A solution was prepared in the lab when equal volumes of 3.00 x 10-4 M calcium chloride and 1.00 × 10-4 M lithium phosphate were combined. Will a precipitate form? A solution was prepared in the lab when equal volumes of calcium chloride and lithium phosphate were combined. Write the formula for the calcium phosphate salt.

A solution was prepared in the lab when equal volumes of 3.00 x 10-4 M calcium chloride and 1.00 × 10-4 M lithium phosphate were combined. Will a precipitate form? A solution was prepared in the lab when equal volumes of calcium chloride and lithium phosphate were combined. Write the formula for the calcium phosphate salt.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 64QAP

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The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.
If 50.0 mL of a 0.0010 M CaCl2 solution were added to 50.0 mL of 0.010 M Na2SO4 solution, would a precipitate of CaSO4 form? The Ksp of CaSO4 at 25oC is 2.4 × 10-5
The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?
A solution is prepared by dissolving 1.40 g of silver sulfate in 100 mL of hot water. Will a precipitate form if the solution is cooled to 25oC? Assume that a negligible change in volume occurs during the operations. (Ksp = 1.2 x 10-5).
Consider a solution that is made from mixing 122.3ml of 0.333M ZnCl2 and 83.57ml of 0.654M Na2CO3 a. What is the concentration of cations and anions at equilibrium(in molarity)? Use x-is-small approximation. b. What is the ‘net’ amount of precipitate produced(in moles)? ksp (ZNCO3) = 1 x 10^-10
25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?
A solution of NaF is added dropwise to a solution that is 0.0144M in Ba2+. When the concentration of F- exceeds ____M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp=1.7•10-6
The Ksp of strontium phosphate Sr₃(PO₄)₂ is 1.2× 10⁻³¹. At what molarity of SrCl₂ will you just start to precipitate the phosphate from a solution that has a phosphate concentration of 6.4× 10⁻⁴ M?
A solution is prepared such that Li3+=3.0×10-3 M while PO43-=2.0×10-3 M. If the Ksp of Li3PO4 is 2.37×10-11, will a precipitate form in the prepared solution? Show your complete solution.
The molar solubility of Ca3(PO4)2 is 1.14×10-7 mol/L at 25°C. Calculate the solubility of Ca3(PO4)2 at 25°C in g/L and Calculate Ksp at 25°C.
Will a precipitate form when 75ml of 0.20 M AgNo3 are combined with 266 mL of 0.050 M NaCl? The Ksp for AgCl=1.8 x 10^-10. ( Report Qsp)
At 25 °C, for Lead (II) sulphate (PbSO4), Ksp = 2.53×10-8 and for Barium sulphate (BaSO4) Ksp = 1.08×10-10. Suppose that Na2SO4 is added gradually to 500 mL of a solution that contains both Pb2+ ion and Ba2+ ion. (i) What will the Ba2+ concentration be (in mol/l) when Pb just begins to precipitate if the initial solution contains 0.40 M Pb2+ and 0.52 M Ba2+? (ii) What percentage of the strontium ion has precipitated when PbSO4 just begins to precipitate if the initial solution contains 0.28 M Pb2+ and 0.32 M Ba2+?

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