Asked by Emma
A clumsy chemist accidentally pours 100 mL of a 0.004 M Na2SO4 solution into a beaker containing 500 mL of 0.050 M CaCl2 solution. Will a precipitate be formed?
Answers
Answered by
DrBob222
Na2SO4 + CaCl2 ==> 2NaCl + CaSO4
I looked up on the internet to find Ksp for CaSO4 to be 4.93E-5. You should have posted Ksp from your notes/text. Use the Ksp from your notes and not the one I found.
What is the molar concentration of each component for the final solution?
M CaCl2 = 0.050 x (500/600) = 0.0417
M Na2SO4 = 0.004 x (100/600) = 0.000667
Qsp CaSO4 = (Ca^2+)(SO4^2-) =(0.000667)(0.0417) = 2.78E-5
A ppt will occur IF Ksp is exceeded. Since 2.78E-5 < 4.93E-5, no ppt will occur.
I looked up on the internet to find Ksp for CaSO4 to be 4.93E-5. You should have posted Ksp from your notes/text. Use the Ksp from your notes and not the one I found.
What is the molar concentration of each component for the final solution?
M CaCl2 = 0.050 x (500/600) = 0.0417
M Na2SO4 = 0.004 x (100/600) = 0.000667
Qsp CaSO4 = (Ca^2+)(SO4^2-) =(0.000667)(0.0417) = 2.78E-5
A ppt will occur IF Ksp is exceeded. Since 2.78E-5 < 4.93E-5, no ppt will occur.
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