Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003 M, [CO3 2−] = 0.003 M (b) Co(OH)2: [Co2+] = 0.01 M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01 M, [HPO4 2−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01 M, [PO4 3−] = 1 × 10–13 M
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix...
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003M, [CO32−] = 0.003M (b) Co(OH)2: [Co2+] = 0.01M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01M, [HPO42−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01M, [PO43−]= 1 × 10–13 M
Question 12 The following compounds precipitates from a solution with the concentrations indicated. Ag2S: [Ag+] = 1 10-10M, [S2-) = 1 x 10-13M True False
D2. (8 pts) Determine whether the following compound precipitates from a solution that has the concentrations indicated. [Pb"+-0.0030 M, [1] Pbl2 (s)Pb2 (aq) 2 I (aq) 1.3 x 10" M Kip8.7 x 10
Which of the following compounds has the highest molar solubility? A. PbS; Ksp = 8.4 x 10-28 B. PbSO4; Ksp = 1.8 x 10-8 C. PbCO3; Ksp = 1.5 x 10-13 D. PbI2; Ksp = 8.7 x 10-9 E. Pb3(PO4)2; Ksp = 3.0 x 10-44
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (a) AgBr: [Ag+] = 5.7 × 10^-7 M, [Br–] = 5.7 × 10^-7 M (b) CaCO3: [Ca^2+] = 5.3 × 10^-3 M, [CO3^2−] = 9.0 × 10^-7 M (c) PbF2: [Pb^2+] = 2.1 × 10^-3 M, [F–] = 4.2 × 10^-3 M (d) Ag2CrO4: [Ag+] = 5.3 × 10^-5 M, 3.2...
please andwer all qeustions (24) Ag2 S (s) has the solubility equilibrium in water solution: Ag2 S (s) 22 Ag+ (aq) + S2- (aq) Which is the correct expression for Ksp of Ag2 S ? (a) Ksp = 2 [Ag 1? [S2-1 (b) Kyp = [Ag+] [S?) (C) Kop = [Ag 1824 (d) Ksp = [[Ag 7? + [5243 (25) When dissolving slightly soluble CaCO3 (s) in water, a solubility equilibrium is reached, with (Ca2+] = [CO3 2-1 = 5.3...
2. Which compound has the highest molar solubility in neutral aqueous solution? (A) ZnS. Ksp-3x10-23 (B) Agl, Ksp 8.52x10-17 (C) BaCO, Ksp 2.58x10 ) Fe(OH)3, Ksp-2.79x10-39 (E) Pblz, Ksp 8.7x10 3. A solution contains 0.01 M Pb2+ and 0.01 M Agt What happens when Na SO(s) is added to bring SO1 to 0.01 M? (Kp(PbSO.)-1.6x10-8. Ksp(Ag SO4) 4x10.) Neither PbSO4 nor Ag SO4 precipitate (B) Both PbSO4 and Ag SO4 precipitate (C) AgaSO4 selectively precipitates. (D) PbSO4 selectively precipitates. 4....
What is the concentration of Co(OH)2(aq) in a solution in which the concentrations of Co2+ and OH® are fixed at 3.9 x 10-5 M? The cumulative formation constant (B2) for Co(OH)2(aq) in water is 1.6 x 109. (CO(OH)2) = M
1. A solution contains 8.68×10-3 M sodium hydroxide and 6.04×10-3 M ammonium sulfide. Solid manganese(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of manganese(II) ion when this precipitation first begins? [Mn2+] = M 2. A solution contains 5.04×10-3 M magnesium nitrate and 1.31×10-2 M nickel(II) acetate. Solid sodium hydroxide is added slowly to this mixture. A. What is the formula of...
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find Kedata in the ALEKS Data tab. Does solubility change with highest solubility compound pH = 6 pH 5 yes ka Ni(OH), ooloo A CN 3 To Data Formula Ksp BaCro4 1.17x10-10 BaSO4 1.08x10-10 CaCO3 3.36x10-9 CaF2 3.45x10-11 Co(OH) 5.92x10-15 CuBr 6.27x10-9 CuCO3 1.4x10-10 Fe(OH)2 4.87x10-17 PbCO3...