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.

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

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?

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

I have 100mls of an antibiotic stock solution at a concentration of 6mg/ml. I would like a final volume of 10mls of the antibiotic at a concentration of 1.5mg/ml. How much of the stock solution do I need to obtain this?

You characterize a new enzyme's kinetics. Using a saturating (very high so all E is ES) substrate concentration, you measure the initial rate of the reaction at various enzyme concentrations. Does this data fit the Michaelis Menton model/equation? If not, what may be happening?
E (nM), rate (mM,s)
5, 50
10, 225
15

Find the solutions without using the Henderson-Hasselbalch equation. Please show all calculations.
Question #1
A student dissolves 0.25 moles of the acid HA in water and dilutes the solution to the final volume of 500 mL. The student then gives a small portion of the solution to her professor. The professor uses a pH meter

Please see attached file for full problem description.
1. Find the concentration of the hydrogen peroxide solution.
Doing an analysis of hydrogen peroxide using Potassium Permangate
Equation is:
2KMnO4(aq)+5H2O2(aq)+3H2SO4(aq) -->5O(g)+K2SO4(aq)+2MnSO4(aq)+8H2O(l)
Potassium Permangate is the titrant.
Obtained a 1.00mL al

1. Consider a lake containing 39 ppb (parts per billion) of parathion, which has a log Kow = 3.8.
a. If a sample of lake water was mixed with octanol, what is the expected concentration of parathion in the octanol?
b. Assuming the body weight of a fish is 4% fat, what is the equilibrium concentration of parathion in the f

For the second order reaction below, the initial concentration of A is 1.34M. If k=7.61x10(exponent negative 4) seconds(exponent negative 1), what is the concentration of A after 18.3 minutes?
2A-->B rate=k[A](exponent2)