Please find the solutions without using the Hasselbach equation. Please show all calculations.

Question 1

Find [H^+] in a 25 degrees Celsius solution prepared by dissolving 0.20 moles of NH4Cl in water and diluting to a volume of 400 mL, given that Kb = 1.8 x 10^-5 for NH3 (aq) at 25 degrees Celsius.

Question 2

Find [H^+] in an aqueous 25 degrees Celsius that is .20 M in HC2H3O2 and .48 M in NaC2H3O2. For HC2H3O2, Ka = 1.8 x 10^-5 at 2 degrees Celsius.

Question #3

A solution is prepared by adding HCl and HC2H3O2 to water. In the equilibrium constant.

Ka = [H^+] [C2H3O2^-]/[HC2H3O2]

Which of the following is correct

a) The H^+ in the numerator includes only the H+ that comes from the ionization of the HC2H3O2.

b) The H+ in the numerator in includes both the H+ that comes from the ionization of the HC2H3O2 and from the ionization of the HCl.

Solution Preview

Q1. NH4+ -----> NH3 + H+

[NH4+] = 0.20mol / 0.4L = 0.5M

If' x' is the change in concentration, then

Ka = 1 x 10^(-14) / Kb = [NH3][H+] / [NH4+] => 5.56 x 10^-10 = x^2/ (0.5 -x)
Hence 2.78 x 10^-10 - 5.56 x 10^-10x = ...

Solution Summary

Three equilibrium problems that deal with finding out unknown concentrations are solved without using the Henderson-Hasselbach equation.

Using a ICE table (initial change equilibrium)
a) Calculate the pH of solution that is 0.175M in acidic acid(HC2H3O2) ans 0.110Min potassium Acetate(KC2H302)
b) Perform same calculation using the Henderson HasselBach equations to determine pH of the solution

This solution is an answer to finding the pH of a solution if it is either a strong acid/base or a weak acid/base or a buffer containing a weak acid and its conjugate or weak base and it's conjugate.
1.
a) Give examples of strong acids and bases.
b) find the pH of 0.01 M and 0.001 M solution
of each.
2.
a) Give exa

Hey there. I am having trouble with this question.
Calculate the molar concentration of OH- ions in a 0.550 M solution of hypobromite ion (BrO-; Kb=4.0 x 10^-6). What is the pH of this solution?
Could you please show the work. And no power points please.
Thanks in advance!

Part 1: What is the pH of a solution of 1M HCO3 and 1M CO3?
Part 2: What is the pH if it was mixed with an equal volume of water?
Part 3: What is the pH if it was mixed with an equal volume of 0.001 M HCl?
Part 4: What is the pH if it was mixed with an equal volume of 0.001 M NaOH?

The concentration(in milligrams per cubic centimeter) of a certain drug in a patients body t hours after injection is given by C(t)= t^2/3t^3+1, 0 greater than t or greater than 5.(0concentration of the drug increasing and when is it decreasing?

The concentration C of a certain drug in a patient's bloodstream t minutes after injection is given by
C(t)=50T divide by t^2 +25
a) Using your graphing utility, graph C=C(t).
b) Determine the time at which the concentration is highest.
c) Find the horizontal asymptote of C(t). What happe

The equillibrium constant Kc for the reaction shown is 2.18 x 10^6 at 730 deg. C.
H2(g)+Br2(g) <--> HBr(g)
Starting with 3.30 moles of HBr in a 12.0 L reaction vessel, calculate the concentration of H2, Br2, and HBr at equil.

I would like to see the details of the calculations.
For my lab experiment I have the following data:
Titration 1:
25.00mL of unknown concentration HCl
2 drops of phenolpthalein to show end-point
1.0M NaOH
What is the molarity of the HCl?
What is the Ka of the HCl?
What is the equivalence point?
What is the half-equival

Assume the market shares of the six largest firms in an industry are 12 percent each. Calculate the six-firm concentration ratio and Herfindahl-Hirschman index for this industry. What does each of these measures have to say about the degree of concentration in the industry? Explain.