If the theoretical molar solubility of CaCO3 in pure water at 25°C is 5.7 x 10−5 M, estimate the theoretical molar solubility of CaCO3 in "hard water" containing 2.0 x10−3 M Ca2+ ions. (Hint: what is the Ksp of CaCO3 at 25°C ?)
If the theoretical molar solubility of CaCO3 in pure water at 25°C is 5.7 x 10−5...
14. What is the molar solubility of AgCl in pure water at 25°C? Ksp =1.8 x 10
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...
Calculate the solubility at 25 °C of CuBr in pure water and in a 0.0010 M CoBr, solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: x10 solubility in 0.0010 M CoBry solution: 0 X 5 ?
4) Calculate the molar solubility of AgCl (Ksp = 1.8 x 10-) at 25°C in: (a) Pure water (b) 3.0 M NH3 [Hint: AgCl(s) + 2NH3(aq) Ag(NH3)2(aq) + Cl(aq) K = 3.1 x 10
Determine the molar solubility of AgBr in: Ksp (AgBr) = 7.7 x 10^ -13 a. a solution of pure water b. a solution containing 0.150 M NaBr c. A solution containing 0.25 M NaCL
Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold. Lead thiocyanate has a Ksp value of 2.0*10^-5.
15) Determine the molar solubility of BaF2 in pure water. Ksp for BaF2 = 2.45 x 10-5. A) 1.83 x 10-2 M B) 1.23 x 10-5 M C) 2.90 10-2 M. D) 4.95 x 10-3 M 15) E) 6.13 x 10-6 M
1.17x10-10 Calculate the solubility at 25 °C of BaCrO, in pure water and in a 0.0180 M BaCl, solution. Yo Round both of your answers to 2 significant digits solubility in pure water: L x10 solubility in 0.0180 M BaCl) solution: ? X
5. a) Determine the molar solubility of PbSO4 in pure water, Ksp (PbSO4) = 1.82 * 10-8 b) A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. Calculate the value for the process. Will a precipitate of AgCl form? Give evidence to support your claim. Ksp (AgCl) = 1.77 10-10
15. Put the following compounds in order of increasing molar solubility in pure water at 25°C. 1. CaF2 Ksp = 3.45x10-11 II. SrCo, Ksp = 5.6x10-10 III. Ag200, Ksp = 8.46x10-12