How many moles of Ag+ ions are present in 33 . mL of a 0.520 M Ag2SO4 solution?
2007-03-26 04:41:40 · 3 answers · asked by kris h 1 in Science & Mathematics ➔ Chemistry
0.520 moles / 1.00 L = x moles / 0.033 L
Calculate moles from equation above. Multiply by 2 since there are 2 Ag 1+ for each molecule.
2007-03-26 05:05:28 · answer #1 · answered by physandchemteach 7 · 0⤊ 0⤋
First write the ionization equation for the compound:
Ag2SO4------------2Ag(+) +SO4 (2-) the charges on the ions are in brackets, the ratio is thus:
1 : 2 : 1
Then find the number of moles of Ag2SO4 that is in the solution.
Moles of Ag2SO4 = (33/1000)*.520
=.01716
Since the ratio of Ag2SO4: Ag+ = 1:2
No of moles of Ag+ = 2*.01716
=.03432
2007-03-26 05:08:52 · answer #2 · answered by Med.chem 1 · 0⤊ 0⤋
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2016-05-16 04:31:53 · answer #3 · answered by Anonymous · 0⤊ 0⤋