1. Find the pH of a 0.030 M barium hydroxide solution.
2. Calculate [H+] at 25oC for a solution
where [OH-] is 1.0 x 10-8 M.
3. In the following reaction, choose the conjugate acid:
HNO3(aq) + H2O(l) --->
H3O+(aq) + NO3-(aq)
A 20.00 mL solution of 0.0840M HOCl is titrated with 0.0560M KOH
solution. Calculate the pH after each of the following additions of
the KOH solution:
a. 15.00mL
b. 30.0mL
c. 32.0mL
4. Calculate the equilibrium constant at standard temperature,
25oC, for the redox reaction between Pb2+(aq) and Zn(s). HINT:
Write a balanced chemical reaction first. a) 1.17x1030 b) 1.92x1021
c) 4.38x1010 d) 1.08x1015 e) 1.75x109
16.29 calculate [H+] for each of the following solution and
indicate whether the solution is acidic, basic, or neutral.(b)
[OH-]= 8.8 * 10-9 M; (c) a solution in which [OH-] is 100 times
greater than [H+] SHOW ALL WORK
Calculate the concentration of H+ in a 0.250 M solution of
oxalic acid. Consider only [H+] from the first ionization. (Ka =
5.37 x 10^-2) Then calculate [H+] of the same solution, including
the H+ ions resulting from the second ionization. (Ka = 5.37 x
10^-5)
Calculate the [H+] in each of the following solutions and
indicate whether the solution is acidic or basic? a) [OH-] = 2.32 X
10^-4 M b)[OH-] = 8.99 x 10^-10 M c) [OH-] = 4.34 x 10^-6 M d)
[OH-] = 6.22 x 10^-12 M
At a temperature other than 25oC, Cd(OH)2
solubility is 5.5 x 10-4 . Calculate it's Ksp at this
temperature.
[ACCORDING TO MY TEXT, Ksp of Cd(OH)2 = 2.5 x
1014 @ 25 C]
A.1.7 x 10-10
B.6.7 x 10-10
C.2.5 x 10-14
Calculate the [H ] and pH of a 0.0045 M hydrazoic acid solution.
Keep in mind that the Ka of hydrazoic acid is 2.20 × 10-5. Use the
method of successive approximations in your calculations or the
quadratic formula.?
[H+] = M?
pH = ?