As HOMEWORKLIB RULES rule we are allowed to solve maximum 4 parts of any question.
A) ph = -log(H+)
So, Ph increases when H+ decreases.
Ph of HCl = - log( 2.56 * 10^-2)
= 1.59
Ph of HBr = -log(4.09 * 10^-2)
= 1.38
Ph of HCl is lower.
B)
[H+] of weak acid = (Ka * c)^1/2
Ka of formic acid is greater than that of acetic acid.
So H+ of formic acid is higher
So ph of formic acid is lower .
C)
Pkb of CH3NH2 = 3.39
Kb = 4.07 * 10^-4.
Pkb of (CH3)2NH2 = -log kb = -log(5.9 * 10^-4)
= 3.23
[OH-] = (kb * c)^1/2
So, [OH-] of (CH3)2NH2 is higher.
So, POH of (CH3)2NH2 is less
So, Ph of (CH3)2NH2 is high.
D)
Pkb of NH3 = 4.75
Pka of CH3COOH = 4.75
so PKa of NH3 > Pka of CH3COOH
If PKa of CH3COOH is less , so PH of CH3COOH is also less.
please explain and show steps V. 15.102. Predict which solution in each pair below will have...
i just need 103 & 105 please explain fully
15.103. Predict which solution in each pair below will have the a. 1.25 X 10" M HNO3 or 1.00 x 10" M NaOH higher pH. b. 0.345 mM HBrO (PK. = 8.64) or 0.345 mM HCIO 45 mM Be(OH)2 (K = 5 x 10-1) or 45 mM Ba(OH)2 (K. = 2.9 X 10-8) c. d. 1.6 mm (pKs = 8.03) or 0.60 mM (pK6 = 8.32) e. 1.67 X 10-3 M...