Question 1

From the information given below which one of the 5 solutions would be the most acidic?

Accepted Answer

A lower pOH indicates a higher concentration of hydroxide ions, which means a lower pH and a more acidic solution. Therefore, the solution with a pOH of 12 would be the most basic, leaving option E as the most acidic.

Question 2

The pH of a certain black coffee is 5.3. What is its hydroxide ion concentration, [OH^-]?

Accepted Answer

The pH of the coffee is 5.3, which means the pOH is 14 - 5.3 = 8.7. The hydroxide ion concentration, [OH⁻], is 10^(-pOH) = 10^(-8.7) ≈ 2.0×10^(-9) M.

Question 3

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s). Refer to Exhibit 15-2. What is the hydroxide ion concentration, [OH^-], of this solution?

Accepted Answer

The answer of Exhibit 15-2 The pH of a solution...

Question 4

What is the H₃O⁺ ion concentration in an aqueous solution having an OH^- concentration of 1.0×10^{- 2} M?

Accepted Answer

The given chemical formula H₃O⁺ contains three types of ions: H₃O- (which we can simplify to HSO4-), H+, and OH-. The concentration of HSO4- is not relevant to the question, so we can ignore it. Since the concentration of OH- is given as 1.0×10^{- 2} M, we can use the self-ionization constant of water to find the concentration of H+. At room temperature, Kw = 1.0×10^{- 14}, and we know that [OH-][H+] = Kw. Substituting in the given [OH-], we get: [OH-][H+] = 1.0×10^{- 14} (1.0×10^{- 2})([H+]) = 1.0×10^{- 14} ([H+]) = 1.0×10^{- 14} / (1.0×10^{- 2}) ([H+]) = 1.0×10^{- 12} M Therefore, the concentration of H+ is 1.0×10^{- 12} M, which is answer choice D.

Question 5

Which of the following aqueous solutions is(are) considered basic ? I. [H₃O⁺] = 3.4×10^{- 10} M II. pH = 8.54 III. [OH^-] = 6.7×10^{- 4} M

Accepted Answer

The answer of Which of the following aqueous solutions is(are)...

Question 6

Which of the following aqueous solutions is(are) considered acidic ? I. A solution with [OH^-] = 2.5×10^{- 8} II. A solution with [H₃O⁺] = 1×10^{- 7} III. A solution with a pOH = 8

Accepted Answer

To determine if a solution is acidic, we need to consider the concentration of hydrogen ions ([H+]) or the pOH value. For a solution to be acidic, its pH must be less than 7, or equivalently, its pOH must be greater than 7 (since pH + pOH = 14 at 25°C).I. A solution with [OH-] = 2.5×10^-8 M. To find if it's acidic, we need to calculate the pOH and then the pH. However, without doing the calculations, knowing that the [OH-] is low suggests it's not a basic solution, but we can't directly infer it's acidic without comparing it to the [H+].II. A solution with [H3O+] = 1×10^-7 M. This concentration of hydronium ions corresponds to a neutral solution at 25°C, as pure water has [H3O+] = 1×10^-7 M. However, any slight increase in [H3O+] would make the solution acidic, but based on this value alone, it's at the border between neutral and acidic.III. A solution with a pOH = 8. Since pOH + pH = 14, a pOH of 8 means the pH is 6, which is less than 7. Therefore, this solution is acidic.Given the information, the correct choices are I and III, as they are the ones that can be considered acidic based on the provided data.

Question 7

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH^-] present in this solution?

Accepted Answer

The pH of the solution can be used to calculate the concentration of [H+]: 
pH = -log[H+]
3.12 = -log[H+]
[H+] = 8.63x10^-4 M

Since this is a Coca Cola solution, we can assume that there is negligible presence of other acidic or basic compounds. Therefore, the [OH-] concentration can be calculated using the Kw expression: 
Kw = [H+][OH-] = 1x10^-14
[OH-] = Kw/[H+]
[OH-] = 1.16x10^-11 M

Therefore, the concentration of [OHS-] can be calculated using the following equation: 
[OHS-] + [OH-] = [H2O]
[OHS-] = [H2O] - [OH-]
Assuming that the volume of the solution is 1 L, the concentration of water is approximately 55.6 M. 
[OHS-] = 55.6 M - 1.16x10^-11 M
[OHS-] = 55.6 M

However, since the [OHS-] concentration is much larger than the [OH-] concentration, we can assume that the [OHS-] concentration is equal to the total concentration of solutes in the solution. Therefore, the concentration of [OHS-] is approximately 55.6 M.

The correct answer is C: [OHS-] = 1.3x10^-11 M.

Question 8

A solution is found to have a pH of 10.45. What is [H₃O⁺]?

Accepted Answer

To find the concentration of the hydrogen sulfide ion [HS-], we need to use the pH and the dissociation constant (pKa) of hydrogen sulfide. 
pH = pKa + log([HS-]/[H2S]) 
10.45 = 7.0 + log([HS-]/[H2S]) 
log([HS-]/[H2S]) = 3.45 
[HS-]/[H2S] = 3.5 x 10^-4

Since the solution is basic, we can assume that [OH-] is significantly greater than [H+], therefore:
[H2S] ≈ [HS-] + [S2-]

We don't have information to calculate the concentration of sulfide ion [S2-]. However, we can assume that it is negligible compared to [HS-] and [H2S], so:
[H2S] ≈ [HS-]

[HS-] + [H2S] = 1 M 
Substituting [HS-]/[H2S] = 3.5 x 10^-4, we get:

[HS-] + 3.5 x 10^-4 [HS-] = 1 M 
[HS-] (1 + 3.5 x 10^-4) = 1 M 
[HS-] = 1 / (1 + 3.5 x 10^-4) = 2.8 x 10^-4 M

Finally, since we are not given any other species besides HS-, the answer is [HS-] = 2.8 x 10^-4 M.

Question 9

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H₃O⁺], for this solution?

Accepted Answer

The pH of a solution is defined as the negative logarithm of the hydronium ion concentration, so we can use the following equation to find the hydronium ion concentration:

pH = -log[H3O+]

2.32 = -log[H3O+]

log[H3O+] = -2.32

[H3O+] = 10^-2.32

[H3O+] = 4.8 x 10^-3 M

Therefore, choice B is correct.

Question 10

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s). -Refer to Exhibit 15-1. What is the molar concentration of the hydronium ion , [H₃O⁺], in this milk?

Accepted Answer

The molar concentration of the hydronium ion, [H3O+], in a solution is given by 10^(-pH). For a pH of 6.60, [H3O+] = 10^(-6.60) = 2.5×10^-7 M.

Question 11

Measurements show that the [OH^-] of a solution is 6.02×10^{- 6} M. The pH of this solution is:

Accepted Answer

The pOH of the solution is calculated using the formula pOH = -log[OH⁻]. Substituting the given concentration, pOH = -log(6.02×10⁻⁶) ≈ 5.22. Since pH + pOH = 14, the pH = 14 - 5.22 = 8.78.

Question 12

The hydroxide ion concentration in a solution with pH = 3.50 is:

Accepted Answer

The pH of the solution is 3.50, which means the pOH is 14 - 3.50 = 10.50. The hydroxide ion concentration is then 10^(-10.50) M, which is approximately 3.2×10^(-11) M.

Question 13

The hydronium ion concentration, [H₃O⁺], for a certain brand of beer is 3.16×10^{- 5} M. What is the pOH of this aqueous solution?

Accepted Answer

To find the pOH, first calculate the pH using the formula pH = -log[H3O+]. Then, use the relation pH + pOH = 14 to find the pOH. Here, pH = -log(3.16×10^-5) ≈ 4.50, so pOH = 14 - 4.50 = 9.50.

Question 14

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s).
Refer to Exhibit 15-2. What is the pOH of this solution?

Accepted Answer

The pOH of a solution can be found using the relationship pH + pOH = 14. Given the pH is 2.27, pOH = 14 - 2.27 = 11.73.

Question 15

The pH of a solution is 5. The [H₃O⁺] and [OH^-] are:

Accepted Answer

The pH of a solution is a measure of the hydrogen ion concentration, [H+]. A pH of 5 means [H+] = 10^-5 M. The concentration of hydroxide ions, [OH-], can be found using the water dissociation constant (Kw = 10^-14 at 25°C), so [OH-] = Kw / [H+] = 10^-14 / 10^-5 = 10^-9 M.

Question 16

The pH of a certain specimen of urine is 4.8. What is the hydroxide ion concentration, [OH^-], of this solution?

Accepted Answer

The pH of the urine specimen is 4.8, which means the hydrogen ion concentration ([H+]) is 10^-4.8 M. 
Using the equation for the dissociation of water, we can find the hydroxide ion concentration ([OH-]):
Kw = [H+][OH-] 
1.0 x 10^-14 = (10^-4.8)[OH-] 
[OH-] = (1.0 x 10^-14) / (10^-4.8) 
[OH-] = 6.3 x 10^-11 M 
Therefore, the hydroxide ion concentration is 6.3 x 10^-11 M, which corresponds to choice B.

Question 17

If the pH of a solution is 4.40:

Accepted Answer

The answer of If the pH of a solution is...

Question 18

Which of the following aqueous solutions is(are) considered basic ? I. [OH^-] = 6.2×10^{- 8} II. [H₃O⁺] = 3.8×10^{- 12} III. pOH = 2.5

Accepted Answer

Option I has a pH value of 7.2 (using the formula pH = 14 - pOH), which is neutral. Option II has a pH value of 10.2, which is basic. Option III has a pOH value of 11.5, which corresponds to a pH of 2.5 (using the formula pH = 14 - pOH), which is acidic. Therefore, only Option II and Option III are basic aqueous solutions. The answer is D.

Question 19

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s). -Refer to Exhibit 15-1. What is the molar concentration of hydroxide ion , [OH^-], in this milk?

Accepted Answer

The pH of the milk is 6.60, so the pOH is 14 - 6.60 = 7.40. The hydroxide ion concentration, [OH⁻], is 10^(-pOH) = 10^(-7.40) ≈ 4.0×10^(-8) M.

Question 20

A famous brand of sweet and sour barbecue sauce (consisting of tomato paste, water, vinegar, sugar, and secret spices) has a measured pH of 2.6. What is the hydrogen ion concentration in the sauce?

Accepted Answer

The pH is the negative logarithm of the hydrogen ion concentration. A pH of 2.6 corresponds to a hydrogen ion concentration of 10^(-2.6) M, which is approximately 2.5×10^(-3) M.

Quiz 15: Solutions of Acids and Bases

From the information given below which one of the 5 solutions would be the most acidic?

The pH of a certain black coffee is 5.3. What is its hydroxide ion concentration, [OH^-]?

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s) . Refer to Exhibit 15-2. What is the hydroxide ion concentration, [OH^-], of this solution?

What is the H₃O⁺ ion concentration in an aqueous solution having an OH^- concentration of 1.0×10^{- 2} M?

Which of the following aqueous solutions is(are) considered basic ? I. [H₃O⁺] = 3.4×10^{- 10} M II. pH = 8.54 III. [OH^-] = 6.7×10^{- 4} M

Which of the following aqueous solutions is(are) considered acidic ? I. A solution with [OH^-] = 2.5×10^{- 8} II. A solution with [H₃O⁺] = 1×10^{- 7} III. A solution with a pOH = 8

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH^-] present in this solution?

A solution is found to have a pH of 10.45. What is [H₃O⁺]?

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H₃O⁺], for this solution?

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of the hydronium ion , [H₃O⁺], in this milk?

Measurements show that the [OH^-] of a solution is 6.02×10^{- 6} M. The pH of this solution is:

The hydroxide ion concentration in a solution with pH = 3.50 is:

The hydronium ion concentration, [H₃O⁺], for a certain brand of beer is 3.16×10^{- 5} M. What is the pOH of this aqueous solution?

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s) . Refer to Exhibit 15-2. What is the pOH of this solution?

The pH of a solution is 5. The [H₃O⁺] and [OH^-] are:

The pH of a certain specimen of urine is 4.8. What is the hydroxide ion concentration, [OH^-], of this solution?

If the pH of a solution is 4.40:

Which of the following aqueous solutions is(are) considered basic ? I. [OH^-] = 6.2×10^{- 8} II. [H₃O⁺] = 3.8×10^{- 12} III. pOH = 2.5

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of hydroxide ion , [OH^-], in this milk?

A famous brand of sweet and sour barbecue sauce (consisting of tomato paste, water, vinegar, sugar, and secret spices) has a measured pH of 2.6. What is the hydrogen ion concentration in the sauce?

Quiz 15: Solutions of Acids and Bases

From the information given below which one of the 5 solutions would be the most acidic?

The pH of a certain black coffee is 5.3. What is its hydroxide ion concentration, [OH - ]?

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s) . Refer to Exhibit 15-2. What is the hydroxide ion concentration, [OH - ], of this solution?

What is the H3O+ ion concentration in an aqueous solution having an OH - concentration of 1.0×10 - 2 M?

Which of the following aqueous solutions is(are) considered basic ? I. [H3O+] = 3.4×10 - 10 M II. pH = 8.54 III. [OH - ] = 6.7×10 - 4 M

Which of the following aqueous solutions is(are) considered acidic ? I. A solution with [OH - ] = 2.5×10 - 8 II. A solution with [H3O+] = 1×10 - 7 III. A solution with a pOH = 8

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH - ] present in this solution?

A solution is found to have a pH of 10.45. What is [H3O+]?

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H3O+], for this solution?

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of the hydronium ion , [H3O+], in this milk?

Measurements show that the [OH - ] of a solution is 6.02×10 - 6 M. The pH of this solution is:

The hydroxide ion concentration in a solution with pH = 3.50 is:

The hydronium ion concentration, [H3O+], for a certain brand of beer is 3.16×10 - 5 M. What is the pOH of this aqueous solution?

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s) . Refer to Exhibit 15-2. What is the pOH of this solution?

The pH of a solution is 5. The [H3O+] and [OH - ] are:

The pH of a certain specimen of urine is 4.8. What is the hydroxide ion concentration, [OH - ], of this solution?

If the pH of a solution is 4.40:

Which of the following aqueous solutions is(are) considered basic ? I. [OH - ] = 6.2×10 - 8 II. [H3O+] = 3.8×10 - 12 III. pOH = 2.5

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of hydroxide ion , [OH - ], in this milk?

A famous brand of sweet and sour barbecue sauce (consisting of tomato paste, water, vinegar, sugar, and secret spices) has a measured pH of 2.6. What is the hydrogen ion concentration in the sauce?

The pH of a certain black coffee is 5.3. What is its hydroxide ion concentration, [OH^-]?

Exhibit 15-2 The pH of a solution of a certain brand of Cola is 2.27. Use this information to solve the following problem(s) . Refer to Exhibit 15-2. What is the hydroxide ion concentration, [OH^-], of this solution?

What is the H₃O⁺ ion concentration in an aqueous solution having an OH^- concentration of 1.0×10^{- 2} M?

Which of the following aqueous solutions is(are) considered basic ? I. [H₃O⁺] = 3.4×10^{- 10} M II. pH = 8.54 III. [OH^-] = 6.7×10^{- 4} M

Which of the following aqueous solutions is(are) considered acidic ? I. A solution with [OH^-] = 2.5×10^{- 8} II. A solution with [H₃O⁺] = 1×10^{- 7} III. A solution with a pOH = 8

The pH of a diet Coca Cola solution is 3.12. What is the concentration of [OH^-] present in this solution?

A solution is found to have a pH of 10.45. What is [H₃O⁺]?

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H₃O⁺], for this solution?

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of the hydronium ion , [H₃O⁺], in this milk?

Measurements show that the [OH^-] of a solution is 6.02×10^{- 6} M. The pH of this solution is:

The hydronium ion concentration, [H₃O⁺], for a certain brand of beer is 3.16×10^{- 5} M. What is the pOH of this aqueous solution?

The pH of a solution is 5. The [H₃O⁺] and [OH^-] are:

The pH of a certain specimen of urine is 4.8. What is the hydroxide ion concentration, [OH^-], of this solution?

Which of the following aqueous solutions is(are) considered basic ? I. [OH^-] = 6.2×10^{- 8} II. [H₃O⁺] = 3.8×10^{- 12} III. pOH = 2.5

Exhibit 15-1 The pH of a certain brand of milk is 6.60. Use this information to answer the following question(s) . -Refer to Exhibit 15-1. What is the molar concentration of hydroxide ion , [OH^-], in this milk?