posted by .

Consider the titration of 100.0 mL of 0.500 M NH3 (Kb = 1.8 x 10-5) with 0.500 M HCl. At the
stoichiometric point of this titration, the [H+] is:

  • chemistry -

    NH3 + HCl ==> NH4Cl
    (NH4Cl) at eq. point = 0.500 x (100/200) = 0.25M
    The pH is determined by the hydrolysis of the salt, NH4Cl.
    .......NH4^+ + H2O ==> H3O^+ + OH^-

    Ka for NH4^+ = (Kw/Kb for NH3) = (H3O^+)(OH^-)/(NH4^+)
    Substitute into the equil equation from the equil line in the ICE chart and solve for x = (OH^-) and convert to pH.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemisty

    Consider the titration of 50 mL of 0.15 M NH3 with 0.1 M HCl. What is the pH at the equivalence point of the titration?
  2. AP Chemistry

    In the titration of 50.0 mL of 1.0 M CH3NH2 (kb=4.4 x 10^-4), with 0.50 M HCl, calculate the pH a) after 50.0 mL of 0.50 M has been added b) at the stoichiometric point.
  3. Chemistry 12

    Hey guys i only have this question left on my review and i just can't fingure it out! Sketch a pH curve for the titration of 40.00mL of 0.100 M hydrazine, H2NNH2, having a K of 3.0x10^-6 by 0.100 M HCIO4 a) what combination of acide-base …
  4. chemistry

    There is a titration of 5.00 mL .010 M NaOH with .005 M HCl. Indicate the pH of the initial and final solutions and the pH at the stoichiometric point. What volume of HCl has been added at the stoichiometric point and the halfway point …
  5. chemistry

    The titration of HCl with NaOH is represented by the equation HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) What volume of 0.100 M HCl is required to titrate 50.0 mL of 0.500 M NaOH?
  6. AP Chemistry

    In the titration of 77.5 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 10-4), with 0.38 M HCl, calculate the pH under the following conditions. (a) after 50.0 mL of 0.38 M HCl has been added (b) at the stoichiometric point
  7. Chem 1A

    A 15.00 g sample of an ionic compound NaA, where A- is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 700.0 mL of HCl was added, the pH was 5.00. The …
  8. ap chemistry

    What is the pH at the point during a titration when 34 mL of 0.200 M HCl has been added to 29 mL of 0.0500 M NH3 solution?
  9. Chemistry

    Consider the titration of 30.0 mL of 0.100 M NH3 with 0.150 M HCl. calculate the pH after the following volumes of titrant have been added:(a) 0mL (b) 10.0 mL (c) 19.5 mL (d) 20.0 mL (e) 20.5 mL (f) 30 mL
  10. Chemistry

    Consider the titration of a 50.0 mL 0.500 M F- with 0.500 M HCl. The pKa of HF = 3.46 and the pKb of F- is 10.54. Calculate the pH at the following volumes of HCl added. 1. Vsa= 0.00 mL of 0.500 M HCl 2. Vsa= 25.0 mL of 0.500 M HCl …

More Similar Questions