The pH of 0.1M NaCl is 7.14. After 1 drop of 0.1M HCl
the pH change to 3.59. And after another 1 drop of 0.1M HCl the pH
become 3.13.
Why does pH change significantly 7.14 to 3.59? And also why the pH
doesn't change very much after another 1 drop of 0.1M HCl (3.59 to
3.13)?
A) 7mL of a 0.1M CaCl2 solution was diluted to a final volume of
150mL. Please determine the concentration of Cl- in this
solution.
B) Explain why creating a
standard curve is better than simply using the Beer-Lambert law
directly. Assume that a value for molar absorptivity is readily
available.
QUESTION 10 Calculate the change in pH if 10mL of 0.1M HCl is
added to the buffer made by mixing 25 mL of 1.0 M CH3COOH and 25 mL
of 0.5 M CH3COONa. For these types of questions where a strong acid
or base is added to a buffer solution, first write out the chemical
reaction. What will the HCl react with: CH3COOH or CH3COO−? Since
HCl is an acid, it will react with CH3COO-. Because HCl is a strong...
I) You have an HCl solution of pH 3.13.
(a) The concentration of this solution is ______________ M
(b) If you increased the HCl concentration exactly 2 fold, the
pH would be ______________
(c) If you decrease the pH to 2.13, the new HCl concentration
would be ______________
II) To 20.000 mL of distilled water in a 50 mL beaker, you add
exactly 13 drops of 0.100 M HCl and swirl to mix. If exactly 18
drops of HCl are...
calculate the pH of the following
a) 20.00 mL of 1.40 M HCl diluted to .500 L
b) a mixture formed by adding 44.0 mL of 2.5 × 10^-2 M
HCl to 150 mL of 1.0 ×10^-2 M HI
How you would prepare a 500 mL solution of 0.1M "tris" buffer at
pH of 7.5 starting with solid tris free base. The free base has a
chemical forumla of (HOCH2)3-C-NH2 and a MW of 121.1 g/mol. The
protonated amine form, tris-chloride, has a pKa of 8.10. To prepare
the solution, 1.0M HCl will be used.