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Show work please 1) What is the result if 175.0 mL of 0.0055 M KCl solution...

Show work please

1) What is the result if 175.0 mL of 0.0055 M KCl solution is added to 145.0 mL of 0.0015 M AgNO3 solution ?  The Ksp for AgCl is 1.77 x 10-10.   ________________

            a.  No precipitate will form.

            b.  Nothing will happen since both potassium chloride and silver nitrate are soluble.

                  c.  A precipitate will form since Ksp > Q.

            d.  A precipitate will form since Q > Ksp for AgCl    

2) Which process is likely to have ΔS > 0?  _________

              a.   CO(g) + Cl2(g)     COCl2 (g)

              b.  Pb2+(aq) +  2 Cl-(aq)   PbCl2 (s) at 25ºC

3)What is the pH and [C2O42-] for a 0.150 M H2C2O4 solution? (Ka1 = 6.0 x 10-2; Ka2 = 6.1 x 10-5)

pH = _________;          [C2O42-] = ___________

              c.   SiO2(s)  +  3 C(s)    SiC(s)  +  2 CO(g)

              d.   H2O(g)   H2O(l)  at 100ºC

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Expert Solution

queen_honey_blossom answered 2 years ago
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