9)
use:
Ka = Kw/Kb
Kw is dissociation constant of water whose value is 1.0*10^-14 at
25 oC
Ka = (1.0*10^-14)/Kb
Ka = (1.0*10^-14)/2.5*10^-7
Ka = 4*10^-8
HClO + H2O
-----> ClO- +
H+
0.2
0 0
0.2-x
x x
Ka = [H+][ClO-]/[HClO]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((4*10^-8)*0.2) = 8.944*10^-5
since c is much greater than x, our assumption is correct
so, x = 8.944*10^-5 M
So, [H+] = x = 8.944*10^-5 M
use:
pH = -log [H+]
= -log (8.944*10^-5)
= 4.0485
Answer: 4.05
Only 1 question at a time please
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34/35 A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.122 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made that is 0.365 M in HCN and 0.365...
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6) Calculate the pH of a 0.021 M NaCN solution. [K (HCN) 4.9 x 1010] 6) a A) 5.49 B) 1.68 C) 3.18 D) 7.00 E) 10.82
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Just give me the answers 14) A0.15 M aqueous solution of the weak acid HA at 25.0 °C has a pHi of 5.35. The value of Kg for HA is A) 14 10-10 B) 7.1 10-9 E) 33 104 918-10-5 D) 3.0 10-5 15) The Kg for HON is 49-10-10, What is the value of Kb for CN-? A) 49-10-24 B) 20 10-5 D) 4.9-104 9 4.0 10-6 E) 2.0 109 16) Caleulate the pOH of a 0.0827 M aqueous...