Asked by Jennie

I have no idea where to begin with this?? This class is moving so fast! Dr. Bob222 I made a 100 on my prelab!! and the online test was so fast I was going through my notes and I was scrambling to figure it out and look up stuff on the periodic table and all!! But I made an 80! I'm happy with that!
Now... What the heck is this?? PH and acids?


Calculate the concentration of OH− and the pH value of an aqueous solution in which [H3O+] is 0.014M at 25°C. Is this solution acidic, basic or neutral?

Write the acid-dissociation reaction of nitrous acid (HNO2) and its acidity constant expression.

Calculate the concentration of the hydronium ion ([H3O+]) for a solution with the pH = 4.51.

Consider the HF solution with the concentration of 5% (w/v). Calculate its concentration in the molarity. Use four significant figures in your answer.

At equilibrium, it was found that [CH3COOH] = 0.8537 M, [CH3COO−]= 0.0040M, and [H3O+] =0.0040 M. Calculate the acidity constant (Ka) and the pKa value of CH3COOH.

Answered by DrBob222
You would do well to post separate posts. Sometimes we don't have time to answer 4-5 questions at a time.

Calculate the concentration of OH− and the pH value of an aqueous solution in which [H3O+] is 0.014M at 25°C. Is this solution acidic, basic or neutral?

<b>pH = -log(H3O^+)
pH = -log(0.014M) etc. It's a matter of finding the right buttons on your computer.</b>
Answered by DrBob222
(H3O^+)(OH^-) = Kw = 1E-14. You know Kw and H3O^+, solve for OH^-
Answered by DrBob222
If H3O^+ > 10-7M, acid
If H3O^+ = 10^-7M, neutral
If H3O^+ < 10^-7M, basic
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