(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_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_forwardThe 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_forward
- a. Using the Ksp value for Cu(OH)2 (1.6 1019) and the overall formation constant for Cu(NH3)42+ (1.0 1013), calculate the value for the equilibrium constant for the following reaction: Cu(OH)2(s)+4NH3(aq)Cu(NH3)42+(aq)+2OH(aq) b. Use the value of the equilibrium constant you calculated in part a to calculate the solubility (in mol/L) of Cu(OH)2 in 5.0 M NH3. In 5.0 M NH3 the concentration of OH is 0.0095 M.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_forwardThe salt MX has a solubility of 3.17 108 mol/L in a solution with pH = 0.000. If K4 for HX is 1.00 1015, calculate the Ksp value for MX.arrow_forward
- Two 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_forwardA 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_forwardSolid Pbl2 (Ksp = 9.8 109) is placed in a beaker of water. After a period of time, the lead(II) concentration is measured and found to be 1.1 103 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more Pbl2 dissolve?arrow_forward
- The solubility of zinc oxalate, ZnC2O4, in 0.0150 M ammonia is 3.6 104 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for zinc oxalate is 1.5 109, what must be the zinc-ion concentration in the solution? Now calculate the formation constant for the complex ion Zn(NH3)42+.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
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