Determine Ka for hydrogen sulfate ion, HSO 4^- In a 0.10 -M solution the acid is 29% ionized.

Name: Problem 59, Chapter 14: Chemistry
Uploaded: 2020-04-20T17:24:17-08:00
Duration: 6 min 34 s
Channel: Jasmine Haskell
Description: Determine Ka for hydrogen sulfate ion, HSO 4^- In a 0.10 -M solution the acid is 29% ionized.

Determine Ka for hydrogen sulfate ion, HSO 4^- In a 0.10 -M...

Key Concepts

Acid Dissociation Constant (Ka)

The acid dissociation constant is a measure of the strength of an acid in solution. It quantifies the equilibrium between the undissociated acid and its dissociation products (hydrogen ions and the conjugate base) in water. A higher Ka indicates a stronger acid that ionizes more completely in solution, while a lower Ka denotes a weaker acid.

Percent Ionization

Percent ionization is the measure of the fraction of an acid that dissociates into ions in solution, expressed as a percentage of the initial concentration. It provides insight into the extent of acid dissociation under specific conditions and is used to relate the initial concentration of the acid to the equilibrium concentrations of the ions formed.

Equilibrium Concentration Calculations

Calculating equilibrium concentrations often involves setting up an ICE (Initial, Change, Equilibrium) table, a method that organizes the initial amounts, the changes occurring as equilibrium is established, and the final equilibrium concentrations. This systematic approach is essential for deriving expressions for the equilibrium constant, such as Ka, based on known starting concentrations and observed ionization percentages.

Transcript

00:01 Problem 59 from chapter 14 is asking us to determine the ca of the hydrogen sulfate ion in a 0 .1 molar solution where the acid is 29 % ionized.

00:15 So our first step in answering this question will be to set up an ice table.

00:21 This will just help us visualize the problem a little bit better.

00:26 And then we will use the percent ionization to help us fill in the blanks of our ice table.

00:31 Table and then with those values that we calculate we will then be able to determine the k a so i've gone ahead and drawn the equilibrium equation of this weak acid and then we can go ahead and start to fill out our ice table so as stated in the question our initial concentration of the solution is 0 .1 molar.

01:07 And we can neglect the water and move on to the hydrogen concentration.

01:17 And this is going to be around zero as water is going to be, we're going to have a negligible effect on the concentration of hydronium.

01:29 And then we have zero.

01:37 For the initial concentration of the sulfate ion.

01:41 Next, so our change.

01:43 Our change is going to be minus x.

01:47 And here we have plus x and plus x.

01:58 And then at our at equilibrium, we're just going to combine our initial and change terms.

02:04 We have 0 .1 molar minus x.

02:08 And then for the hydronium ion, we have x.

02:11 The sulfate ion, we have x.

02:14 So the question is, provides us with the ionization percentage of this weak acid.

02:20 So if you can go ahead and actually calculate this value of x with the percent ionization concentration, excuse me, just the percent ionization.

02:32 And that will give us the hydrogen ion concentration...

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