Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393600681
Author: Gilbert
Publisher: W. W. Norton & Company
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Chapter 16, Problem 16.70QA
Interpretation Introduction
To explain:
A color change that happens when copper sulphate reacts with a strong base and then ammonia.
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Students have asked these similar questions
When a strong base is added to a solution of CuSO4, which is pale blue, a precipitate forms and the
solution above the precipitate is colorless. What is the net chemical equation that describes this reaction?
Include the phases of all species in the chemical equation.
When ammonia is then added, the precipitate dissolves and the solution turns a deep navy blue. What is the
net chemical equation that describes this event? Include the phases of all species in the chemical equation.
Cu(OH)₂(s) + 4NH₂(aq) → [Cu(NH₂)]²+ (aq) + 2OH¯(aq)
Tip: Plus signs (+) can be typed from the keyboard. Reaction arrows can be found in the Tools
menu of the answer module. Include phases in the balanced chemical equation. Click on the
(aq) button in the tools to select the phase to add. Phases should not be subscripted.
Consider a pale blue solution of CuSO4.
Include phases in the balanced chemical equations.
When a strong base is added to the pale blue solution of CuSO4, a precipitate forms and the solution above the precipitate is colorless(1) What is the net ionic equation that describes this irreversbile reaction?
Ammonia is then added to the above heterogenous mixture. The precipitate dissolves, and then the entire solution turns a deep navy blue. However adding OH- to the deep navy blue solution results in the precipiate reforming.(2) What is the net ionic equation that describes this reversible event?
Consider the insoluble compound silver bromide, AgBr. The silver ion also forms
a complex with cyanide ions. Write a net ionic equation to show why the solubility
of AgBr(s) increases in the presence of cyanide and calculate the equilibrium
constant for this reaction. Solubility product constant data is found in the
Chemistry References.
For Ag(CN)₂, Kf = 1.3×1021. Be sure to specify states such as (aq) or (s).
K=
+
+
Chapter 16 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 16 - Prob. 16.2VPCh. 16 - Prob. 16.3VPCh. 16 - Prob. 16.4VPCh. 16 - Prob. 16.5VPCh. 16 - Prob. 16.6VPCh. 16 - Prob. 16.7VPCh. 16 - Prob. 16.8VPCh. 16 - Prob. 16.9VPCh. 16 - Prob. 16.10VPCh. 16 - Prob. 16.11QA
Ch. 16 - Prob. 16.12QACh. 16 - Prob. 16.13QACh. 16 - Prob. 16.14QACh. 16 - Prob. 16.16QACh. 16 - Prob. 16.17QACh. 16 - Prob. 16.18QACh. 16 - Prob. 16.19QACh. 16 - Prob. 16.20QACh. 16 - Prob. 16.21QACh. 16 - Prob. 16.22QACh. 16 - Prob. 16.23QACh. 16 - Prob. 16.24QACh. 16 - Prob. 16.25QACh. 16 - Prob. 16.26QACh. 16 - Prob. 16.27QACh. 16 - Prob. 16.28QACh. 16 - Prob. 16.29QACh. 16 - Prob. 16.30QACh. 16 - Prob. 16.31QACh. 16 - Prob. 16.32QACh. 16 - Prob. 16.33QACh. 16 - Prob. 16.34QACh. 16 - Prob. 16.35QACh. 16 - Prob. 16.36QACh. 16 - Prob. 16.37QACh. 16 - Prob. 16.38QACh. 16 - Prob. 16.39QACh. 16 - Prob. 16.40QACh. 16 - Prob. 16.41QACh. 16 - Prob. 16.42QACh. 16 - Prob. 16.43QACh. 16 - Prob. 16.44QACh. 16 - Prob. 16.45QACh. 16 - Prob. 16.46QACh. 16 - Prob. 16.47QACh. 16 - Prob. 16.48QACh. 16 - Prob. 16.49QACh. 16 - Prob. 16.50QACh. 16 - Prob. 16.51QACh. 16 - Prob. 16.52QACh. 16 - Prob. 16.53QACh. 16 - Prob. 16.54QACh. 16 - Prob. 16.55QACh. 16 - Prob. 16.56QACh. 16 - Prob. 16.57QACh. 16 - Prob. 16.58QACh. 16 - Prob. 16.59QACh. 16 - Prob. 16.60QACh. 16 - Prob. 16.61QACh. 16 - Prob. 16.62QACh. 16 - Prob. 16.63QACh. 16 - Prob. 16.64QACh. 16 - Prob. 16.65QACh. 16 - Prob. 16.66QACh. 16 - Prob. 16.67QACh. 16 - Prob. 16.68QACh. 16 - Prob. 16.69QACh. 16 - Prob. 16.70QACh. 16 - Prob. 16.71QACh. 16 - Prob. 16.72QACh. 16 - Prob. 16.73QACh. 16 - Prob. 16.74QACh. 16 - Prob. 16.75QACh. 16 - Prob. 16.76QACh. 16 - Prob. 16.77QACh. 16 - Prob. 16.78QACh. 16 - Prob. 16.79QACh. 16 - Prob. 16.80QACh. 16 - Prob. 16.81QACh. 16 - Prob. 16.82QACh. 16 - Prob. 16.83QACh. 16 - Prob. 16.84QACh. 16 - Prob. 16.85QACh. 16 - Prob. 16.86QACh. 16 - Prob. 16.87QACh. 16 - Prob. 16.88QACh. 16 - Prob. 16.89QACh. 16 - Prob. 16.90QACh. 16 - Prob. 16.91QACh. 16 - Prob. 16.92QACh. 16 - Prob. 16.93QACh. 16 - Prob. 16.94QACh. 16 - Prob. 16.95QACh. 16 - Prob. 16.96QACh. 16 - Prob. 16.97QACh. 16 - Prob. 16.98QACh. 16 - Prob. 16.99QA
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- 9. [CoCl4]? (suda) + 6H2O (s) [Co(H2O)6]?* (suda) + 4Cl (suda) + isi blue ping The reaction given above is in equilibrium at constant temperature and the following steps are applied. Balance Answer the following questions taking into account the reaction. a) When distilled water is added to the balance, in which direction does the balance move and what will be the resulting color? b) When a salt containing chloride ions is added to the equilibrium, in which direction does the equilibrium move and what color will be formed? c) When the reaction at equilibrium is heated, in which direction does the equilibrium move and what color will be formed?arrow_forwardBarium fluoride has increased solubility in acidic solution. Why?arrow_forwardExplain why the solubility of AgBr decreases when NaBr is added to the system.arrow_forward
- The final product of this reaction, [Cu(NH3)4]SO4 H₂O is soluble in water. What will you add to the solution after you add the concentrated ammonia to cause this product to precipitate out of solution? 95% ethanol methanol isopropyl alcohol Nothing will be added. The precipitate will form when the solution is cooled in an ice bath. O Nothing will be added. The precipitate that we will isolate will form as the concentrated NH3 is added to the solution of [Cu(H₂O)4]²+arrow_forwardConsider the insoluble compound copper(II) hydroxide, Cu(OH)₂ . The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Cu(OH)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)4²+, Kf = 6.8×10¹² . Be sure to specify states such as (aq) or (s). K = 2+ Submit Answer + + Retry Entire Group 2 more group attempts remainingarrow_forward<p>When solid Cd(OH)2 is added to a solution of 0.10 M NaI some of it dissolves. Calculate the pH of the solution at equilibrium.arrow_forward
- provide explanation of formula.arrow_forwardAfter completing a distillation to purify a mixture of sodium chloride and water, you decide to test the water to determine its purity. Upon addition of silver nitrate (AgNO3), a white solid precipitates out of the solution. Use the solubility table on Page 96 to determine the identity of the precipitate.arrow_forwardIn reaction with aqueous ammonia, Zn(OH)2 forms a complex ion. Explain the term complex ion, and explain how the formation of such a species can affect the solubility of a salt.arrow_forward
- (a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?arrow_forwardIn a solution of potassium chromate, there is an equilibrium where chromate ions are bright yellow and dichromate ions are orange. What would you observe if you treated the orange solution with sodium hydroxide?arrow_forwardA saturated solution of Mg3(PO4)2 has a concentration of 0.939 mg per liter. Calculate the solubility product constant for Mg3(PO4)2.arrow_forward
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