Question 18 of 30 What is the solubility of La(IOs)s in a solution that contains 0.200 M La ions? (Ksp of La(IOs)s is 7.5 × 10-12)

Question 40 of 43 Submit What is the solubility of PbF, in a solution that contains 0.0600 M F- ions? (Ksp of PbF2 is 3.60 x 10-8) M 1 4 C 7 8 +/- x 10 0 Tap here or pull up for additional resources LO

Activity 4   Another example of going from KSP to Solubility.  Then, another application of LeChatelier’s Principle: The Common Ion Effect:  BaSO4 is a very toxic ion, yet BaSO4 is used for gastrointestinal x-rays because it is opaque to x-rays.  The drink given is actually a suspension, with solid BaSO4 suspended in the solution, so the solution is saturated.  KSP for this compound is 1.10 x 10-10.  (a) What is the concentration of Ba2+ in a saturated solution of BaSO4?                 (b)  Given the toxicity of Ba2+ ions, why do you think magnesium sulfate is added to the drink?  Hint:  What would the presence of more sulfate ions do to the amount of dissolved Ba2+ in the solution?  Think Le Chatelier’s Principle! Note:  sulfate ions are called “common ions” here.            (c)  Suppose you start with the saturated solution of BaSO4 from part (a) of this problem.  Now, figure out what the solubility of BaSO4 becomes if enough MgSO4 is added to the solution to make it 0.10 M in…

What is the solubility of PbF₂ in a solution that contains 0.0700 M F⁻ ions? (Ksp of PbF₂ is 3.60 × 10⁻⁸)

The formation constant* of [M(CN)2]¯ is 5.30 × 1018, where M is a generic metal. A 0.150 mole quantity of M(NO3) is added to a liter of 0.690 M NaCN solution. What is the concentration of M+ ions at equilibrium? [M2+] = M * TOOLS x10

5. What is the molarity of NaCl in which AgCl has a molar solubility of 2.38 x 10-9 mol /L? The Ksp for Silver Chloride is: 1.83 x 10-10.    Group of answer choices A. 0.0769 b. 7.69 c, 6.34 d, 36.70

Can you explain it step by step?