A solution is made by mixing 25.0 mL of 0.250 M nitric acid
(HNO3) with 15.0...
A solution is made by mixing 25.0 mL of 0.250 M nitric acid
(HNO3) with 15.0 mL of 0.500 M sodium hydroxide (NaOH). What is the
resulting concentration of each ion in solution?
A. A solution is made by combining 15.0 mL of 18.5 M acetic acid
with 5.50 g of sodium acetate and diluting to a total volume of
1.50 L. Calculate the pH of the solution.
B.A 115.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3
is mixed with a 225.0 −mL sample of a solution that is 0.14 M in
NaCN. After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
A nitric acid solution is composed of 63.75 g of HNO3 and 205.65
mL of pure water. What is the percent by mass of the nitric acid
solution? Use the density of water as 0.9984 g/mL.
A solution is made by combining 15.0 mL of 16.5 M acetic acid
with 5.50 g of sodium acetate and diluting to a total volume of
1.50 L.
Calculate the pH of the solution.
A solution is made by combining 15.0 mL of 17.0 M acetic acid
with 5.50 g of sodium acetate and diluting to a total volume of
1.50 L.
what is the pKa?
what is the pH?
A 280.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M
in sodium acetate. For acetic acid, Ka=1.8×10−5.
Part A) What is the initial pH of this solution?
Part B) What is the pH after addition of 0.0150 mol
of HCl?
Part C) What is the pH after addition of 0.0150 mol
of NaOH?
20.0 mL of nitric acid (HNO3) solution is neutralized with 30.0
mL 0.10M of potassium hydroxide (KOH) solution. what is the
concentration of nitric acid solution? The answer is 0.67 M but how
do you get that?
A solution is made by mixing 12.5
g of Sr(OH)2and 40.0 mL of 0.200 M HNO3.
a. Calculate the
concentration of OH− ion remaining in solution.
b.Calculate the concentration of Sr2+ ion remaining in
solution.
c.Calculate the concentration of NO−3 ion remaining in
solution.
d. Is the resultant solution acidic or basic?
A solution is made by mixing 30.0 mL of 0.150M (mol/L) compound
A with 25.0 mL of 0.200M (mol/L) compound B. At equilibrium, the
concentration of C is 0.0454M. Calculate the equilibrium constant,
K, for this reaction.
A (aq) + 2B (aq) <---> C (aq)
Consider the titration of 25.0 mL of 0.175 M cyanic
acid, HCNO, with 0.250 M LiOH. The Ka of HCNO is 3.5 * 10^-4.
What is the volume of LIOH required to reach the
equivalence point?
b. calculate the pH after the following volumes of LIOH have been
added:
a. 0mL
b. 5.0 mL
c. 8.75 mL
d. 17.5 mL