In: Chemistry

1. Calculate [H3O+] in the following aqueous solution at 25 C:
[OH−]=1.1×10^{−9} M.

2. Calculate [H3O+] in the following aqueous solution at 25 C:
[OH−]=2.4×10^{−2} M .

3. Calculate [H3O+] in the following aqueous solution at 25 C:
[OH−]=6.2×10^{−12} M

then classify the solutions as acidic or basic.

1)

.[OH^{-}] = 1.1 X 10^{-9} M

we know the equation

K_{w} = .[OH^{-}] X
[H_{3}O^{+}]

where, K_{w} = 1.0 X 10^{-14}

then

[H_{3}O^{+}] = K_{w} /
[OH^{-}]

substitute the value

[H_{3}O^{+}] = 1.0 X 10^{-14}/ 1.1 X
10^{-9} = 9.09 X 10^{-6} M

**[H _{3}O^{+}] = 9.09 X 10^{-6}
M**

pH = - log[H_{3}O^{+}] = -log(9.09 X
10^{-6} ) = 5.04

Solution is **acidic** because pH from 0 to 7 is
acidic

2)

.[OH^{-}] = 2.4 X 10^{-2} M

we know the equation

K_{w} = .[OH^{-}] X
[H_{3}O^{+}]

where, K_{w} = 1.0 X 10^{-14}

then

[H_{3}O^{+}] = K_{w} /
[OH^{-}]

substitute the value

[H_{3}O^{+}] = 1.0 X 10^{-14}/ 2.4 X
10^{-2} = 4.167 X 10^{-13} M

**[H _{3}O^{+}] = 4.167 X 10^{-13}
M**

pH = - log[H_{3}O^{+}] = -log(4.167 X
10^{-13} ) = 12.38

Solution is **basic** because pH from 7 to 14 is
basic

3)

.[OH^{-}] = 6.2 X 10^{-12} M

we know the equation

K_{w} = .[OH^{-}] X
[H_{3}O^{+}]

where, K_{w} = 1.0 X 10^{-14}

then

[H_{3}O^{+}] = K_{w} /
[OH^{-}]

substitute the value

[H_{3}O^{+}] = 1.0 X 10^{-14}/ 6.2 X
10^{-12} = 1.61 X 10^{-3} M

**[H _{3}O^{+}] = 1.61 X
10^{-3} M**

pH = - log[H_{3}O^{+}] = -log(1.61 X
10^{-3} ) = 2.79

Solution is **acidic** because pH from 0 to 7 is
acidic

A.
Calculate [H3O+] in the following aqueous solution at 25 ?C:
[OH?]= 1.6×10?9 M .
Express your answer using two significant figures.
B.
Calculate [H3O+] in the following aqueous solution at 25 ?C:
[OH?]= 3.0×10?2 M .
Express your answer using two significant figures.
C.
Calculate [H3O+] in the following aqueous solution at 25 ?C:
[OH?]= 7.0×10?12 M .
Express your answer using two significant figures.

Calculate the [H3O+] of each aqueous solution with the following
[OH-]. 1) NaOH, 1.6x10^2 M. 2) milk of magnesia, 1.0x10^-5 M. 3)
aspirin, 2.2x10^-11 M. 4) seawater, 2.5x10^-6 M.

Calculate [H3O ], [ClO4–], and [OH–] in an aqueous solution that
is 0.130 M in HClO4(aq) at 25 °C.
[H^+]=
[ClO4^-]=
[OH^-]=
Is the solution acidic, basic or neutral?

1.Calculate the [H3O+] value of each aqueous solution.
aspirin with [OH−]=1.4×10−11M.
seawater with [OH−]=1.5×10−6M
2. To calculate pH and use it as a measure of
acidity.
What is the pH of an aqueous solution with [H3O+] =
4×10−13M ?
Carbonated cola is more acidic than coffee or even orange juice
because cola contains phosphoric acid.
What is the molar concentration of H3O+ in a cola that has a pH
of 3.120?

Calculate the [OH−] of each aqueous solution with the following
[H3O+]:
1)stomach acid, 5.0×10−2M. Express your answer using two
significant figures.
2)urine, 3.0×10−6M. Express your answer using two significant
figures.
3)orange juice, 1.6×10−4M. Express your answer using two
significant figures.
4)bile, 6.0×10−9M.Express your answer using two significant
figures.

Calculate the [OH−] of each aqueous solution with the following
[H3O+]:
stomach acid, 2.0×10−2M Express your answer using two
significant figures.
urine, 7.0×10−6M Express your answer using two significant
figures.
orange juice, 2.2×10−4M Express your answer using two
significant figures.
bile, 6.0×10−9M Express your answer using two significant
figures.

Calculate the [H3O+] of each aqueous solution with the following
[OH−] . Express your answer using two significant figures.
1.Vinegar, 1.2 x 10-11M, Express your answer using
two significant figures.
2. Urine, 2.3x10-9 M, Express your answer using two
significant figures.
3. Ammonia, 5.8×10−3 M, Express your answer using two
significant figures.
4. NaOH, 4.0×10−2 M, Express your answer using two
significant figures.

Calculate [H3O+] and [OH−] for each of the following solutions
at 25 ∘C given the pH.
Part A.) pH= 8.65
Part B.) pH= 11.40
Part C.) pH= 2.94

If theres saturated aqueous solution of Fe(OH)2 at 25°C and Ksp
= 4.87 × 10−17, which one is false statement?
A. Adding acid to the solution will increase the solubility.
B. Fe(OH)2 is a strong electrolyte.
C. The pH of the solution will be greater than 7.
D. The solubility of the salt will be equal to [OH−].
E. Addition of more solid Fe(OH)2 to the solution will increase
the hydroxide ion concentration.
Whats pH of saturated solution of Mg(OH)2?...

Formic acid (HCOOH) is secreted by ants. Calculate
[H3O+] for a 4.98E-2 M aqueous solution of
formic acid (Ka = 1.80E-4).

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