I specifically need help with part B 11) Consider the chemical reactio.docx

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I specifically need help with part B 11) Consider the chemical reaction shown below: a) Which reactant functions as an acid in this reaction? Explain your answer clearly b) When this reaction reaches equilibrium, will the cquilibrium mixture contain a higher concentration of products or of reactants? Explain your answer clearly Ka values: H2SO3-0.015 H:P04-62 x 10\" HS03-1,0 x 107 HP0,-0.007s Solution (b) Note : in this reaction 1: For forward reaction H 2 SO 3 is acid whereas for backwards H 3 PO 4 is acting acid thus more K a means faster reation as for H2SO3 is more thus forward reaction proceeds fast and hence more products will be formed. 2: same is the case for base acting species, more K a means less basic thus the species with lesser Ka will react faster with acid. this is for H2PO4 hence forward reaction is favoured. .

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9:46 LTE Labs Le.chateliers-lab.pdf Before beginning this experiment in the laboratory you should be alieto answer the following questions PRE LAB QUESTIONS 1. Beiefly stabe LeChidelier\'s Principle. 2. Consider the following equilibrium In which direction will the equilibrium shit if a. HSO,ibs added? Why? b. Buicl, is added? Why C NaCl is added? Why d. Heat is added? Why? Consider the folewing equilibrium foe nitous acid, HNOs,a weak acid In which direction will the equilibrium shift if a NaOH is added? b. NaNO, is added HCl is added? d. The acid solution is made more dilute? Complete and balance the following equations and then wrae balanced net ionic equations. 4· 3. On the busis of LeChitelier\'s Principle, explain why Ag-C0 disos when HNO, is added Previous Next Dashboard Calendar To DoNotifications Inbox Solution Answer: 1. Le Chtelier\'s principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to re-establish a new equilibrium 2.a) H2SO4 is added: the equilibrium shifts to the left because as there are more sulfate ions are added. b)BaCl2 is added The equilibrium shifts to the left because as there are more Ba^+2 are added. c) NaCl is added There is no shift in the equilibrium. As there are no Na^+1 and Cl^-1 are present in the equilibrium mixture d) Heat is added The equilibrium will shift to the right. As the forward reaction is endothermic, when the heat is added, the reaction will favours the product 3. a) NaOH is added The equilibrium will shift to the left because as there are more OH^-1 ions added, it will react with H+ present in the right side and forms more water. b)NaNO2 is added The equilibrium will shift to the left because the more NO2^-1 ions added, it forms more HNO2 by reacts with H3O^+1. c) HCl is added The equilibrium will shift to the right because more H+ is added in the equilibrium mixture d) The acid solution is made more dilute The equilibrium will shift to the right as there are more water is added. 4 a) AgNO3 (aq) + HCl (aq) <<>> AgCl (s) + HNO3 (aq) Net ionic equation: Ag^+1 (aq) + Cl^-1 (aq) >> AgCl (s) b) NH3(aq) + HCl (aq) <<<>> NH4Cl (s) Net equation: NH3 (aq) + H^+1 (aq) + Cl^-1 (aq) > NH4Cl(s) c) Na2CO3 (aq) + 2HNO3 (aq) <<>> H2O(l) + 2NaNO3 (aq) + CO2 (g) Net ionic equation: CO3 ^-2 (aq) + 2H+ (aq) >> H2O (l) + CO2 (g) 5. Ag2CO3 (s) + 2HNO3 (aq) <<<>>> 2AgNO3 (aq) + H2O (l) + CO2(g) Ag2CO3 is a solid . When adding nitric acid to silver carbonate, it forms soluble silver nitrate..

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