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18 Nov 2019
± Dissociation Constant Part A For the dissociation reaction of a weak acid in water HA(aq)H2Ol) H3O (aq)A (aq) the equilibrium constant is the acid-dissociation constant, Ka, and takes the form Aspirin (acetylsalicylic acid, CHsO4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirn in 0.600 L of water and measured the pH What was the Ka value calculated by the student if the pH of the solution was 2.60? Express your answer numerically using two significant figures. Hints Weak bases accept a proton from water to give the conjugate acid and OH ions: å ? B(aq) + H2O(l) ê·¼ BH"(aq) + OH (aq) The equilibrium constant Kb is called the base- dissociation constant and can be found by the formula Submit My Answers Give Up Bl Part B When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an I.C.E table, where I stands for Initial Concentration, C. stands for Change, and E. stands for Equilibrium Concentration. To create such a table, write the reaction across the top creating the columns, and the rows I.C.E on the left-hand side A 0.100 M solution of ethylamine (C2HNH2) has a pH of 11.87. Calculate the K, for ethylamine Express your answer numerically using two significant figures. Hints A+B â AB Initial (M) Change (M) Equilibrium (M) Submit My Answers Give Up Continue
± Dissociation Constant Part A For the dissociation reaction of a weak acid in water HA(aq)H2Ol) H3O (aq)A (aq) the equilibrium constant is the acid-dissociation constant, Ka, and takes the form Aspirin (acetylsalicylic acid, CHsO4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirn in 0.600 L of water and measured the pH What was the Ka value calculated by the student if the pH of the solution was 2.60? Express your answer numerically using two significant figures. Hints Weak bases accept a proton from water to give the conjugate acid and OH ions: å ? B(aq) + H2O(l) ê·¼ BH"(aq) + OH (aq) The equilibrium constant Kb is called the base- dissociation constant and can be found by the formula Submit My Answers Give Up Bl Part B When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an I.C.E table, where I stands for Initial Concentration, C. stands for Change, and E. stands for Equilibrium Concentration. To create such a table, write the reaction across the top creating the columns, and the rows I.C.E on the left-hand side A 0.100 M solution of ethylamine (C2HNH2) has a pH of 11.87. Calculate the K, for ethylamine Express your answer numerically using two significant figures. Hints A+B â AB Initial (M) Change (M) Equilibrium (M) Submit My Answers Give Up Continue
Keith LeannonLv2
5 May 2019