10 A 50mL of 020 M solution of AgNO 3 is mixed with 50mL solution of 0010 M

10 a 50ml of 020 m solution of agno 3 is mixed with

This preview shows page 23 - 27 out of 33 pages.

10. A 50mL of 0.20 M solution of AgNO3is mixed with 50mL solution of 0.010 M NaCl will AgCl (s) precipitate?
Image of page 23
17-24 To calculate the new concentration… New [Ag + ] = M 0.10 (100) (0.20)(50) V V M total New [Cl ] = M 0.0050 (100) ) (0.010)(50 V V M total [Ag + ][Cl ] = (0.10)(0.0050) = 5.0 x 10 4 >> 1.6 x 10 10 = K sp Therefore… AgCl precipitates. Do at home… a) Would there be a precipitate when one mixes 200mL of 1.0 x 10 5 M AgNO 3 with 800mL of 1.8 x 10 5 M NaCl? b) What is the [Cl ] in 0.25 M MgCl 2 ? ( strong electrolyte ). c) Would there be a precipitate when one mixes 100 mL of 1.00 x 10 4 M AgNO 3 with 100 mL of 1.5 x 10 4 M MgCl 2 ? Hint: calculate [Ag + ][Cl ].
Image of page 24
Consider the following: To a solution in which [Ca2+] is 0.0050 M, one adds sufficient sodium oxalate solid, Na2C2O4, to make the solution also having [C2O42-] =0.0100M. Will the precipitation of CaC2O4(s) be complete? Kspfor CaC2O4=2.7x10-9. (s) (aq) s
Image of page 25
Question: Is there a way to precipitate one ion (one salt the one that has the lower solubility of the two salts ), leaving the other ion still in solution? Namely, can one have selective precipitation? -17What should the [Ag+] be to start precipitating AgCl(s)? M M
Image of page 26
Image of page 27

You've reached the end of your free preview.

Want to read all 33 pages?

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture