Week 2 Sapling Hw #2

[RaniyaFeroz_1E]

The Ka of a monoprotic weak acid is 0.00214. What is the percent ionization of a 0.121 M solution of this acid?
I'm confused about how to calculate the percent ionization.

[ColmConnolly3D]

The percent ionization will be the amount of charged particles at equilibrium (for a monoprotic acid, this is just the H30+ concentration) divided by the initial concentration (in this case 0.00214M) of the acid. This will tell you what percentage of the acid has dissociated to form charged species.

Hope this helps!
Colm

[Varsha Ravi 3E]

Find the equilibrium value of the conjugate base at equilibrium (which would be the same as the hydronium concentration) and divide it by the initial amount of the acid that's given in the problem. Multiply that against 100 for the percentage. Hope this helps!

[rhettfarmer-3H]

Percent Ionization =What you have made conjugate acid or base /initial base or acid *100. Therefore first you need to find all the ingredients for it. So first set up the equilibrium table and find the values. then plug them in. Hence, I look at it as a post percentage of how much was converted.

[Xinying Wang_3C]

Basically, the percentage ionized is the [dissociated]/[original reactant]. So you would use the ICE Table to solve for the [ H+] as usual. and just use that value to calculate [H+]/0.121 M. Hope this helps.

[Laura 3l]

Basically, the percentage ionized is the [dissociated]/[original reactant]. So you would use the ICE Table to solve for the [ H+] as usual. and just use that value to calculate [H+]/0.121 M. Hope this helps.

Yes you would do this and then multiply by 100 to get the percent ionization.

[RaniyaFeroz_1E]

Thank you so much, everyone!!

[Keshav Patel 14B 2B]

Do your ice table and find the concentration of Hydroniums in the solution, after that it’s easy just multiply by 1/100.

[Charlotte Chen 3B]

Since Ka=[H+]{A-]/[HA], you can plug in the values given so 0.00214=x^2/0.121-x , then you can solve for x using the quadratic equation and once you've solved for x, you can then divide it by the original concentration 0.121M and multiply it by 100 to get the percent ionization