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
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+] = 0.003 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
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
3. Tooth enamel consists of the mineral hydroxyapatite, Cas(PO4)3OH, which has Ksp = 6.8 x 10-37. a. (10 points) Fill the in the ICE Box for the equilibrium of hydroxyapatite in water. You may use "x" or "S" for the changes. Cas(PO4)2OH(s) = 5 Ca2+ (aq) + 3 PO43- (aq) + OH- (aq) Initial Change Equilibrium b. (10 points) Write an expression for Ksp in terms of the concentrations of product. C. (10 points) Calculate the solubility of hydroxyapatite in...
in the table below, predict which of the following reactant combinations will produce precipitates and write all the products that form (including states of matters- l, s, aq, g; write "ss" if it is slightly soluble). Useful information is also below. TABLE 4.1 | Simple Rules for the Solubility of Salts in Water 1. Most nitrate (NO3-) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cst, Rb+) and the ammonium ion (NH4+) are soluble....
in the table below, predict which of the following reactant combinations will produce precipitates and write all the products that form (including states of matters- l, s, aq, g; write "ss" if it is slightly soluble). Useful information is also below. TABLE 4.1 | Simple Rules for the Solubility of Salts in Water 1. Most nitrate (NO3-) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cst, Rb+) and the ammonium ion (NH4+) are soluble....
in the table below, predict which of the following reactant combinations will produce precipitates and write all the products that form (including states of matters- l, s, aq, g; write "ss" if it is slightly soluble). Useful information is also below. TABLE 4.1 | Simple Rules for the Solubility of Salts in Water 1. Most nitrate (NO3-) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cst, Rb+) and the ammonium ion (NH4+) are soluble....
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
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...