Mercury (II) bromide is a sparingly soluble salt.
HgBr2(s) ↔ Hg2+(aq) + 2Br-(aq)
At 25 ℃ the concentration mercury ion in a saturated solultion is 2.49 x 10-7 M. What is it’s value of Ksp at 25℃?
Mercury (II) bromide is a sparingly soluble salt. HgBr2(s) ↔ Hg2+(aq) + 2Br-(aq) At 25 ℃...
4.2 x 10-3 4. Magnesium fluoride (MgF,) is a sparingly soluble salt. It has Kp = 7.4 x 10-9. Calculate the concentration of fluoride ion in a saturated solution of MgF2.
6. Enough of a sparingly soluble salt AB(s) dissolved in a certain amount of water to bring it into equilibrium with the ions A" (aq) and B (aq). If the equilibrium concentration of A*? is 4.9 x 10 mol kg"', and the Debye Hückel Limiting Law (DHLL) is obeyed at this concentration, K sp for the salt is: A) 2.11e-9 B) 4.90e-9 C) 4.86e-10 D) 8.46e-9 E) 3.91e-10
Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 1.94 x 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 6.24 x 10-6 M. (a) What is the concentration of chloride ions, [CI – ], in the resulting solution? XM (b) What is the molar solubility of silver chloride, AgCl, in 1.94 x 10-5 M NaCl? 4.9 6.24e-6...
Lead(II) sulfate, PbSO4 (s), dissociates into the ions, Pb+2(aq) and SO4 -2 (aq) as shown: PbSO4 (s) ↔ Pb+2 (aq) + SO4 −2 (aq) Given that Ksp is 2.53 × 10−8 for PbSO4 (s), what is the ion concentration of lead ions and sulfate ions in a saturated lead sulfate solution?
Question 6 (Extra Credit Challenge): When the sparingly soluble salt lead fluoride, PbF2, is added to an acidic solution with [H+] = 1.6 x 10–4 M, the resulting concentration of [Pb2+] after the salt dissolves is determined to be 7.75 x 10–5 M. (a) Determine the equilibrium constant for the dissolving of PbF2 in an acidic solution of H3O+ and (b) given Ka = 6.8 x 10–4, use the value determined in part a to calculate the Ksp for PbF2...
At 25 °C, only 0.0450 mol of the generic salt AB is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB(s) 7 A+ (aq) +B+ (aq) Ksp = At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.18. What is the Ksp of the salt at 22 °C? ot a generic metal hydroxide, M(OH), is mixed...
1) For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.5 mL of 0.070 M lead nitrate is added to 19 mL of 0.018 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms. 2) Sodium phosphate is added to a solution that contains 0.0041 M aluminum nitrate and 0.028 M calcium chloride. The concentration of the first ion to...
Having a tough time. 1. What is the molar solubility of Mg3(PO4)2 in a 0.860 M solution of sodium phosphate? The Ksp for Mg3(PO4)2 = 1.04 x 10-24 M 2. What is the molar solubility of Ag2SO4 in a 0.950 M solution of Al2(SO4)3? The Ksp for Ag2SO4 = 1.20 x 10-5 1.33e-5 x M 3. Select all of the following that are true about the common ion effect for dissolving solids. If you add potassium sulfate to a saturated...
Calcium sulfate is only sparingly soluble. CaSO4(s) ⇌ Ca2+(aq) + SO42-(aq) For this type of dissolution reaction the equilibrium constant, also known as the solubility product, is denoted Ks. In the reaction above, Ks = 8.8 x 10-6. When an excess of the solid is dissolved in water what is the maximum concentration of Ca2+(aq) in mol L-1? (Give your answer to at least TWO significant figures and do not include the units in the answer box. Hint: to help...
An insoluble salt, MX2, dissociates slightly in water, MX2(s) + M2+ (aq) + 2X-(aq); Ksp = 9.5 x 10-14 at 25 oC. Calculate AG for the dissociation reaction when the concentration of ions are: [M2+] = 6.4 x 10-2 M and {X-} = 9.4 x 10-5 M.