Interpretation:
It is given that, when sodium chloride is added to a solution of silver nitrate, a white precipitate is formed. This precipitate will be dissolved when ammonia is added to this mixture. Now a pale yellow precipitate will appear when a solution of potassium bromide is added to it. Now this precipitate will be dissolved when sodium thiosulfate is added and finally a yellow precipitate is formed when potassium iodide is added to this solution. The balanced equations are to be stated to explain these observations. The conclusion drawn corresponding to the size of the
Concept introduction:
The formation of solid in a solution is known as precipitation. Solubility product,
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry: An Atoms First Approach
- Refer to Appendix J for solubility products for calcium salts. Determine which of the calcium salts listed is most soluble in moles per liter and which is most soluble in grams per liter.arrow_forwardExplain why the solubility of AgBr decreases when NaBr is added to the system.arrow_forwardBased on the solubility observations, would you except potassium and bromide to form a precipitate, and would you except sodium and nitrate to form a precipitate ? Yes or no ?arrow_forward
- What is the maximum amount of copper(II) sulfide that will dissolve in a 0.135 M solution of copper acetate solution?arrow_forwardExplain how a solution of butanoic acid and potassium butanoate can function as a buffer solution. Your answer must include a brief description of how this buffer functions on the addition of a small amount of acid , a small amount of alkali and a small amount of deionised water.. Include balanced chemical equations with physical statesarrow_forwardA buffer solution is one which a. contains the maximum amount of solute possible for a particular temperature. b. resists changes in pH upon addition of acid or base. c. contains more than the expected amount of solute for a particular temperature and is therefore unstable. d. changes color upon addition of strong base. e. contains an equal number of hydronium and hydroxide ionsarrow_forward
- A 0.6407g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430g. This precipitate was then strongly heated in a stream of chlorine gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181g. Calculate the percentage of chloride and iodide in the sample.arrow_forwardHow does one usually denote a complex ion when writing it?arrow_forwardWhich of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in acidic solution? According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming magnesium hydride and causing more magnesium hydroxide to dissolve. Magnesium hydroxide does not dissolve in acidic solutions. According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming water and thereby decreasing the concentration of hydroxide ions in solution causing more magnesium hydroxide to dissolve. According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a precipitate. According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide ions and thereby decreasing the concentration of magnesium ions in solution causing more magnesium hydroxide to dissolve.arrow_forward
- In water the solubility of lead chloride is higher than that of silver chloridearrow_forwardA chemistry student adds a known amount of solution of known concentration to determine the concentration of another solution. What is this process called? A) neutralization B) hydrolysis C) titration D) buffer capacityarrow_forwardConsider 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?arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax