At 30.°C, the concentration of hydronium (H3O^+) ions in an aqueous solution is 1.1 ✕ 10^−9 M. (Note: At 30.°C, the ion-product constant for water is 1.46 ✕ 10^−14.)

(a) What is the concentration of hydroxide (OH^−) ions in this solution?

(b)is the solution acidic, basic, or neutral, and why?

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.......2HOH ==> H3O^+ + OH^-
I......liquid..0......0
C......liquid..x......x
E......liquid..x......x

Kw = 1.46E-14 = (H3O^+)(OH^-)
Solve for x = (H3O^+)(OH^-)

Post your work if you get stuck. By the way, look at your answer and tell me, is the solution acidic, basic, or neutral.

To determine the concentration of hydroxide (OH^-) ions in the solution, we can use the ion-product constant for water (Kw) at 30°C.

Given:
[H3O^+] = 1.1 × 10^-9 M
Kw = 1.46 × 10^-14

(a) To find [OH^-], we can use the equation:
Kw = [H3O^+][OH^-]

Let's substitute the known values:
1.46 × 10^-14 = (1.1 × 10^-9)([OH^-])

Now, rearrange the equation to solve for [OH^-]:
[OH^-] = (1.46 × 10^-14) / (1.1 × 10^-9)

Using a calculator, we find that [OH^-] is approximately 1.327 × 10^-6 M.

(b) To determine if the solution is acidic, basic, or neutral, we can compare the concentrations of H3O^+ and OH^- ions.

In this case, the concentration of H3O^+ (1.1 × 10^-9 M) is greater than the concentration of OH^- (1.327 × 10^-6 M).

Since the concentration of H3O^+ ions is greater than OH^- ions, the solution is acidic.

To answer these questions, we need to use the concept of the ion-product constant for water, also known as the Kₐ. The expression for Kₐ is written as:

Kₐ = [H₃O^+][OH^-]

Where [H₃O^+] is the concentration of hydronium ions (in M) and [OH^-] is the concentration of hydroxide ions (also in M).

(a) Finding the Concentration of Hydroxide (OH^-) Ions:
Given that the concentration of H₃O^+ ions is 1.1 × 10^(-9) M, we can use the Kₐ expression to determine the concentration of OH^- ions.

We know that Kₐ for water is 1.46 × 10^(-14) at 30°C. Since water is neutral, the concentration of both H₃O^+ and OH^- ions will be equal.

Let's denote the concentration of OH^- ions as x. Therefore, we can set up the equation:

1.46 × 10^(-14) = (1.1 × 10^(-9))(x)

Solving this equation will give us the concentration of OH^- ions in the solution.

(b) Determining the Acidity/Basicity/Neutrality of the Solution:
To determine if the solution is acidic, basic, or neutral, we need to compare the concentrations of H₃O^+ and OH^- ions.

If the concentration of H₃O^+ ions is greater than the concentration of OH^- ions, the solution is acidic. If the concentration of OH^- ions is greater than the concentration of H₃O^+ ions, the solution is basic. If the concentrations of both ions are equal, the solution is neutral.

By comparing the concentrations of H₃O^+ and OH^- ions obtained in part (a), we can determine the nature of the solution.

Please provide some time as I evaluate and calculate the values.