Answered: Which one of the following would NOT…

Which one of the following would NOT form a precipitate with Ag* in solution? A) NaCI B) NaNO, C) Na,s D) NaOH E) All of the combinations will form precipitates.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 113SCQ: Suggest a method for separating a precipitate consisting of a mixture of solid CuS and solid...

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A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system called a heterogeneous equilibrium?
Suggest a method for separating a precipitate consisting of a mixture of solid CuS and solid Cu(OH)2.
A student was performing this experiment with an antacid tablet which contained C a CO3 but forgot to heat the antacid solution prior to starting the back-titration. As sodium hydroxide was added the student noticed the formation of an insoluble white precipitate. Would the presence of this precipitate cause the students experimentally determined volume of N a O H be incorrectly high or incorrectly low? Briefly explain. Hint: Carbon dioxide reacts with water to form carbonic acid. Question 3 options: Incorrectly high, the solution becomes more acidic if not boiled gently Incorrectly high, the solution becomes less acidic if not boiled gently Incorrectly low, the solution becomes more acidic if not boiled gently Incorrectly low, the solution becomes less acidic if not boiled gently
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Will a precipitate form if the chemist mixes 7.1x10^-3 M Ag+ (aq) with 4.2 x 10^-4 M CrO4 ^2- (aq)? (Explain)
Will adding water to SbCl + H20 <----> SbOCl + 2HCl form more or less precipitate? Will adding hydrochloric acid to SbCl + H20 <----> SbOCl + 2HCl form more or less precipitate?
PbCl2 is a slightly soluble salt. A solution contains 0.0045 M Pb+2. What concentration of Cl- is required to start precipitating the solid ?
Suppose that 150 mL of 0.200 M K2CO3 and 100 mL of 0.400 M Ca(NO3)2 are mixed together. Assume that the volumes are additive, that CaCO3 is completely insoluble, and that all other substances that might be formed aresoluble. Calculate the mass of CaCO3 precipitated, and calculate the concentrations in the final solution of the four ions that were present initially.
1. Describe a process to individually remove ions Br-, SO42-, and S2- from a solution. Be sure to list the compounds that you add in order, and the method of removing the precipitate.
An analytical chemist has a solution containing chloride ion, Cl−. She decides to determine the amount ofchloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AgNO3. As a way to indicate theendpoint of the titration, she added 1.00 g of potassium chromate, K2CrO4 (see Figure 1). As she slowly addedthe silver nitrate to the solution, a white precipitate formed. She continued the titration, with more whiteprecipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution atthis point was 60.3 mL. How many moles of chloride ion were there in the original solution? How many molesof chloride ion were there in the final solution? You may make any reasonable approximations

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