Question

If the Ka of a monoprotic weak acid is 7.5 × 10-6, what is the pH of a 0.12 M solution of this acid?

Answer #1

Lets write the acid as HA

Lets write the dissociation equation of HA

HA -----> H+ + A-

0.12 0 0

0.12-x x x

Ka = [H+][A-]/[HA]

Ka = x*x/(c-x)

Assuming small x approximation, that is lets assume that x can be ignored as compared to c

So, above expression becomes

Ka = x*x/(c)

so, x = sqrt (Ka*c)

x = sqrt ((7.5*10^-6)*0.12) = 9.487*10^-4

since c is much greater than x, our assumption is correct

so, x = 9.487*10^-4 M

so,

[H+] = x = 9.487*10^-4 M

we have below equation to be used:

pH = -log [H+]

= -log (9.487*10^-4)

= 3.02

Answer: 3.02

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the
pH of a 0.12 M solution of this acid?

If the Ka of a monoprotic weak acid is 3.3 × 10-6, what is the
pH of a 0.30 M solution of this acid?

If the Ka of a monoprotic weak acid is 5.7 × 10-6, what is the
pH of a 0.14 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
pH of a 0.43 M solution of this acid?

If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the
pH of a 0.50 M solution of this acid?

1.) If the Ka of a monoprotic
weak acid is 4.5 x 10^-6, what is the pH of a 0.30M solution of
this acid?
2.) The Ka of a monoprotic weak
acid is 7.93 x 10^-3. What is the percent ionization of a 0.170 M
solution of this acid?
3.) Enolugh of a monoprotic acid
is dissolved in water to produce a 0.0141 M solution. The pH of the
resulting solution is 2.50. Calculate the Ka for the
acid.

a. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.1×10−5.
b.Find the percent dissociation of this solution.
c. Find the pH of a 0.100 M solution of a weak
monoprotic acid having Ka= 1.8×10−3
d. Find the percent
dissociation of this solution.
e.Find the
pH of a 0.100 M solution of a weak monoprotic
acid having Ka= 0.16.
f.Find the percent dissociation of this solution.

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the
[H ] of a 0.27 M solution of this acid?

1. The Ka of a monoprotic weak acid is 5.90 × 10-3. What is the
percent ionization of a 0.148 M solution of this acid?
2. If the Kb of a weak base is 4.5 × 10-6, what is the pH of a
0.26 M solution of this base?
3. Assuming complete dissociation, what is the pH of a 3.00 mg/L
Ba(OH)2 solution?

The Ka of a monoprotic weak acid is 6.69 × 10-3. What is the
percent ionization of a 0.158 M solution of this acid?

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