What is the pH of a solution made by mixing 500 mL of 1.00 M HCN
and 1.50 L of 0.250 M NaOH, and then diluting the entire solution
to a volume of 3.00 L? (Ka HCN = 4.0 x 10-10)
A.
8.92
B. 6.52
C.
9.88
D.
9.27
E.
5.08
To obtain one litre of a solution of pH = 7, you should dissolve
in water
A.
Two mol of HI + two mol of CH3NH2
B.
One mol...
A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and
100 mL of .001 M NaF. Will PbF2(s) precipitate in this reaction?
Calculate the concentration of F- ions present at equilibrium.
PbF2(s) <--> Pb2+(aq) + 2F-(aq) Kc= 3.7E-8
Please show all work! Thank you!
Consider a solution made by mixing 500.0 mL of 0.03158 M
Na2HAsO4 with 500.0 mL of 0.04202 M NaOH. Complete the mass balance
expressions below for Na and arsenate species in the final
solution.
[Na+] = ____ M
[HAsO42-] + [__] + [__] + [__] = ____ M
100 mL of LiOH(aq) (0.500 M) is reacted with 250 mL of sulfuric
acid solution (0.200 M). Consider the following statements;
i) This is an example of a strong acid-strong base
neutralization reaction.
ii) LiOH(aq) is the limiting reagent and produces 0.05 moles of
water
iii) The final concentration of Li+ (aq) in the mixture would be
0.071 M
a. Only statement i is correct.
b. Only statement ii is correct.
c. Only statement iii is correct.
d. Statements i...
10. What is the [CH3COOH ]/[CH3COO– ] ratio in an acetic
acid/sodium acetate buffer at pH = 4.90? (Ka = 1.8 x 10–5 )
a. 0.31
b. 0.70
c. 1.45
d. 2.41
e. 4.90
11. How many grams of NaCH3COO should be added to 250 mL of
0,100 M CH3COOH when the above solution is prepared?
a. 0.431 g
b. 2.95 g
c. 5.66 g
d. 1.43 g
e.11.9 g
CH3COOH yields CH3COO- +
H+
If NaCH3COO is added to the solution then…
Will the concentration of H+ will
increase/decrease/same? Why?
Will the concentration of CH3COOH will
increase/decrease/same? Why?
Will the concentration of OH- will increase/decrease/same?
Why?
Will pKa will increase/decrease/same? Why?