Titration of 25.00 mL of a 7.35*10^-2M Phosphoric acid solution
with a secondary NaOH solution with concentration of .1225M. What
is the pH after the following addition of NaOH?
a. 10mL
b. 15mL
Calculate the pH change when 10. mL of 3.0 M NaOH is added to
500. mL of the following:
(a) pure water
(b) 0.10 M CH3COO-
(c)0.10 M CH3COOH
(d)a solution that is 0.10 M CH3COO- and 0.10 M CH3COOH
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300
M HCl. The solution was then treated with an excess of aqueous
chromium(III) nitrate, resulting in formation of 2.36 g of
precipitate. Determine the concentration of the solution.
(a) How many mL of a 0.1 N
solution of NaOH must be added to a 25 mL solution of 0.1 N
Acetic Acid to obtain a pH of 9.75? What is the concentration
of Acetic Acid at this pH?
(b) Answer the same question with the following changes: [Acetic
Acid] = 0.01 N in25mL and the normality of the titrant is
0.02 N. The final pH is 11.
(c) What are the alkalinity and
acidity of a water that...
Calculate the volume of 0.5M solution of NaOH that need to be
added to 100 mL of 0.2M solution of H3PO4 to get pH = 3. Calculate
the ionic strength of resulting solution?
A solution is made by mixing exactly 500 mL of 0.153 M
NaOH with exactly 500 mL of 0.100 MCH3COOH.
Calculate the equilibrium concentration of the species below.
Ka of CH3COOH is 1.8
×10−5
[H+]=? M
[OH-]=? M
[CH3COOH]=? M
[Na+]=? M
[CH3COO−]=? M
A solution is made by mixing exactly 500 mL of 0.149 M NaOH with
exactly 500 mL of 0.100 M CH3COOH. Calculate the equilibrium
concentration of the species below. Ka of CH3COOH is 1.8 X 10-5
[H+], [OH-], [CH3COOH], [Na+], [CH3COO-} enter answer in
scientific notation.