1)calculate the pH of 0.154 M solution of a monoprotic acid with
ka= 1.65x10^-8
2)A solution of B-, a weak base , has a pH of 10.90.what is
the molarity of B- if kb=3.24 x 10^-5
1. What is the pH of a solution with 15 mL of 0.5 M acetic acid
and 15 mL of 0.5 M sodium acetate in solution.
2. What is the pH if we were to take 5 mL of the above solution
and add it to 25 mL of water.
Please explain and work all steps.
What is the pH of a solution that is 0.0924 M in malonic acid?
What will be the equilibrium concentration of each of the three
malonic acid species? pKa1 = 2.85 pKa2 = 5.70
pH: _________________
[H2A]: ____________________ [HA-]: _________________ [A2-]:
_________________
What is the structure of
1. palmatic acid and 2-oleoyl-3-phosphatidylserine
2. oleic acid and 1-palmitoyl-3-phosphatidylserine
3. phosphoserine and 1-palmitoyl-2-oleoyl-glycerol
4. serine and 1-palmitoyl-2-oleoyl-phosphatidic acid
1.A 25.0 L solution is made of 0.10 M acid and 0.13 M conjugate
base. What mass of HNO3 (MM = 63.01) in grams can the
buffer absorb before one of the components is no longer
present?
2. If 147 g of ZnF2 (Ksp=0.0300) is added to water to make a
1.00 L to the solution, what is the [F-] concentration
in the solution in molarity?
3. A solution begins with .100M of NaF dissolved in water. What
is the...
a. A 0.037 M solution of a weak acid is 4.67 percent ionized in
solution. What is the Ka for this acid?
b. The pOH of a 0.29 M weak acid solution is 9.7. What is the Ka
for this weak acid?
1) If 22.0 mL of 2.3 M C2H5NH2
are titrated with 0.9 M HCl, what is the pH at 13.1 mL?
2) If 25.1 mL of 2.2 M CH3COOH are titrated with 0.9
M NaOH, what is the pH at 14.9 mL?
3) Exactly 47.0 mL of 0.2 M HNO2 are titrated with a
0.2 M NaOH solution. What is the pH at the equivalence point ?