PRINCIPLES OF MODERN CHEMISTRY-OWLV2
8th Edition
ISBN: 9781305271609
Author: OXTOBY
Publisher: CENGAGE L
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Calculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution with 0.0.00010 M CN–.
The equilibrium-constant expression for the reaction
Ti (s) + 2CI 2 (g) TICI 4 (1)
is given by
O [Ti (s)] [Cl2 (g)F
[TIC14(1}]
[TIC14 (1)]
[Ti (s)] [Cl2( g))?
[TIC14 (1)]
[Ti (s)] [Cl2 (g)]
O [TIC14 (1)]
[Cl2 (g))?
O [Cl2 (g)]2
For [Co(NH3)6]3+ , Kf has a value of 5.00 × 1031. Calculate the concentration of free, uncomplexed Co3+ ions in a solution that contains a total of 0.160 mol/L cobalt III ions and an equilibrium concentration of 0.50 M NH3.
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- What is the concentration of [Cd2+ (aq)] in a solution made by dissolving 0.020 mol of Cd(NO3)2 in 400 mL of a solution of KCN that is 0.50 M at equilibrium? Kf of [Cd(CN)4]2− = 3.0 × 1018arrow_forwardA concentrated ammonia solution is added to a 0.010 M Ni(No3)2 to solution. Given the equilibrium concentration of ammonia [NH3] to is 0.20 M, determine the nickel (II) ion concentration. The formation constant Kf of the complex Ni(NH3)6^2+ + is 1.2 x 10^9. Assume the volume change from the addition of ammonia solution is negligible.[No^2+]=arrow_forwardConsider the following tetrahedral complex ions: [Zr(H₂O)4]²+, [Zr(CN)4]²¯, and [Zr(OH)4]². Arrange these in terms of increasing wavelength of the color they appear. [Zr(OH)4]²- < [Zr(CN)4]² < [Zr(H₂O)4]²+ O [Zr(CN)4]²- < [Zr(OH)4]²¯ < [Zr(H₂O)4]²+ [Zr(CN)4]² < [Zr(H₂O)4]²+ < [Zr(OH)4]²- O [Zr(H₂O)4]²+ < [Zr(CN)4]²¯ < [Zr(OH)4]²- [Zr(OH)4]² < [Zr(H₂O)4]²+ < [Zr(CN)4]²-arrow_forward
- [Fe(H2O)6]3+ (aq) + SCN1- ↔ Fe(H2O)5SCN]2+(aq) + heat yellow red For the above reaction, describe using Le Chatelier’s Principle what changes (color changes and shifts) would occur when each stress is applied to this equilibrium. Explain your answers. a) Add KSCN(aq) b) Decrease temperature c) Add AgNO3, which causes AgSCN to precipitate out.arrow_forwardFor the aqueous complex at Fe (CN)6]4-complex Kf= 1.0 x 10^35 Suppose equal volumes of 0.0062M Fe(NO2) solution and 0.10M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe^2+ ion. Round your answer to 2 significant digits.arrow_forwardCobalt(II) complex ion solution: [Co(H2O)6]+2(aq) + 4Cl-(aq) [CoCl4]-2(aq) + 6H2O(l) Pink Blue 1). When silver nitrate is added the blue color becomes pink. Why is that ? 2. When heat is added , in which direction the equilibrium will shift ? Is this reaction exothermic or endothermic ? 3.What happens when the temperature is lowered in the ice bath ?arrow_forward
- What is the theoretical percentage by weight of Cr in K[Cr(C2O4)2(H2O)2]·2H2Oarrow_forwardIn the presence of aqueous ammonia, cobalt(III) forms the complex ion Co(NH3)63+. Determine the molar concentration of free cobalt(III) ion in solution when 0.210 mole of Co(NO3)3 is dissolved in a liter of 2.50 M aqueous ammonia.arrow_forward(a) Draw a Lewis dot and cross structure (including any lone pairs) for a NBr3 molecule and determine the shape of the molecule and number of valence electrons. (b) Six ammonia ligands form a complex ion with Co²+. What is the overall charge of the complex ion? Write the formula for the complex ion. What is the coordination number of the complex ion? Explain how ammonia ligands form a complex ion with Co²+? What is the geometry of the complex ion? Would you expect the complex to be coloured? Explain why? i. ii. iii. iv. V. vi.arrow_forward
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