Chapter 15.docx - Chapter 15B A particular saturated...

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Chapter 15B A particular saturated solution of Ca3(PO4)2 has [Ca2+] = [PO3-4] =2.9x10-7M Part A What is the value of Ksp for Ca3(PO4)2? [Ca 2+ ]^3 * [PO 4 3- ]^2 = Ksp Ksp= [2.9*10 -7 ] 5 Ksp= 2.05*10 -33 Part B What is [Ca2+] in a saturated solution of Ca3(PO4)2 that has [PO3-4]= 1.1*10^-2 M? [Ca 2+ ]= 3 Ksp [ PO 4 3 ] 2 = 2.57*10 -10 M Part C What is [PO3-4] in a saturated solution that has [Ca2+]=1.0x10^-2 M? [PO 4 3- ]= 2 + ¿ Ca ¿ ¿ ¿ 3 ¿ ¿ Ksp ¿ 3 ¿ = 1.27*10 -9 M Express your answer using two significant figures PartA Use the values of Ksp in Appendix C in the textbook to calculate the molar solubility of Ag2CO3. Ksp: 8.4 x 10^-12 AgCO3  2Ag + CO3                   2S + S Ksp= [S][2S] 2 8.4 x 10^-12 = 4S 3
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S = 1.28*10^-4 molar solubility=1.28*10^-4 Part B Use the values of Ksp in Appendix C in the textbook to calculate the molar solubility of MgCO3 Ksp: 6.8 x 10^-6 MgCO3  Mg + CO3                     S + S Ksp= [S][S] 6.8 x 10^-6 = S 2 S= 2.61*10^-3 molar solubility= 2.61*10^-3 Part C Use the values of Ksp in Appendix C in the textbook to calculate the molar solubility of Cu (OH)2
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