Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.
(a) 100.0 mL of 0.14 M HC7H5O2 (Ka= 6.4 multiplied by 10-5) titrated by 0.14 M NaOH
(b) 100.0 mL of 0.29 M C2H5NH2 (Kb = 5.6 multiplied by 10-4) titrated by 0.58 M HNO3
(c) 100.0 mL of 0.28 M HCl titrated by 0.14 M NaOH
I'm pretty unclear as far as how to go about it and would greatly appreciate help. Thanks in advance!
Chemistry - DrBob222, Friday, June 1, 2012 at 5:39pm
The pH at the half-way point of a monoprotic acid is just pKa. For a monoprotic base (C2H5NH2) it is pKa but remember they give you pKb in the problem so pKa = 14-pKb.
The pH at the equivalence point of a monoprotic acid or monoprotic base is calculated from the hydrolysis of the salt. Use (salt) = C = mols salt/L soln.
For the acid the anion is hydrolyzed:
........A^- + HOH ==>HA + OH^-
Kb for the A^- = Kw/Ka for the acid = (x)(x)/(C-x) and solve for x = OH^-, then convert to pH.
For the C2H5NH2 it is the salt C2H4NH3 that is hydrolyzed. I'll call that BNH3^+. Find (BNH3^+) at the equivalence point following the same procedure for the weak acid above.
........BNH3^+ + H2O ==> H3O^+ + BNH2
Ka for BNH3^+ = (Kw/Kb for BNH2) = (x)(x)/(C-x) and solve for x = (H3O^+) and convert to pH.
For the NaOH/HCl (strong base/strong acid),
mols acic to start - mols base added = mols HCl remaining. That gives H^+ when corrected for dilution and pH from that.
The equivalence pint is the hydrolysis of the salt but for SA/SB titrations neither the anion nor the cation are hydrolyzed so the pH = 7.0.
Post your work if you get stuck.
Chemistry - Andrew, Friday, June 1, 2012 at 7:09pm
So for the first portion I came to Kb=1.5x10^-10
x^2-(2.2x10^-11)x - 1.56x10^-10=0
solving with the quadratic equation I came to x= 1.25x10^-5 (I'm disregarding i)
So -log(1.25x10^-5)= 4.9
But somewhere I've done something wrong as the homework program I'm using is saying neither 4.9 or 9.1 are correct.
Chemistry - DrBob222, Friday, June 1, 2012 at 8:13pm
The concn of the salt is not 0.14. Note my instructions were the C = mols/L. At the equivalence point you have (let's call the acid HA)
HA + NaOH ==> NaA + H2O
You have 100 mL x 0.14M acid = 0.014 mols.
You have added 100 mL of 0.14M NaOH so
(salt) = 0.14mol/0.200 L = 0.07M.
You should have ended up with
Kb = 1.56E-10 = (x)(x)/(0.07-x)
If we assume 0.07-x = 0.07, then
x^2 = 1.09E-11 and
x = 3.31E-6 = (OH^-). First we check to see that the assumption is ok. Since 0.07-3.31E-6 = essentially 0.07 the assumption is ok and we need not solve a quadratic.
If OH^- = 3.31E-6 then pOH = 5.48 so pH = 8.52
Chemistry - Andrew, Friday, June 1, 2012 at 8:44pm
Alright, I was able to figure them all out. Thank you!
Chemistry - Gina, Friday, June 1, 2012 at 11:38pm
Hi, I need help with a chemistry question.
Question: Iron ore is treated with carbon monoxide to extract and purify the iron.
a) Calculate the minimum mass of carbon monoxide that must be ordered by a refining company for every metric tonne of iron ore that is processed.