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,
Trending nowThis is a popular solution!
Chapter 16 Solutions
Chemistry
- When two reactants have combined in proportions and the both of them have been consumed and neither of them remains in excess, this point is called? Equivalence point Titration point Neutrality End pointarrow_forwardAn aqueous solution is prepared to be 0.408 M in sodium formate and 0.291 M in acetic acid. (1) Is this solution a buffer solution? (2) What is the pH of this solution? pH = (3) If 0.128 moles of hydrobromic acid are added to one liter of this solution, what is the pH of the resulting solution? pH = Use the Tables link in the References for any equilibrium constants that are required.arrow_forwardWhat is the solubility product constant? What is the solubility product constant? The solubility product constant is the equilibrium expression for a chemical equation representing the formation of a molecular compound. The solubility product constant is the equilibrium expression for a chemical equation representing the dissolution of a molecular compound. The solubility product constant is the equilibrium expression for a chemical equation representing the formation of slightly soluble ionic compounds. The solubility product constant is the equilibrium expression for a chemical equation representing the dissolution of an ionic compound. SubmitRequest Answer Part B Choose a general expression for the solubility constant of a compound with the general formula AmXnAmXn. Choose a general expression for the solubility constant of a compound with the general formula . Ksp=[An+]m[Xm−]nKsp=[An+]m[Xm−]n Ksp=[Am+]n[Xn−]mKsp=[Am+]n[Xn−]m…arrow_forward
- What is molar solubility?arrow_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_forwardWhen 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.arrow_forward
- A student receives an unknown mixture that is thought to contain the Group I cations. The student performs qualitative analysis on the sample and makes the folowing observa -After adding excess Nact a precipitate was formed. - After the mixture was heated and decanted, a precipitate was seen when the heat was removed. With the addition of ammonia to the tube containing the precipitate, no color change was observed. -No white precipitate was formed after the addition of the pH 4 solution to the test tube Which of the Group I cations are likely to be present? Choose all that apply. DANa B. Ag OC. No Group I cations are present in this mixture □D-Hg₂+ E.Pb2+ OF. Hg2+arrow_forwardA solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCI to this buffer solution causes the pH to drop slightly. The pH does not present in the buffer solution. The Ka of hypochlorous acid is 1.36 decrease drastically because the HCI reacts with the × 10-3. Select one: Oa. hypochlorous acid Ob. H30¹ Ос H2O Od. hypochlorite ionarrow_forwardThis question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added. b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?arrow_forward
- Based 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_forwarda buffer solution is prepared by mixing the solution of a weak acid with its salt.Write two expressions that show what happens when two substances are dissolved in water. b) Based on the answer you gave to the above question explain why the pH of a buffer solution does not change even if we add a little acid.arrow_forwardWhat is the number of moles of 10.0 g NH₄Cl? What is the molar concentration of NH₄Cl? What is the pH of the buffer solution?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
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning