15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a....
Question 1 1 pts The Ksp value for BaSO4 Ksp = 1.1 x 10 10. If 50.0 mL of 2.0 x 10-4 M Ba(NO3)2 is mixed with 350.0 mL of 1.0 x 10-5 M Na2SO4, will a precipitate be observed? A precipitate forms because the ion pair product, Q> Ksp A precipitate forms because the ion pair product, Q< Ksp. No precipitate forms because the ion pair product, Q = Ksp No precipitate forms because the ion pair product, Q<Ksp...
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C. 2. Calculate the molar solubility of CaF2 (Ksp = 4.0 x 10-11) in a 0.025 M NaF solution. 3. Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in both Ba2+ and Pb2+ until [SO42-] reaches 1.0 x 10-4 M. Would either BaSO4 (Ksp = 1.1 x 10-10) or PbSO4 (Kop -1.7 x 10-8) precipitate under...
D Question 4 5 pts 2b) There are 0.10 moles of N2O4 and 0.20 moles of NO 2 present in a 2.0 L container which may react according to: N2O4(g) = 2N028) Kp = 11 What is the value of Qp for the initial gas mixture? a. 4.0 b. 0.20 c. 0.40 d.5.0 . a. b. Consider the following equilibrium systems. Which direction will the reactions shift (reactants or products) when cooled? 200g + O2(g) = 2CO2(g) H2e+12(e)=2HI® H2(g) +126)...
QUESTION 2 Kep(Ag2CrO4) = 9,0 x 10-12, Ksp(BaSO4) = 1.1 x 10-10, Ksp (AgSCN) - 1.2 x 10-12 What is the correct order of the solubility of the above ionic compounds? (from smallest to greatest) a. BaSO4 → AgSCN → Ag2C+04 b. AgSCN → Ag2CrO4 → BaSO4 c. AgSCN → BaSO4 → Ag2C104 d. No correct order is found. e. BaSO4 → Ag2Cr04 → AgSCN
The Ksp for BaSO4 is 1.1 x 10^-10 and that for BaSeO4 is 2.8 x 10^-11. What concentration of [SO4]^-2 and [SeO4]^-2 are needed to precipitate out each salt? Which will precipitate first?
QUESTION 13 1 points Save Answer What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 x 10-19) in 0.0100 M Na2SO4 solution? ОА. 1.1 x 10-8 ОВ. 1.1 x 10-4 Ос. 1.1 x 10-7 OD. 1.1 x 10-5 ОЕ. 1.1 x 10-6
Calculate the solubility of BaSO4 (a) in pure water and (b) in a solution in which [SO42-) = 0.285 M. Ksp (BaSO4) = 1.1 x 10-10 Solubility in pure water = Solubility in 0.285 M ,2- - D M Submit Show Approach Show Tutor Steps
Question 5 10 points Determine the water solubility of Cul(s) (Ksp = 1.1 x 10-12) 1- 1- Ksp - S2, S-(Ksp)1/2, S = 1.05 x 10-6 M 2- 2- Ksp = 453, S = (Ksp/4)1/3, S = 6.5 x 10-5 M 3- 3- Ksp = 25, S = (Ksp/2). S = 5.5 x 10-13 M
using debye-huckel limiting law (b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions in aqueous solutions containing 1.2 x 10-3 mol kg of (i) Sucrose (you may assume this mixture is ideal) (ii) potassium nitrate (KNO3) (ii) copper sulphate (CuSO4). A 0.509 mol-1/2 kg 1/2) (b) Given that the solubility product Ksp of barium sulphate (BaSO4) is 1.1 x10-10 (mol kg-1)2, calculate the concentration of barium ions...
A saturated solution of BaSO4 is made by dissolving excess solid BaSO4 in a 1 L solution of 0.20 M Na2SO4. How many grams of BaSO4 will dissolve in the 1.0 L volume? Assume the volume does not change when the solid is added. Ksp = 1.1 x 10-10. (A) 2. 85 x 10-7 (B) 2. 93 x 10-7 (C) 3.02 x 10-7 (D) 3. 18 x 10-7 (E) 1.28 x 10-7 Submit