Which of the following will produce the solution with the lowest
pH?
(A) 0.2 M HCl(B) 0.5 M HF(C) 0.2 M KOH(D)
0.5 M HClO4(E) There is not enough information to
predicT
please help? im kind of lost
1. Calculate the pH of a 0.339 M H2S. Calculate the [S2-] in the
solution.
2. A titration is performed by adding 0.656 M KOH to 40 mL of
0.172 M HNO3:
b) Calculate the pH after the addition of 2.1, 5.25 and 9.49 mL
of the base.(Show your work in detail for one of the volumes.)
e)Calculate the pH after adding 5.00 mL of KOH past the
equivalence point
26.
A solution of 0.075 M CoBr2 is saturated with H2S (
[H2S] = 0.10 M). What is the minimum pH at which CoS ( Ksp = 5.9 x
10 -21) will precipitate?
Ka1 =8.9 x 10 -8 & Ka2 = 1.2 x 10 -13 for H2S and Ksp for CoS =
5.9 x 10 -21
26.
A solution of 0.075 M CoBr2 is saturated with H2S ( [H2S] = 0.10
M). What is the minimum pH at which CoS ( Ksp = 5.9 x 10 -21) will
precipitate?
Ka1 =8.9 x 10 -8 & Ka2 = 1.2 x 10 -13 for H2S Ksp for CoS = 5.9
x 10 -21
8. You have prepared a 0.2 M acetate solution with a pH = 4.76.
Determine the resulting pH when the acids and bases below are added
to the solution. The pKa of CH3COOH is 4.76.
a. 0.025 M HCl
b. 0.050 M HCl
c. 0.025 M NaOH
d. 0.050 M NaOH
e. 0.050 M HCl and 0.025 M NaOH
f. 0.025 M HCl and 0.050 M NaOH
pH and Activity
Calculate the pH of a solution which is 0.0010 M in KOH and 0.013 M
in NaNO3 using activities.
Calculate a pH for the same solution, ignoring
activities
Consider a 1.0 L solution which is 0.40 M
CH3CO2H and 0.2 M
CH3CO2Na (Ka for
CH3CO2H = 1.8 x 10−5). Calculate
the pH of the original soultion, the pH after 0.10 mol of HCl is
added to the original solution, and the pH after 0.20 mol of NaOH
is added to the original solution. Calculate all the pH values to
two decimal places. Assume no volume change on addition. Please
explain and /or show work please.
Given a 0.1 M NH4Cl solution: a) Which is the pH of this
solution? b) If 100 mL of 0.1 M HCl solution are added to 100 mL of
the original solution, which is the pH? c) And if 100 mL of 0.1 M
NH3 are added to 100 mL of the original solution? Data: kb(NH3 ) =
1.8 10^-5 .