Calculate the final concentrations ofK* (aq),C20,2- (ag),Ba?+ (aq) andBr (aq) in a solution prepared by adding 0.100 L of 0.190 MK2C204 to 0.260 L of 0.320 MВаBr2. (ForBaC204, Ksp = 2.3 x 10-8.)Concentration of Kt(aq)Concentration of C2042- (aq) =Concentration of Ba2+ (aq) =MConcentration of Br (aq) =Submit AnswerRetry Entire Group

Given: The volume of K2C2O4 is 0.100 L The molarity of K2C2O4 is 0.190 M The volume of BaBr2 is…

Calculate the final concentrations of K (ag), C20,2- (aq), Ba+ (aq) and Br (aq) in a solution prepared by adding 0.100 L of 0.190 M K2C204 to 0.260 L of 0.320 M BaBr2. (For BaC204, Kp = 2.3 x 10-8.) %3D Concentration of Kt(aq) = M Concentration of C20,2- (aq) = Concentration of Ba2+ (aq) = Concentration of Br (aq) = Σ

Calculate the final concentrations of K (ag), C20,2- (aq), Ba+ (aq) and Br (aq) in a solution prepared by adding 0.100 L of 0.190 M K2C204 to 0.260 L of 0.320 M BaBr2. (For BaC204, Kp = 2.3 x 10-8.) %3D Concentration of Kt(aq) = M Concentration of C20,2- (aq) = Concentration of Ba2+ (aq) = Concentration of Br (aq) = Σ

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...

See similar textbooks

Similar questions

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Ksp for PbCl2(s) is 1.6 x 10-³. If you mix 200.0 mL of 0.010 M Pb(NO3)2(aq) with 400.0 mL of 0.010 M NaCI(aq), then sodium nitrate will precipitate. the concentration of CI will be 0.0033 M. no precipitate will form. PbCl2(s) will precipitate.
The Ksp value for Calcium Phosphate [Ca3(PO4)2] is 1.00 x 10-26 so calculate themolar solubility in units of grams per liter of calcium ions [Ca2+(aq)] if a chemist only made 2.198 Liters. What would the new molar solubility in grams per liter of calcium ions [Ca2+(aq)] be if the chemist added 0.129 M of Calcium Sulfate [CaSO4] to the solution? Calculate the ion products (Q) for Calcium Phosphate [Ca3(PO4)2] after the addition of the 0.129 M of Calcium Sulfate [CaSO4] to the solution. Determine if the reaction will shift to the right (no precipitate will form), shift to the left (a precipitate will form), or is at equilibrium
5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)
Calculate the final concentrations of K* (aq), C20,2- (aq), Ba?+ (aq) and Br (ag) in a solution prepared by adding 0.100 L of 0.170 M K2C2O, to 0.280 L of 0.220 M ВаBrz. (For BaC204, Kp = 2.3 x 10-8.) Concentration of K* (aq) M Concentration of C20,2- (aq) M Concentration of Ba?+ (aq) M Concentration of Br (aq) M
The solubility-product constant for Ce(IO3)3 is 3.2 X 10-10. What is the Ce3+ concentration in asolution prepared by mixing 50.0 mL of 0.0250 M Ce3+ with 50.00 mL of
The Ksp of Cu3 (PO4), is 1.00 × 10-37. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of K3PO4 , how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
Calculate the solubility in grams per liter of Pb(IO3)2 (s) in 0.10 M KIO3 (aq) at 25 °C. The Ksp for Pb(103)2 (s) is 3.7 × 10-13 at this temperature. Answer:
The solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass of KCl(s) must be dissolved in 150.00 mL of 1.15M Pb(NO3)2 to produce a solution that is just saturated in PbCl2?
2a Suppose the Gapon constant K =([Ca ] X/([Cd ]X.) is 25. Also suppose that your soil has equilibrated with a large mass of contaminated water with a [Ca ] of 0.1 millimoles per liter and a [Cd ] of 0.025 millimoles per liter. What is the X/X. in the soil? 2b. Suppose the CEC of the soil is 0.3 milliequvalents per kilogram and assume that the only two cations attached to the soil particles are Ca and Cd What is the total amount of Cd attached to a kilogram of soil. 2c. Suppose that an area of soil 300 meters long, 200 meters wide and 2 meters deep with a density of 1800 kilograms per cubic meter has been contaminated with this water. What is the total mass of Cd in this soil?
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.3172-g sample is dissolved in 50 mL of water and titrated to the Ag,CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.