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51 PM Wed Apr 19 ... ☎96% + 1. Write the chemical reaction for the titration of the filtered KHT solution with NaOH

51 PM Wed Apr 19 ... ☎96% + 1. Write the chemical reaction for the titration of the filtered KHT solution with NaOH

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter8: Molecules And Materials
Section: Chapter Questions
Problem 8.72PAE
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1 of 3 + Automatic Zoom Theory In the previous lab, the dissolution of potassium bitartrate was described by the following chemical equation: KHC4H4O6(s) K(aq) + HC4H4O6 (aq) To simplify notation, potassium bitartrate (KHC4H4O6) was denoted as KHT and the bitartrate ion (HC4H406) will be denoted as HT where the H denotes an acidic proton: KHT(s) K (aq) + HT (aq) The solubility product constant for this process can be written as: (1) To determine the Ksp for this reaction, the equilibrium concentrations for K* and HT must be measured in a saturated solution of KHT. When enough solid KHT is added to pure water so that a saturated solution of KHT is prepared, then [K*]eq = [HT]eq. This leads to a simplification of eq. 1, Ksp = [HT]eq². The equilibrium concentration of HT is readily determined by titrating the solution with OH: [HT ] eq Ksp [K]eq[HT]eq = moles of HT- volume of HT-at beginning of titration (2) The equivalence point for the titration is determined using phenolphthalein as an indicator. Since KHT has been dissolved in pure water, the [HT-lea also represents the molar solubility of KHT (i.e. how many moles of KHT will dissolve in one liter of water). The Gibbs Free Energy change can be readily calculated from: AG = -RT In(Ksp) The equilibrium constant depends upon temperature and it can be shown that (3)
Transcribed Image Text:1 of 3 + Automatic Zoom Theory In the previous lab, the dissolution of potassium bitartrate was described by the following chemical equation: KHC4H4O6(s) K(aq) + HC4H4O6 (aq) To simplify notation, potassium bitartrate (KHC4H4O6) was denoted as KHT and the bitartrate ion (HC4H406) will be denoted as HT where the H denotes an acidic proton: KHT(s) K (aq) + HT (aq) The solubility product constant for this process can be written as: (1) To determine the Ksp for this reaction, the equilibrium concentrations for K* and HT must be measured in a saturated solution of KHT. When enough solid KHT is added to pure water so that a saturated solution of KHT is prepared, then [K*]eq = [HT]eq. This leads to a simplification of eq. 1, Ksp = [HT]eq². The equilibrium concentration of HT is readily determined by titrating the solution with OH: [HT ] eq Ksp [K]eq[HT]eq = moles of HT- volume of HT-at beginning of titration (2) The equivalence point for the titration is determined using phenolphthalein as an indicator. Since KHT has been dissolved in pure water, the [HT-lea also represents the molar solubility of KHT (i.e. how many moles of KHT will dissolve in one liter of water). The Gibbs Free Energy change can be readily calculated from: AG = -RT In(Ksp) The equilibrium constant depends upon temperature and it can be shown that (3)
Caps Shift Fn Q A N W -- 3:51 PM Wed Apr 19 S X E Alt 5 D C R F T V T G Y B JODOCU P H N J M K < L Alt 96% +: 1. Write the chemical reaction for the titration of the filtered KHT solution with NaOH.
Transcribed Image Text:Caps Shift Fn Q A N W -- 3:51 PM Wed Apr 19 S X E Alt 5 D C R F T V T G Y B JODOCU P H N J M K < L Alt 96% +: 1. Write the chemical reaction for the titration of the filtered KHT solution with NaOH.
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