At 25 degree celsius, 50mL of .150M AgNO3 is mixed with 30mL of .300M NaC2H3O2?

Question

can't figure it out!
1)After the solution is filtered to remove the precipitant, a 20mL sample of solution required 12.63 mL of .100M KSCN to titrate to the end point. Determine the number of millimoles of Ag+ in the 20mL sample. NEED IT IN mmOLES.
2)how many mmoles of Ag must have been in the 80 ml of soln?
3) determine the number of mmoles of ag in the precipitant. How many moles mmoles of c2h3o2 must be in the precipitant?
thank you!!!!

can't figure it out!
1)After the solution is filtered to remove the precipitant, a 20mL sample of solution required 12.63 mL of .100M KSCN to titrate to the end point. Determine the number of millimoles of Ag+ in the 20mL sample. NEED IT IN mmOLES.
2)how many mmoles of Ag must have been in the 80 ml of soln?
3) determine the number of mmoles of ag in the precipitant. How many moles mmoles of c2h3o2 must be in the precipitant?
thank you!!!!

Explanation / Answer

moles acetate = 0.030 L x 0.300 M=0.0090
moles silver acetate precipitate = 0.0090 => moles Ag+ in 50 mL of the solution
moles Ag+ in 20 mL = 0.0036
moles SCN- used = 0.01263 L x 0.100 M = 0.001263 in 20 mL = moles Ag+

total moles Ag+ = 0.0036 + 0.001263 =0.004863

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