Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Chapter 19, Problem 23E
Dilute sodium cyanide solution is slowly dripped into a slowly stirred silver nitrate solution. A white precipitate forms temporarily but dissolves as the addition of sodium cyanide continues. Use chemical equations to explain this observation. Silver cyanide is similar to silver chloride- in its solubility.
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Dilute sodium cyanide solution is slowly dripped into a slowly stirred silver nitrate solution. A white precipitate forms temporarily but dissolves as the addition of sodium cyanide continues. Use chemical equations to explain thisobservation. Silver cyanide is similar to silver chloride in its solubility.
A solution of potassium dichromate is made basic with sodium hydroxide;the color changes from red to yellow. Addition of silver nitrate to the yellow solution gives a precipitate. This precipitate dissolves in concentrated ammonia but re-forms when nitric acid is added. Write balanced net ionic equations for all the reactions in this sequence.
Chromium(III) hydroxide is highly insoluble in distilled water but dissolves readily in either acidic or basic solution. Briefly explain why the compound can dissolve in acidic or in basic but not in neutral solution. Write appropriate equations to support your answer.
Chapter 19 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 19 - Write the electron configurations far each of the...Ch. 19 - Write the electron con?gurations for each of the...Ch. 19 - Write the electron configurations for each of the...Ch. 19 - Why are the lanthanoid elements not found in...Ch. 19 - Which of the following elements is most likely to...Ch. 19 - Which of the following is the strongest oxidizing...Ch. 19 - Which of the following elements is most likely to...Ch. 19 - The following reactions all occur in a blast...Ch. 19 - Why is the formation of slag useful during the...Ch. 19 - Would you expect an aqueous manganese (VII) oxide...
Ch. 19 - Iron (II) can be oxidized to iron (III) by...Ch. 19 - How many cubic feet of air at a pressure of 760...Ch. 19 - Find the potentials of the following...Ch. 19 - A 2.5624-g sample of a pure solid alkali metal...Ch. 19 - The standard reduction potential for the reaction...Ch. 19 - Predict the products of each of the following...Ch. 19 - Predict the products of each of the following...Ch. 19 - Describe the electrolytic process for refining...Ch. 19 - Predict the products of the following reactions...Ch. 19 - What is the gas produced when iron(II) sulfide is...Ch. 19 - Predict the products of each of the following...Ch. 19 - Balance the following equations by...Ch. 19 - Dilute sodium cyanide solution is slowly dripped...Ch. 19 - Predict which will be more stable, [CrO4]2- or...Ch. 19 - Give the oxidation state of the metal for each of...Ch. 19 - Indicate the coordination number for the central...Ch. 19 - Give the coordination numbers and write the...Ch. 19 - Give the coordination number for each metal ion in...Ch. 19 - Sketch the structures of the following complexes....Ch. 19 - Draw diagrams for any Cis, trans, and optical...Ch. 19 - Name each of the compounds or ions given in...Ch. 19 - Name each of the compounds or ions given in...Ch. 19 - Specify whether the following complexes have...Ch. 19 - Predict whether the carbonate ligand CO32- will...Ch. 19 - Draw the geometric, linkage, and ionization...Ch. 19 - Determine the number of unpaired electrons...Ch. 19 - Draw the Crystal field diagrams for [Fe(NO2)6]4-...Ch. 19 - Give the oxidation state of the metal, number of d...Ch. 19 - The solid anhydrous solid CoCl2 is blue in color....Ch. 19 - Is it possible for a complex of a metal in the...Ch. 19 - How many unpaired electrons are present in each of...Ch. 19 - Explain how the diphosphate ion, [O3P-O-PO3]4-,...Ch. 19 - For complexes of the same metal ion with no change...Ch. 19 - Trimethylphosphine, P(CH3)3, can act as a ligand...Ch. 19 - Would you expect the complex [Co(en)3]Cl3 to have...Ch. 19 - Would you expect the Mg3[Cr(CN)5]2 to be...Ch. 19 - Would you expect salts of the gold(I) ion, Au+, to...Ch. 19 - [CuCl4]2- is green. [Cu(H2O)6]2+ is blue. Which...
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- Barium fluoride has increased solubility in acidic solution. Why?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_forward1. When potassium dichromate (K2CRO4) is added to a solution containing 0.500 g silver nitrate (AGNO3), solid silver chromate (Ag2CrO4) is formed. ( Note: Be sure to write down the balanced chemical equation.) a) Determine the theoretical yield of the silver chromate precipitate. b) If 0.455 g of silver chromate is obtained, calculate the percentage yield.arrow_forward
- Approximately 1 mL of two clear, colorless solutions, 0.1 M Mn(NO3)2 and 0.1 M NaOH, were combined. Upon mixing, a brown precipitate formed. After centrifugation, the solution above the precipitate was found to be clear and colorless. Based on the these observations, determine if a reaction occurred. If so, write the balanced chemical equation.arrow_forward:) thanksarrow_forwardSuppose you mistakenly used tap water instead of distilled water to dissolve your consumer product. When you did the test for chloride, you observe formation of a white precipitate after addition of silver nitrate. Can you rightly conclude that the product being tested contains chloride? Explain your reasoning.arrow_forward
- 5. When copper sulfate is dissolved in water, it forms a clear blue solution. What are the formulas of the two ions in this solution? A small amount of aqueous ammonia is added to this solution, and a light blue precipitate forms. What is the formula for this precipitate? The precipitate dissolves to form a dark blue solution when more ammonia is added. Why?arrow_forwardConsider 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= + +arrow_forwardThe substance to be analyzed – is white, highly soluble in water salt. Addition of barium chloride or silver nitrate (in presence of nitric acid) doesn't give any precipitation. Reaction with zinc uranyl acetate leads to formation of yellow crystals, which have tetrahedral geometry. Addition of antipyrin in acid medium changes color to red. What kind of substance is this? NaNO3 BaSO3 LİCI NaNO,arrow_forward
- In 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_forwarddescribe how would you precipitate copper(II) phosphate from a solution of copper(II) chloride.arrow_forwardConsider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(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 = + +arrow_forward
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