What Is the Ph of a 3.5x10-11 M H+ Solution
Assignment 026
Question 1
What is the pH of a solution where [H3O +] = 5.2x10-2?
Question 2
What is the pH of a solution where [OH-] = 3.4x10-12?
Question 3
What is the pOH of a solution where [OH-] = 5.9x10-8?
Question 4
What is the [H3O +] in a solution with a pH of 9.45?
Question 5
What is the [
Question 6
What is the [
Question 7
What is the [H3O +] in a solution where [
ANSWERS
Question 1 (00000001B0402400, Variation No. 70): 1.28
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An alternative method of specifying the acidity of a solution is by using the term called pH (for the "power of the hydrogen ion")
pH = - log10 [H+] = - log10 [H3O +]
The lower the pH, the more acidic the solution.
In this problem,
pH = - log10 [H3O +] = - log10 [5.2x10-2] = 1.28
Question 2 (00000001B0402401, Variation No. 53): 2.53
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An alternative method of specifying the acidity of a solution is by using the term called pH (for the "power of the hydrogen ion")
pH = - log10 [H+] = - log10 [H3O +]
The lower the pH, the more acidic the solution.
In this problem, we are given the [
] not the [H3O + ] ; therefore, there are several ways to obtain the correct answer. The easiest method is to combine the following two equations into one simple equation:
14.00 = pH + pOH
pOH = - log10 [OH-]
rearranging the first equation for pH and substituting the second equation for pOH in the first we obtain
pH = 14.00 + log[OH-] = 14.00 + log[3.4x10-12] = 2.53
Note: This is a useful equation to remember that converts [OH-] to pH quite easily.
Question 3 (00000001B0402402, Variation No. 57): 7.23
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An alternative method of specifying the acidity of a solution is by using the term called pH (for the "power of the hydrogen ion")
pH = - log10 [H+] = - log10 [H3O +]
A similar approach is used for the hydroxide ion concentration. The pOH of a solution is defined as
pOH = - log10 [
]
In this problem,
pOH = - log10 [
] = - log10 [5.9x10-8] = 7.23
Question 4 (00000001B0402403, Variation No. 28): 3.5x10-10 M
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An alternative method of specifying the acidity of a solution is by using the term called pH (for the "power of the hydrogen ion")
pH = - log10 [H+] = - log10 [H3O +]
[H3O +] = [H+] = 10-pH
In this problem,
[H3O +] = 10-9.45 = 3.5x10-10 M
Question 5 (00000001B0402404, Variation No. 30): 7.6x10-8 M
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In this problem we are given the pH but want the [
]. To obtain this value, we will need to convert the pH to pOH by rearranging the following equation
14.00 = pH + pOH
pOH = 14.00 - pH = 14.00 - 6.88 = 7.12
Next, we will calculate the [
] using the following equation
[
] = 10-pOH = 10-7.12 = 7.6x10-8 M
Question 6 (00000001B0402405, Variation No. 77): 1.86x10-6 M
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There is an inverse relationship between [
] and [H3O +] through the ionization of water. The equilibrium constant expression is
Kw = [H3O + ][
] = 1.00 x 10-14 @25oC
where Kw is referred to as the ionization constant for water. Plugging in the given concentration for hydronium and rearranging for the concentration of hydroxide we obtain
[
] = 1.00 x 10-14 / 5.37x10-9 = 1.86x10-6 M
Question 7 (00000001B0402406, Variation No. 1): 1.29x10-8 M
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There is an inverse relationship between [
] and [H3O +] through the ionization of water. The equilibrium constant expression is
Kw = [H3O + ][
] = 1.00 x 10-14 @25oC
where Kw is referred to as the ionization constant for water. Plugging in the given concentration for hydroxide and rearranging for the concentration of hydronium we obtain
[H3O +]= 1.00 x 10-14 / 7.75x10-7 = 1.29x10-8 M
What Is the Ph of a 3.5x10-11 M H+ Solution
Source: http://www.faculty.sfasu.edu/janusama/Assignment026.htm