Lead chloride, PbCl2, is partially soluble with Ksp of 1.7e-05. a. What is the solubility of lead chloride in pure water? (How many moles of PbCl2 could be completely dissolved in one liter of solution?) Solubility of lead chloride in pure water = moles/L. b. What would its solubility be in 0.0630 M NaCl? (How many moles of PbCl2 could be completely dissolved in 1 L of solution?) Solubility of lead chloride in 0.0630 M NaCl = moles/L. c. The difference in these two results is caused by what is known as the common ion effect. Complete the sentence to state what the common ion effect predicts. The solubility of a salt in a solution containing an ion common to an ion in the salt will be v its solubility in water.

Lead chloride, PbCl2, is partially soluble with Ksp of 1.7e-05. a. What is the solubility of lead chloride in pure water? (How many moles of PbCl2 could be completely dissolved in one liter of solution?) Solubility of lead chloride in pure water = moles/L. b. What would its solubility be in 0.0630 M NaCl? (How many moles of PbCl2 could be completely dissolved in 1 L of solution?) Solubility of lead chloride in 0.0630 M NaCl = moles/L. c. The difference in these two results is caused by what is known as the common ion effect. Complete the sentence to state what the common ion effect predicts. The solubility of a salt in a solution containing an ion common to an ion in the salt will be v its solubility in water.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

One mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will form
The solubility product of silver carbonate (Ag₂CO₃) is 8.46 × 10⁻¹² at 25°C. What is the solubility product expression for silver carbonate? A. Ksp = [Ag⁺] [CO₃²⁻]² B. Ksp = ½ [Ag⁺] [CO₃²⁻] C. Ksp = 2 [Ag⁺] [CO₃²⁻] D. Ksp = [Ag⁺]² [CO₃²⁻]
25
What happens when equal volumes of 2x104 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The K of calcium fluoride, CaF 2, is 4.0x10-11, sp O a. Q K; no precipitate forms c. Q K; a precipitate forms
7. Consider the equilibrium reaction: AX3(s) = A³+(aq) + 3X´(aq). What is the solubility of AX3 (MM = 78.0 g/mol) in mg/L at 25ºC if its Ksp is 1.0 x 10-33?
Please help with Parts 1A 1B and 1 C
11. What minimum mass of NaF must be added to a 1.0 L solution that contains 1.10 x 10- M Ba2* in order to precipitate BaF2? The Ksp for BaF2 is 2.4 x 10
5:23 O13%DE elearning.yu.edu.jo/m O A student was given 2 beakers labeled with numbers 1 and 2, each beaker contains a clear solution. Additionally, he was given two reagent bottles labeled with A and B. Now, he added reagent A to both beakers and he noticed the formation of a precipitate in beaker 2 but not in beaker 1. However, the addition of reagent B to both beakers resulted in the formation of a precipitate in beaker 1 but not in beaker 2. Based on the information, which of the following is correct? a. compound A is the limiting reactant in beaker 1. b. compound B is the limiting reactant in beaker 2. c. compound A is the limiting reactant in beaker 2. d. compound B will be the excess reactant in beaker 1. Question 2
A 100.0 mL mixture is made of water and 1.0 g of silver chloride, AgCl. What does this solution look like, and what mass of silver chloride is in solution? The molar solubility of AgCl = 1.3x10-5, and the molar mass of AgCl = 143.32 g/mol. A.1.9x10-4 (Clump of AgCl undissolved in beaker of water) B. 1.3x10-5 (Clump of AgCl undissolved in beaker of water)
5. If K = 8.1 x 1019 of an MX, type salt, what is its solubility? 6. What is the solubility of TICI) in a 0.0168 M NaCl solution? (Kgp = 1.7 x1 0*)
4. The Ksp for MgCO3 = 1.1 x 101º. CIRCLE the solubility of MgCO3 in pure water. a) 1.1 x 10-10 M b) 1.1 x 108 M c) 1.1 x 107 M d) 1.1 x 106 M e) 1.1 x 10$ M
Calcium sulfide was mixed with lead (II) nitrate, and it formed a precipitate. The precipitate was then separated from the solution. Determine the molar solubility of the precipitate if it has a Ksp value of 3.3x10-10 O O O O O O O 1.8x10-5 M 9.1x10-6 M 4.9x10-6 M 5.3x10-5 M 9.5x10-5 M 3.7x10-5 M 5.1x10-6 M O None of the above