what does [h3o+] = ka simplfy to if you take the -log of both sides LJh be used
ID: 959697 • Letter: W
Question
what does [h3o+] = ka simplfy to if you take the -log of both sides LJh be used to determine the ionization constant of your weak acid. d for the titration of your unknown weak acid with Write the chemical equation for the reaction that shows the equilibrium for the dissociation of the weak acid. Use the abbreviated formulas, HA and A. to represent weak acid and its conjugate base respectively a. b. Write the equilibrium expression (K for the equilibrium above. Ka: Ltlso3CAor the equilibrium CHAJ c. Rearrange this expression to solve for (HO d. How do [HA] and [A] compare when the weak acid is exactly half neutralized (the half-equivalence point)? Thuy aru equal e. What would the expression in (c) above simplify to at the half-equivalence point? f. What does the expression in (e) simplify to if you were to take the negative log of both sides of the equation? g. Use your results above to determine the ionization constant of your weak acid from your titration curve. Look up the Ka's of the three unknown acids used in this lab. Calculate the percent error for the acid you most likely have. Unknown Letter Ka for your unknown HA (show work) Literature value for Formic acid K. -1.10 Acetic acid Ka = 18 : 10 Propanoic acid K,- 3-10's Percent error (show your calculations). Attach your titration curves to the report sheets!Explanation / Answer
yes all your answers are 100 % correct . you are good
f)
-log [H3O+] = - logKa
this means at half equivalece point : pH = pKa
because [HA] = [A-]
other explanation :
from henderson's equation :
pH = pKa + log [A- / HA]
pH = pKa + 0
pH = pKa
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