1. A. HCl does not appear in the equilibrium reaction between barium ion and chr
ID: 501475 • Letter: 1
Question
1. A. HCl does not appear in the equilibrium reaction between barium ion and chromate ion, yet it affects the reaction. Explain, making sure to use any relevant chemical equations. B. Do you think BaCrO4 is more soluble in acidic or in neutral solutions? Explain your answer using relevant chemical equations.
observations. the same all spills your instructor. to lots of An number of of dil (3 insoluble of HC drops ute M) removed salt can caustic. from someti be Barium experiment you will due to a competing if one of the solution mate (a prepare barium can effectively be ions). The source of barium chromate, reaction. net ionic a relatively insoluble of the equilibrium and salt, reaction by Bae is (a source of (aq) t Cro 2 chro (aq) BaCro 4(s) Le Chatelier's Principle According to Le Chatelier's principle, the solid barium chromate precipitate can be dissolved if the concentration of barium ion or chromate ion is The mate ion concentration can be lowered by adding acid, since, as seen in Part A of the procedure, acid will convert the chromate ion to the dichromate ion. 213 1. In a well of the 24-well assay plate, mix 5 drops of 0.1 M BaClo and 2 drops of 1 M KaCro4. Record your observations. 2. Add 12 M HCl (CAUTION: HCl is caustic) dropwise until a change is observed and record your observationsExplanation / Answer
For the given reaction, HCl does not appear in the equilinbrium equation, however it affects the reaction.
BaCrO4 formed from Ba2+ and CrO^2-, is a slightly soluble salt. Once H+ is added in to this solution, CrO4^2- forms Cr2O7^2- and lowers the concentration of CrO4^2- in the solution. Now, according to the LeChatellier's principle, this decrease of CrO4^2- on one end (left handside) causes more of BaCrO4 to dissolve into the solution until it reaches to the same equilibrium concentration of CrO4^2-. Thus BaCrO4^2- is more soluble in acidic medium
2H+ + 2CrO4^2- ---> Cr2O7^2- + H2O
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