Respuesta :
Answer:
See explanation below
Explanation:
The question is incomplete. However, I managed to find a similar question with these values of [OH⁻]. If these values are not the same that you have, don't worry, you all need to replace your given data in this procedure, and you should get the accurate results. The concentrations here will be:
[OH-]=10x10^-12M
[OH-]=7x10^-9M
[OH-]=7x10^-4M
[OH-]=8X10^-10M
[OH-]=1X10^-5M
[OH-]=4X10^-13M
[OH-]=1X10^-7M
[OH-]=2X10^-2
Now, to get the [H₃O⁺] we just use the following expression:
Kw = [OH⁻] [H₃O⁺] -----> [H₃O⁺] = Kw / [OH⁻]
Applying this expression, we'll get the hydronium concentrations and then, we could see which one is acidic, basic or neutral:
a) [OH-] = 1x10⁻¹² M
[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻¹² = 0.01 M or 1x10⁻² M. Acidic
b) [OH-]= 7x10⁻⁹ M
[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁹ = 1.43x10⁻⁶ M. Acidic
c) [OH-] = 7x10⁻⁴ M
[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁴ = 1.43x10⁻¹¹ M. Basic
d) [OH-] = 8x10⁻¹⁰M
[H₃O⁺] = 1x10⁻¹⁴ / 8x10⁻¹⁰ = 1.25x10⁻⁵ M. Acidic
e) [OH-] = 1x10⁻⁵M
[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁵ = 1x10⁻⁹ M. Basic.
f) [OH-] = 4x10⁻¹³ M
[H₃O⁺] = 1x10⁻¹⁴ / 4x10⁻¹³ = 2.5x10⁻² M. Acidic
g) [OH-] = 1x10⁻⁷ M
[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁷ = 1x10⁻⁷ M. Neutral
h) [OH-] = 2x10⁻² M
[H₃O⁺] = 1x10⁻¹⁴ / 2x10⁻² = 5x10⁻¹³ M. Basic.
The hydroxide ion concentrations that correspond to acidic, basic or neutral solutions are as follows;
[OH⁻] = 10 × 10⁻¹² M is acidic
[OH⁻] = 7 × 10⁻⁹ M is acidic
[OH⁻] = 7 × 10⁻⁴ M is basic
[OH⁻] = 8 × 10⁻¹⁰ M is acidic
[OH⁻] = 1 × 10⁻⁵ M is basic
[OH⁻] = 4 × 10⁻¹³ M is acidic
[OH⁻] = 1 × 10⁻⁷ M is neutral
[OH⁻] = 2 × 10⁻² M is basic
We are given formula to get the ion Product constant of water as;
Kw = [H₃O⁺][OH⁻] = 1 × 10⁻¹⁴ M
The hydroxide concentrations are missing and they are;
[OH⁻] = 10 × 10⁻¹² M
[OH⁻] = 7 × 10⁻⁹ M
[OH⁻] = 7 × 10⁻⁴ M
[OH⁻] = 8 × 10⁻¹⁰ M
[OH⁻] = 1 × 10⁻⁵ M
[OH⁻] = 4 × 10⁻¹³ M
[OH⁻] = 1 × 10⁻⁷ M
[OH⁻] = 2 × 10⁻² M
We are told that;
[OH⁻] is acidic when; [H₃O⁺] > 1 × 10⁻⁷ M
[OH⁻] is neutral when; [H₃O⁺] = 1 × 10⁻⁷ M
[OH⁻] is basic when; [H₃O⁺] < 1 × 10⁻⁷ M
[H₃O⁺] will be found using the formula;
[H₃O⁺] = (1 × 10⁻¹⁴)/[OH⁻]
1) For [OH⁻] = 10 × 10⁻¹² M;
[H₃O⁺] = (1 × 10⁻¹⁴)/(10 × 10⁻¹²)
[H₃O⁺] = 1 × 10⁻² M
It is > 1 × 10⁻⁷ M and is acidic
2) For [OH⁻] = 7 × 10⁻⁹ M;
[H₃O⁺] = (1 × 10⁻¹⁴)/(7 × 10⁻⁹)
[H₃O⁺] = 1 × 10⁻⁵ M
It is > 1 × 10⁻⁷ M and is acidic
3) [OH⁻] = 7 × 10⁻⁴ M
[H₃O⁺] = (1 × 10⁻¹⁴)/(7 × 10⁻⁴)
[H₃O⁺] = 1.43 × 10⁻¹¹ M
It is < 1 × 10⁻⁷ M and is basic
4) [OH⁻] = 8 × 10⁻¹⁰ M;
[H₃O⁺] = (1 × 10⁻¹⁴)/(8 × 10⁻¹⁰)
[H₃O⁺] = 1.25 × 10⁻⁵ M
It is > 1 × 10⁻⁷ M and is acidic
5) For [OH⁻] = 1 × 10⁻⁵ M;
[H₃O⁺] = (1 × 10⁻¹⁴)/(1 × 10⁻⁵)
[H₃O⁺] = 1 × 10⁻⁹ M
It is < 1 × 10⁻⁷ M and is basic
6) For [OH⁻] = 4 × 10⁻¹³ M;
[H₃O⁺] = (1 × 10⁻¹⁴)/(4 × 10⁻¹³)
[H₃O⁺] = 2.5 × 10⁻² M
It is > 1 × 10⁻⁷ M and is acidic
7) For [OH⁻] = 1 × 10⁻⁷ M
[H₃O⁺] = (1 × 10⁻¹⁴)/(1 × 10⁻⁷)
[H₃O⁺] = 1 × 10⁻⁷ M
It is = 1 × 10⁻⁷ M and is neutral
8) For [OH⁻] = 2 × 10⁻² M
[H₃O⁺] = (1 × 10⁻¹⁴)/(2 × 10⁻²)
[H₃O⁺] = 5 × 10⁻¹³ M
It is < 1 × 10⁻⁷ M and is basic
Read more about hydroxide concentration at; https://brainly.com/question/25214393
