        where V = 225 ml = 0.225 L

                         = ( 8 x 10^ -5) mmol/L   x (0.225 L)

                   = 1.8 x 10^ -5

AgO moles = milli moles x 10^ -3 = 1.8 x 10^ -5 x 10^ -3 = 1.8 x 10^ -8

AgO mass = moles x molar mass of AgO

               = 1.8 x 10^ -8 mol x 123.9 g/mol

               = 2.2 x 10^ -6 g

             = 2.2 ug                       ( since 1ug = 10^ -6g)

hence silver (II) oxide mass is 2.2 micrograms

queen_honey_blossom answered 1 year ago
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