Consider a mixture of 75.0 mL of 1.00 × 10−6 M thallium nitrate (TlNO3(aq)) and 100.0 mL of seawater (0.51 M in NaCl(aq)) (a) What sparingly soluble compound may form? Write out the chemical equation for its solubility equilibrium, its Ksp expression and the value of its Ksp.  (b) Will a precipitate form from this mixture? Justify your answer.

Express Ksp in terms of molar solubility, x, for the salts with the given formulas. AB(s) Ksp AB, (s) Ksp = AB, (s) Ksp = A,B, (s) Ksp =

The Ksp for CuBr at a certain temperature is equal to 6.65*10^(-9). What is the molar solubility of the compound at this temperature?

Solid silver acetate is slowly added to 50.0 mL of a 0.0620 M sodium sulfite solution. The concentration of silver ion required to just initiate precipitation is  ? M. (Assume that Ksp (AgSO3)= 1.5 x 10^-14.)

35). Will a precipitate of magnesium fluoride form when 400. mL of 1.5 x 10-3 M MgCl2 are added to 600. mL of 2.5 x 10-3M NaF? (Ksp of MgF2 = 6.9 x 10-9) Calculate Q and explain your answer. (b) Calculate the new concentration of Mg2+ ion.                              (c) Calculate the new concentration of F– ion.                                   (d) Show the Q expression.                                                                (e) Calculate Q.      (f) Will a precipitate of magnesium fluoride form?

For PbCl2, Ksp = 0.0000137 What is the molar solubility of PbCl2.

When 22.0 mL of a 2.41×10-4M sodium iodide solution is combined with 15.0 mL of a 2.61×10-4 M lead acetate solution does a precipitate form?| |(yes or no) For these conditions the Reaction Quotient, Q, is equal to

Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOHKOH required for precipitation to begin in each case. 1. 0.010 MM CaCl2CaCl2 (Ksp=4.68×10−6Ksp=4.68×10−6 for Ca(OH)2Ca(OH)2) 2. 0.0020 MM Fe(NO3)2Fe(NO3)2 (Ksp=4.87×10−17Ksp=4.87×10−17 for Fe(OH)2Fe(OH)2) 3. 0.0016 MM MgBr2MgBr2 (Ksp=2.06×10−13Ksp=2.06×10−13 for Mg(OH)2Mg(OH)2)

If you mix 50.0 mL of 0.50 M AgNO3 (aq) with 25.0 mL of 0.010 M NaI (aq) at 25°C, does AgI (s) precipitate? The Ksp for AgI is 8.52 x 10^-17.

The KspKsp of cobalt(II) hydroxide, Co(OH)2, is 5.92×10−15. Calculate the molar solubility, s, of this compound.