Question

Practice Problems with Solubility in Acidic or Complexing Solutions 1. Like we do with our titrations, sometimes it's worthwhile to consider a stoichiometric reaction before dealing with an equilibrium in solubility problems also! For example, if you mix together 10.00 mL of 0.100 M AgNO3 and 10.00 mL of 0.100 M K CrO4... a. What precipitates, and how many grams of that precipitate are made? b. What are the concentrations of [Ag], [K], [NO; ) and (CrO4) at equilibrium? c. In pure water, you can dissolve about 8.4 x 10-mol Ag2 CrO4 per liter... compare your concentrations from part (b) and explain the difference with Le Châtelier's Principle-type logic.

not sure how answer this question or even begin

Answer 1

Date:.... Page:.......... Sen. The reaction takes place as follows- Molare Volume Ke (204+243N03 - 0.100M_0:100M 1ome 10 ml 0.100x10=1 0.100 X 1024 > KNO2+ Ag. 9204 Brick Red Pot Moles H Now determine the limiting reagent- for K₂ GO 4 = moles – zl. Stoichiometric I - coefficient AgNO3 7 2 = 0.5 |_ Limiting Reagent A9 Noz- -al-Ag, 604_is_a_buick_and precipitate, weight_et_Ag2 (804 =_booles K Molecular = 0:5 X 331.5 z 165.75 g vol X molarity concentrations are 10) = Total rol. [Agt) = T-40X0-100 ? = +10 ___= 0.05 M -b>

Date: ............ Page: ............ CR+) = 2XL0 X 0.100 = 0.10M. 10+10 [103] = lox_0:100__= 0.05 M. 10+10 [ Cror2 = 10x 0.100 = 0.05 M 16+10 c7 Ag Goa 0 4x 105 in co C 2 Ag+ + Croft x 0.4x105 0.4x10 =ht:0x100M CAgtJ = 16.0x10-5 M [60, 2] = 0.4X18 S M According to he Chatelier's Principles, the equilibrium will shift in forward direction as the concoutaa ation of [Ag] increases.