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18 Nov 2019
If you were to take a quantity, of PbCI_2, a sparingly soluble salt - maybe 10g - and put it into water, some of it would dissolve based on its K_sp. The equation for this reaction is: PbCI_2 (s) Pb^2+ (aq) + 2CI^- (aq). What will the ratio of the concentrations of Pb^2+ to CI^- be? In other words, wat will be [Pb^2+]/[CI^-]? Equal volumes of 1.0 M Pb(NO_3)_2j and 0.001 M NaI are mixed in a beaker and PbI_2 precipitates out as the solution reached equilibrium. What will the ratio of the concentrations of Pb^2+ to I be in the beaker at equilibrium? Is this the same ratio as you found in problem #1? Why not? In this lab you will be working with potassium chromate (find the SDS here). Please list at list three specific hazards associated with potassium chromate.
If you were to take a quantity, of PbCI_2, a sparingly soluble salt - maybe 10g - and put it into water, some of it would dissolve based on its K_sp. The equation for this reaction is: PbCI_2 (s) Pb^2+ (aq) + 2CI^- (aq). What will the ratio of the concentrations of Pb^2+ to CI^- be? In other words, wat will be [Pb^2+]/[CI^-]? Equal volumes of 1.0 M Pb(NO_3)_2j and 0.001 M NaI are mixed in a beaker and PbI_2 precipitates out as the solution reached equilibrium. What will the ratio of the concentrations of Pb^2+ to I be in the beaker at equilibrium? Is this the same ratio as you found in problem #1? Why not? In this lab you will be working with potassium chromate (find the SDS here). Please list at list three specific hazards associated with potassium chromate.
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Hubert KochLv2
15 Jun 2019
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