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For each strong base solution, determine [H3O+], [OH−], pH, and pOH. E) 1.7×10−4 M KOH for...

For each strong base solution, determine [H3O+], [OH−], pH, and pOH.

E) 1.7×10−4 M KOH for [OH-0, [H3O+]

F) 1.7×10−4 M KOH for pH, pOH

G) 5.1×10−4 M Ca(OH)2

H) 5.1×10−4 M Ca(OH)2

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Homework Answers

Answer #1

E and F)

[OH-] = [KOH] = 1.7*10^-4 M

use:

[H+] = (1.0*10^-14)/[OH-]

[H+] = (1.0*10^-14)/( 1.7*10^-4)

[H+] = 5.882*10^-11

use:

pH = -log [H+]

= -log (5.882*10^-11)

= 10.2304

use:

pOH = -log [OH-]

= -log (1.7*10^-4)

= 3.7696

Since pH > pOH, this is basic in nature

[H3O+] = 5.882*10^-11

[OH-] = 1.7*10^-4

pH = 10.2304

pOH = 3.7696

G and H)

[OH-] = 2*[Ca(OH)2] = 2*5.1*10^-4 = 0.00102 M

use:

[H+] = (1.0*10^-14)/[OH-]

[H+] = (1.0*10^-14)/0.00102

[H+] = 9.804*10^-12

use:

pH = -log [H+]

= -log (9.804*10^-12)

= 11.0086

use:

pOH = -log [OH-]

= -log (1.02*10^-3)

= 2.9914

Since pH > pOH, this is basic in nature

[H3O+] = 9.804*10^-12

[OH-] = 1.02*10^-3

pH = 11.0086

pOH = 2.9914

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