(a)
Interpretation: The molar solubility of AgBr in pure water needs to be determined, if the
Concept Introduction:
A metal complex can be show as
Usually
(a)
Answer to Problem 103CP
Explanation of Solution
Solid
The solubility product of AgBr can be written as:
Calculate solubility:
(b)
Interpretation: The molar solubility of
Concept Introduction:
A metal complex can be show as
Usually transition metal ions and post transition metal ions forms coordinate complexes with different ligands.
(b)
Answer to Problem 103CP
Explanation of Solution
Add both equation:
_____________________________________________
Calculate ‘s’:
(c)
Interpretation: The calculated solubility values needs to be compared.
Concept Introduction:
A metal complex can be show as
Usually transition metal ions and post transition metal ions forms coordinate complexes with different ligands.
(c)
Answer to Problem 103CP
The presence of
Explanation of Solution
Calculated solubility’s:
The presence of
(d)
Interpretation: The mass of
Concept Introduction:
A metal complex can be show as
Usually transition metal ions and post transition metal ions forms coordinate complexes with different ligands.
(d)
Answer to Problem 103CP
Explanation of Solution
Solubility of
Volume = 250.0 mL = 250.0 x 10-3 L
Molar mass of
Calculate mass of
(e)
Interpretation: The effect of addition of
Concept Introduction:
A metal complex can be show as
Usually transition metal ions and post transition metal ions forms coordinate complexes with different ligands.
(e)
Answer to Problem 103CP
By the addition of
The addition of
Explanation of Solution
By the addition of
The addition of
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Chapter 19 Solutions
Chemical Principles
- What mass of Ca(NO3)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 1011 and Ka for HF = 7.2 104. Assume no volume change on addition of Ca(NO3)2(s).arrow_forwarda. Calculate the molar solubility of AgBr in pure water. Ksp for AgBr is 5.0 1013. b. Calculate the molar solubility of AgBr in 3.0 M NH3. The overall formation constant for Ag(NH3)2+ is 1.7 107, that is, Ag+(aq)+2NH3(aq)Ag(NH3)2+(aq)K=1.7107. c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of AgBr will dissolve in 250.0 mL of 3.0 M NH3? e. What effect does adding HNO3 have on the solubilities calculated in parts a and b?arrow_forwardTwo hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20105, what is the Ksp, value for LQ?arrow_forward
- The solubility of Pb(IO3)2(s) in a 7.2 102-M KIO3 solution is 6.0 109 mol/L. Calculate the Ksp value for Pb(IO3)2(s).arrow_forwardWhich of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) KClO4:[K+]=0.01M,[ClO4]=0.01M (b) K2PtCl6:[K+]=0.01M,[PtCl62]=0.01M (c) PBI2:[Pb2+]=0.003M,[I]=1.3103M (d) Ag2S:[Ag+]=11010M,[S2]=11013Marrow_forward. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.arrow_forward
- A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.arrow_forwardYou place 1.234 g of solid Ca(OH)2 in 1.00 L of pure water at 25 C. The pH of the solution is found to be 12.68. Estimate the value of Ksp for Ca(OH)2.arrow_forwardWhat reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the KSP values given in Appendix J.) (a) Hg22+ and Cu2+. (b) SO42- and Cl-. (c) Hg2+ and CO2+. (d) Zn2+ and Sr2+. (e) Ba2+ and Mg2+. (f) CO32- and OH-arrow_forward
- A saturated solution of silver arsenate, Ag3AsO4, contains 8.5 107 g Ag3AsO4 per mL. Calculate the Ksp of silver arsenate. Assume that there are no other reactions but the Ksp reaction.arrow_forwardUse the following data to calculate the Ksp value for each solid. a. The solubility of Pb3(PO4) is 6.2 1012 mol/L. b. The solubility of Li2CO3 is 7.4 102 mol/L.arrow_forward
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