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Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
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Chapter 18, Problem 29E
Interpretation Introduction
Interpretation:
The direction of the equilibrium for
Concept Introduction:
The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their
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Students have asked these similar questions
Calculate the equilibrium constant Kc for the net reaction shown below.
AgCl (s) ⇌ Ag+ (aq) + Cl− (aq) Ksp = 1.6 x 10-10
Ag+ (aq) + 2 NH3 (aq) ⇌ Ag(NH3)2+ (aq) Kf = 1.5 x 107
AgCl (s) + 2 NH3 (aq) ⇌ Ag(NH3)2+ (aq) + Cl− (aq) Kc = ?
Using net reaction, determine the molar solubility of silver iodide in 1.0 M NH3.
a Using the
Kp value for
Cu(OH)2(
1.6 x 10-10) and the overall formation constant for
Cu(NH3)4²+
1.0 x 1013), calculate the value for the equilibrium constant for the following reaction:
Cu(OH)2()+4NH, (aq) Cu(NHs)
2+
(aq) + 20H (aq)
K: = 1.6x10^-6
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 4.8 M NH3. In 4.8 M NH3 the
concentration of OH is 0.0093 M.
Solubility
mol/L
Cobalt(ll) chloride can form two complexes when dissolved in water [Co(H 2 O) 6 )^ 2 + (aq) which is pink in colour, and [CoCl 4 ]^ 2- (ac) which is blue.
The equilibrium system [CO(H 2 O) 6 ]^ 2 +(aq)(pink)+4 Cl^ - (aq) doubleheaded arrow [CoCl 4 )^ 2- (aq)(blue)+ 6H 2 O(l)
(a) Describe how the system and its colour will change in each of the following situations
(I) HCL is added
(II) water is added
(III) AgNO 3 is added
if an aqueous solution of cobalt(II)chloride placed in a hot water bath at 90 Celsius,the solution will turn blue . If the solution is placed in an ice salt mixture , it will turn pink. Is the reaction as written above exothermic or endothermic ? Explain your reasoning
Chapter 18 Solutions
Introductory Chemistry: An Active Learning Approach
Ch. 18 - Prob. 1ECh. 18 - Prob. 2ECh. 18 - Prob. 3ECh. 18 - Prob. 4ECh. 18 - Prob. 5ECh. 18 - Prob. 6ECh. 18 - Prob. 7ECh. 18 - Prob. 8ECh. 18 - Prob. 9ECh. 18 - Prob. 10E
Ch. 18 - Prob. 11ECh. 18 - Prob. 12ECh. 18 - Prob. 13ECh. 18 - Prob. 14ECh. 18 - Prob. 15ECh. 18 - Prob. 16ECh. 18 - Prob. 17ECh. 18 - Prob. 18ECh. 18 - Prob. 19ECh. 18 - Prob. 20ECh. 18 - Prob. 21ECh. 18 - Prob. 22ECh. 18 - Prob. 23ECh. 18 - Prob. 24ECh. 18 - Prob. 25ECh. 18 - Consider the following system at equilibrium at...Ch. 18 - Prob. 27ECh. 18 - Prob. 28ECh. 18 - Prob. 29ECh. 18 - Prob. 30ECh. 18 - Prob. 31ECh. 18 - Prob. 32ECh. 18 - Prob. 33ECh. 18 - Prob. 34ECh. 18 - Which direction of the equilibrium...Ch. 18 - Prob. 36ECh. 18 - Prob. 37ECh. 18 - Prob. 38ECh. 18 - Prob. 39ECh. 18 - Consider the following system at equilibrium at...Ch. 18 - Prob. 41ECh. 18 - Prob. 42ECh. 18 - Prob. 43ECh. 18 - Prob. 44ECh. 18 - Prob. 45ECh. 18 - Prob. 46ECh. 18 - Prob. 47ECh. 18 - Prob. 48ECh. 18 - Prob. 49ECh. 18 - Prob. 50ECh. 18 - The equilibrium between nitrogen monoxide, oxygen,...Ch. 18 - The equilibrium constant expression for a given...Ch. 18 - Prob. 53ECh. 18 - For the following system, K=4.86105 at 298K:...Ch. 18 - Prob. 55ECh. 18 - Prob. 56ECh. 18 - Prob. 57ECh. 18 - Question 57 and 58: In Chapter 9, we discussed how...Ch. 18 - Prob. 59ECh. 18 - A student measures the molar solubility of...Ch. 18 - Prob. 61ECh. 18 - Prob. 62ECh. 18 - Find the moles per liter and grams per 100mL...Ch. 18 - Prob. 64ECh. 18 - Prob. 65ECh. 18 - Prob. 66ECh. 18 - Prob. 67ECh. 18 - Ksp for silver hydroxide is 2.0108. Calculate the...Ch. 18 - Prob. 69ECh. 18 - Prob. 70ECh. 18 - Prob. 71ECh. 18 - Prob. 72ECh. 18 - Prob. 73ECh. 18 - Prob. 74ECh. 18 - Prob. 75ECh. 18 - Prob. 76ECh. 18 - Prob. 77ECh. 18 - Prob. 78ECh. 18 - Prob. 79ECh. 18 - Classify each of the following statements as true...Ch. 18 - Prob. 81ECh. 18 - Prob. 82ECh. 18 - Prob. 83ECh. 18 - Prob. 84ECh. 18 - Prob. 85ECh. 18 - Prob. 86ECh. 18 - Prob. 87ECh. 18 - Prob. 88ECh. 18 - Prob. 89ECh. 18 - Prob. 90ECh. 18 - Hard water has a high concentration of calcium and...Ch. 18 - Prob. 18.1TCCh. 18 - Prob. 18.3TCCh. 18 - a What happens to a reaction rate as temperature...Ch. 18 - Prob. 18.5TCCh. 18 - Write a brief description of the relationships...Ch. 18 - Prob. 2CLECh. 18 - Prob. 3CLECh. 18 - Prob. 4CLECh. 18 - Prob. 5CLECh. 18 - Prob. 1PECh. 18 - Prob. 2PECh. 18 - Prob. 3PECh. 18 - Prob. 4PECh. 18 - Prob. 5PECh. 18 - Prob. 6PECh. 18 - Prob. 7PECh. 18 - Prob. 8PECh. 18 - Prob. 9PECh. 18 - Prob. 10PECh. 18 - Prob. 11PECh. 18 - Prob. 12PECh. 18 - What is the molar solubility of calcium fluoride...Ch. 18 - Prob. 14PECh. 18 - Prob. 15PECh. 18 - Prob. 16PECh. 18 - Prob. 17PECh. 18 - Prob. 18PECh. 18 - Prob. 19PE
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- Calculate K for the reactions in Question 1.arrow_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forwardAn aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forward
- Answer the following questions by referring to standard electrode potentials at 25C. a Will oxygen, O2, oxidize iron(II) ion in solution under standard conditions? b Will copper metal reduce 1.0 M Ni2(aq) to metallic nickel?arrow_forwardAlthough silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.arrow_forwardWhat additional information do we need to answer the following question: How is the equilibrium of solid silver bromide with a saturated solution of its ions affected when the temperature is raised?arrow_forward
- Solid silver iodide, AgI, can be dissolved by adding aqueous sodium cyanide. Calculate Knet the following reaction. AgI(s)+2CN[Ag(CN)2](aq)+I(aq)arrow_forwardThe blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O Oarrow_forwardGenerate equilibrium constant expression for the reaction: Fe(CN)6³ + Cr²+ ↔ Fe(CN)6+ + Cr³+. Calculate numerical values for Keq.arrow_forward
- Calculate the solubility of AgBr in a 1.00 M aqueous solution of ammonia, given: AgBr(s) ⇌ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13 Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x 107 [Hint: combine these reactions into a single reaction].arrow_forwardGiven the following reactions, AgBr(s) Ag+(aq) + Br–(aq) Ksp = 5.4 ´ 10–13 Ag+(aq) + 2 CN–(aq) Ag(CN)2–(aq) Kf = 1.2 ´ 1021 determine the equilibrium constant for the reaction below. AgBr( s) + 2 CN –( aq) Ag(CN) 2 –( aq) + Br –( aq)arrow_forward3) Write the equilibrium expression for the following reaction. Cu2+ + 4SCN E→ Cu(SCN),²-arrow_forward
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