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