For the antimony trichloride system, we assume only dilution when calculating concentrations. By making this assumption, are we adding random or systematic error to our data? Explain the error in this assumption. O Random error because we do not consider any reaction that occurs when distilled water or HCI is added. The error will persist regardless of how many times the experiment is repeated O Systematic error because we do not consider any reaction that occurs when distilled water or HCI is added. The error will persist regardless of how many times the experiment is repeated O Random error because the dilution accounts for any reaction that may occur when distilled water or HCI is added. The error may not be introduced if the procedure is repeated O Systematic error because the dilution accounts for any reaction that may occur when distilled water or HCI is added. The error may not be introduced if the procedure is repeated

For the antimony trichloride system, we assume only dilution when calculating concentrations. By making this assumption, are we adding random or systematic error to our data? Explain the error in this assumption. O Random error because we do not consider any reaction that occurs when distilled water or HCI is added. The error will persist regardless of how many times the experiment is repeated O Systematic error because we do not consider any reaction that occurs when distilled water or HCI is added. The error will persist regardless of how many times the experiment is repeated O Random error because the dilution accounts for any reaction that may occur when distilled water or HCI is added. The error may not be introduced if the procedure is repeated O Systematic error because the dilution accounts for any reaction that may occur when distilled water or HCI is added. The error may not be introduced if the procedure is repeated

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 37P

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the free energy for a reaction can be related to the equilibriumconstant through the formula below. K = e (-ΔG° / RT) Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations. G = H – T S In this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established. Na2B4O5(OH)4*8H2O (s) <--> 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l) If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid…
the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid according to the…
the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid according to the…
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