If a solution containing 0.10 M CI-, Br, I, 4 and CrO2 is treated with Ag+, in what order will the anions precipitate?

27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2

Calculate the amount of precipitate when excess CO2 is bbbled through a solution containing 0.205 mol of Ba(OH)2 according to the equation:  Ba(OH)2 + CO2 --> BaCO3 (MM=197.4g) +H2O (MM=18.02)

An acidic solution is 4 mM in each of the following metal ions: Sn2+, Co2+, Pb2+, Mg2+. see the Solubility Product Constant Table. Please see Separation by Precipitation 2 for assistance. (a) Which of the metals would precipitate as their hydroxides at pH = 6.00? (Select all that apply.) I tin O cobalt O lead O magnesium (b) Which of the metals would precipitate as their hydroxides at pH = 8.00? | tin O cobalt O lead O magnesium (c) At what pH do the metal hydroxides begin to precipitate? Sn(OH), 49 Co(OH)2 49. Pb(OH)2 40) Mg(OH), 49)

7.  The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq)                      (Z) 25.0 mL of 1.0 M CH3COOH(aq)   Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True

Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH,CO,K, with 0.207 M HNO3. What is the pH of the solution after 39.83 mL of the HNO3 has been added? (pK, of CH;CH-COH = 4.691)

Will a precipitate form if 0.1M aqueous solutions of AgNO, and Na,S are mixed? If a precipitate forms, identify 1 the precipitate. +) 00

suppose you have a solution that might contain any or all of the following cations: Cu2+, Ag+, Ba2+, and Mn2+. The addition of HBr cuases a precipitate to from. After the precipitate is separated by filtration, H2SO4 is added to the supernatant liquid, and another precipitate forms. Thsi precipitate is separated bu filtration and a solution of NaOH is added to the supernatant liquid until it si strongly alkaline. No precipitate is fromed.Which ions are present in each of the precipitates? Which cations are not present in the original solution?

Which of the following compounds precipitates from a solution that has the concentrations indicated? (a) KClO4: [K+] = 0.01 M, [ClO4-] = 0.01 M (b) K2PtCl6: [K+] = 0.01 M, [PtCl62-] = 0.01 M (c) PbI2: [Pb2+] = 0.003 M, [I–] = 1.3 x 10–3 M (d) Ag2S: [Ag+] = 1 x 10–10 M, [S2–] = 1 x 10–13 M

When potassium iodide is added to soluble lead iodide at 25 oC, what will happen? PbI2 <=> Pb2+ (aq) + 2 I- (aq)   a. the reaction will become more soluble   b. the equillibrium will shift to the left and precipitate   c. the equilibrium will shift to the right   d. lead iodide will become supersaturated