For the following questions, identify the ions comprising the salt, and then use the expression for the solubility product to perform the necessary calculations. Thissimple exercise involves the assumptions that you can ignore any complications which might result as a consequence of the basicity or acidity of the ions, ion pairing,complex ion formation, or auto-ionization of water.Calculate the concentration, in mol/L, of a saturated aqueous solution of Ca5(PO4)3OH (Ksp = 6.80x10-37).mol/LCalculate the solubility, in g/100mL, of Cas(PO4)3OH.g/100mLCalculate the mass of PbSO4 (Ksp = 1.30x10-8) which will dissolve in 100 ml of water.Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume.(The most soluble gets rank 1, the least soluble gets rank 5.)(Ksp = 6.80x10-37)O Ba3(PO4)2 (Ksp = 6.00×10-39)(Ksp = 1.40x10-8)(Ksp = 1.30x10-8)(Ksp = 1.80x10-18)O Cas(PO4)3OHO PbI2O PbSO48 A93PO4

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Calculate the concentration, in mol/L, of a saturated aqueous solution of Cas(PO4)3OH (Ksp = 6.80×10-37). mol/L Calculate the solubility, in g/100mL, of Cas(PO4)3OH. g/100mL Calculate the mass of PbSO4 (Ksp = 1.30x10-8) which will dissolve in 100 ml of water. Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume. (The most soluble gets rank 1, the least soluble gets rank 5.) 8 Cas(PO4)30H O Ba3(PO4)2 (Ksp = 6.00×10-39) O Pbl2 (Ksp = 6.80x1037) (Ksp = 1.40x10-8) O PbSO4 (Ksp = 1.30x10-8) O A93PO4 (Ksp = 1.80×10-18)

Calculate the concentration, in mol/L, of a saturated aqueous solution of Cas(PO4)3OH (Ksp = 6.80×10-37). mol/L Calculate the solubility, in g/100mL, of Cas(PO4)3OH. g/100mL Calculate the mass of PbSO4 (Ksp = 1.30x10-8) which will dissolve in 100 ml of water. Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume. (The most soluble gets rank 1, the least soluble gets rank 5.) 8 Cas(PO4)30H O Ba3(PO4)2 (Ksp = 6.00×10-39) O Pbl2 (Ksp = 6.80x1037) (Ksp = 1.40x10-8) O PbSO4 (Ksp = 1.30x10-8) O A93PO4 (Ksp = 1.80×10-18)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 81QRT

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For the following questions, identify the ions comprising the salt, and then use the expression for the solubility product to perform the necessary calculations. This simple exercise involves the assumptions that you can ignore any complications which might result as a consequence of the basicity or acidity of the ions, ion pairing, complex ion formation, or auto-ionization of water. (a) Calculate the concentration, in mol/L, of a saturated aqueous solution of Ag3PO4 (Ksp = 1.80×10-18). (b)Calculate the solubility, in g/100mL, of Ag3PO4. (c) Calculate the mass of Ca5(PO4)3F (Ksp = 1.00×10-60) which will dissolve in 100 ml of water. (d) Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume.(The most soluble gets rank 1, the least soluble gets rank 5.) 1 2 3 4 5 Hg2I2 (Ksp = 4.50×10-29; Note: The cation is Hg22+) 1 2 3 4 5 Pb3(PO4)2 (Ksp = 1.00×10-54) 1 2 3 4 5 AgI (Ksp = 1.50×10-16) 1 2 3 4 5 Ca5(PO4)3F (Ksp =…
For the following questions, identify the ions comprising the salt, and then use the expression for the solubility product to perform the necessary calculations. This simple exercise involves the assumptions that you can ignore any complications which might result as a consequence of the basicity or acidity of the ions, ion pairing, complex ion formation, or auto-ionization of water. (a) Calculate the concentration, in mol/L, of a saturated aqueous solution of Ag3PO4 (Ksp = 1.80×10-18). (b) Calculate the solubility, in g/100mL, of Ag3PO4. (c) Calculate the mass of Ca5(PO4)3F (Ksp = 1.00×10-60) which will dissolve in 100 ml of water. (d) Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume.(The most soluble gets rank 1, the least soluble gets rank 5.) Hg2I2 (Ksp = 4.50×10-29; Note: The cation is Hg22+) Pb3(PO4)2 (Ksp = 1.00×10-54) AgI (Ksp = 1.50×10-16) Ca5(PO4)3F (Ksp = 1.00×10-60) Ag3PO4 (Ksp = 1.80×10-18)
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hello, i know part a but i need help with part b and c 1a) For the following questions, identify the ions comprising the salt, and then use the expression for the solubility product to perform the necessary calculations. This simple exercise involves the assumptions that you can ignore any complications which might result as a consequence of the basicity or acidity of the ions, ion pairing, complex ion formation, or auto-ionization of water. Calculate the concentration, in mol/L, of a saturated aqueous solution of PbSO4 (Ksp = 1.30×10-8). The answer to this is 1.14×10-4 mol/L 1b) Calculate the solubility, in g/100mL, of PbSO4. 1c) Calculate the mass of Ag3PO4 (Ksp = 1.80×10-18) which will dissolve in 100 ml of water. please quickly help me with part b and c
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