BuyFindarrow_forward

Chemistry: Atoms First

3rd Edition
Julia Burdge + 1 other
ISBN: 9781259638138

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry: Atoms First

3rd Edition
Julia Burdge + 1 other
ISBN: 9781259638138
Interpretation Introduction

Interpretation:

The ionization constant for the given acid solution with 0.010 M concentration whose pH is 6.20 at 25C has to be calculated

Concept Information:

Acid ionization constant Ka :

Acids ionize in water. Strong acids ionize completely whereas weak acids ionize to some limited extent.

The degree to which a weak acid ionizes depends on the concentration of the acid and the equilibrium constant for the ionization.

The ionization of a weak acid HA can be given as follows,

HA(aq)      H+(aq)+A-(aq)

The equilibrium expression for the above reaction is given below.

Ka=[H+][A-][HA]

Where,

Ka is acid ionization constant,

[H+]   is concentration of hydrogen ion

[A-]   is concentration of acid anion

[HA] is concentration of the acid

pH definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H+]

To Calculate: The ionization constant for the given acid solution with 0.010 M concentration whose pH is 6.20 at 25C

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Answers to Your Study Problems

Solve them all with bartleby. Boost your grades with guidance from subject experts covering thousands of textbooks. All for just $9.99/month

Get As ASAP