QUESTION 2 The instructor reveals that the weak acid is hypochlorous acid, HOCI. The known Ką for HOCI is 4.0x10-8. What is the percent error in the experiment?
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Given
Known/accepted value of Ka for HOCl = 4 × 10-8
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- A certain weak acid, HAHA, has a Ka�a value of 4.4×10−7. Calculate the percent ionization of HAHA in a 0.10 M� solution. Express your answer as a percent using two significant figures.That's exactly what is my answer was, and got marked as a wrong answer I put 0.594 M HC2H3O24. Assuming no calculation errors, why would a percent recovery > 100% or a percent recovery < 100% be obtained? Give at least one reason for each
- A student performed a titration on a commercial acid certified to be 0.500 M. Using her data from the titration, the student determined her sample to be 0.487 M. Assuming the certified value was the true value, what was the percent error of her measurement?Please balance these equations! I need help and explain if you can please!! Reference test for Ag+ using NaCl: ______ NaCl (aq) + _______ AgNO3 (aq) → ________ NaNO3 (aq) + ________ AgCl (s) Reference test for Ba2+ using H2SO4: _______ H2SO4 (aq) + _______ Ba(NO3)2 (aq) → ________ HNO3 (aq) + ________ BaSO4 (s) Reference test for Cu2+ using NH3: _______ NH3 (aq) + ________ Cu(NO3)2 (aq) → ________ [Cu(NH3)4]2+ (aq) + ________ NO3– (aq) Reference test for Fe3+ using KSCN: ______ KSCN (aq) + ______ Fe(NO3)3 (aq) → ______ Fe(SCN)2+ (aq) + ______ NO3– (aq) + _____ K+ (aq)The instructor reveals that the weak acid is hypochlorous acid, HOCl. The known Ka HOCl is 4.0x10-8 . What is the percent error in the expirement ?
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