Calcium and magnesium ions can occur in our water supplies (e.g. through rocks and geological formations). A sample of tap water was tested and the calcium ion concentration was measured at 2.1E-5M and the magnesium ion concentration was measured at 1.2E-3M. If carbonate ion is added into the tap water, which ion will precipitate out of solution first? Explain your reasoning. The Ksp values of CaCO3 and MgCO3 are 5.0E-9 and 6.8E-6, respectively.

Calcium and magnesium ions can occur in our water supplies (e.g. through rocks and geological formations). A sample of tap water was tested and the calcium ion concentration was measured at 2.1E-5M and the magnesium ion concentration was measured at 1.2E-3M. If carbonate ion is added into the tap water, which ion will precipitate out of solution first? Explain your reasoning. The Ksp values of CaCO3 and MgCO3 are 5.0E-9 and 6.8E-6, respectively.

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

When 200.0 mL of 5.15 x 10-4 M Ba(NO3)2 is added to 150.0 mL of 8.25 x 10-4 M Na2SO4. Ksp(BaSO4) = 1.08 x 10-10. A precipitate choose your answer.... Ksp because Qsp choose your answer... choose your answer... SIGMA = form
Please use the values in the resources listed below instead of the textbook values. Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a saturated solution of Ce(IO3)4 was found to be 7.35X10 mol/L. Find the Ksp: 4.0 (b) Find the concentration (in M) of iodate ions in a saturated solution of Ra(IO3)2. (Ksp = 1.16X 10-9) 4.0) M
Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively.
The institution decides to add dissolved Al (III) in the form of Al(OH)3 into the water for the water treatment plan. The limit for total Al(III) added is 750 ppb (ug dissolved in Al(III) per L). The Ksp for Al(OH)3 is 3*10^-34. 1. Write the equilibrium expression for this mineral dissolution 2. Do you expect the solubility to increase or decrease with increase ionic strength? 3. Are any of the product of dissolution acids or bases? 4.Would you expect the effective solubility to change with pH? 5. Dossolved oranic matter such as EDTA are good ligand for Al3+, show how you would compute the chane in Al(III) solubility if the lake had a DOM concentration of 0.1 mM
• An unknown acid (HA) was titrated with NaOH(aq). • The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 2. 4 9. 8. 10 12 14 16 18 20 22 24 26 28 30 Volume of Titrant / mL Which of the following net ionic equations explains the pH of the analyte solution before any titrant is added? A (aq) + H20(1) HA(aq) + OH (aq) A (aq) + H3O*(aq) --> HA(aq) + H20(1) O H*(aq) + OH (aq) H20(1) --> O HA(aq) + OH (aq) --> H2O(aq) + A (aq) HA(aq) + H20() H3O*(aq) + A (aq)
2. Teeth and bones are composed, to a first approximation, of calcium phosphate, Ca3(PO4)2(s). The Ksp for this salt is 1.3 x 10-32 at 25 °C. Calculate the concentration of calcium ion in a saturated solution of Ca3(PO4)2 (**tough one**)
Determine the value of Ksp for Cu(10), by constructing an ICE table, writing the solubility constant expression, and solving the expression. The molar solubility of Cu(10), is 2.7 x 10-³ M at this temperature. Complete Parts 1-2 before submitting your answer. NEXT > Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products at this temperature.. Initial (M) Change (M) Equilibrium (M) 4.00 8.1 x 10-³ 0 -2.00 1.5 x 10-5 1 Cu(103)₂(s) 2.7 x 10.³ -1.00 -1.4 x 10.³ -2.7 x 10.³ -4.00 -7.3 x 10.⁰ 11 5.4 x 10-³ 1.4 x 10.³ -2.0 × 10-8 Cu²+ (aq) 2 -5.4 x 10-³ 7.3 x 10-6 + 1.00 2.0 × 10-8 2 10₂(aq) RESET 2.00 9.0 × 10-4
What will be the best precipitating agent for Ba+2 analyte ? (assume precipitating agent will be added in excess) Ksp Barium hydroxide Ba(OH)2 5 x 10-3 Barium sulfate BaSO4 1.1 x 10-10 a. K2SO4b. NH4OHd. KOH
Please don't provide handwritten solution ....
I'm having issues beginning this problem. Could you show me a break down for understanding? Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12×10-12 M3 What is the solubility (in moles per liter) of silver chromate in a 1.20 M potassium chromate aqueous solution? solubility: M What is the solubility (in moles per liter) of silver chromate in a 1.20 M1.20 M silver nitrate aqueous solution? solubility: M What is the solubility (in moles per liter) of silver chromate in pure water? solubility: M
5. A water supply company, One Team, found out that their water supply had been contaminated with a sparingly soluble magnesium salt. They requested the help of Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts: Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51 mL of the same HCl titrant to titrate a 100.0-mL solution. a. What is the molarity of the HCl titrant?…
Show the solution