CHEM 1F92 Lecture Notes - Lecture 7: Alkaline Earth Metal, Acid Strength, Sulfuric Acid
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± Weak Base Calculations Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized asNX3(aq)+H2O(l)âHNX3+(aq)+OHâ(aq) where NX3 is the base and HNX3+ is the conjugate acid. The equilibrium-constant expression for this reaction isKb=[HNX3+][OHâ][NX3] where Kb is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of Kb increases. Ka and Kb are related through the equation KaÃKb=Kw As the strength of an acid increases, its Ka value increase and the strength of the conjugate base decreases (smaller Kb value). | Part A If Kb for NX3 is 2.0Ã10â6, what is the pOH of a 0.175 M aqueous solution of NX3? Express your answer numerically.
SubmitHintsMy AnswersGive UpReview Part Correct Part B If Kb for NX3 is 2.0Ã10â6, what is the percent ionization of a 0.325 M aqueous solution of NX3? Express your answer numerically to three significant figures.
SubmitHintsMy AnswersGive UpReview Part Incorrect; Try Again; 3 attempts remaining Part C If Kb for NX3 is 2.0Ã10â6 , what is the the pKa for the following reaction?HNX3+(aq)+H2O(l)âNX3(aq)+H3O+(aq) Express your answer numerically to two decimal places.
SubmitHintsMy AnswersGive UpReview Part Incorrect; Try Again; 4 attempts remaining Not quite. Check through your calculations; you may have made a rounding error or used the wrong number of significant figures. Provide FeedbackContinue |