Linked Questions

2
votes
2answers
484 views

Are the best buffers those that are in a 1:1 ratio with its conjugate acid/base?

I wanted to comment this, but I don't have enough reputation, so I just made this a question. I know that buffers and their conjugate base/acid must exist in similar amounts for the buffer to be ...
-3
votes
1answer
799 views

Finding the pH value of HF [closed]

Find the pH value of HF. $pH = -\log[H+]$ for strong acids $pOH = -\log[OH-]$ for strong bases $pH = 1/2(pKa - \log C)$ for weak acid $pOH = 1/2(pKb - \log C)$ for weak base HF is weak acid so $...
-1
votes
2answers
264 views

Calculate pH of a mixture of a strong base and acid. Knowing only the pH, wt/v%, and volume of both solution. [closed]

Title explains all. I have been stuck on this for an hour and for some reason cannot understand it. I have tried to do an ICE table but get stuck halfway as I do not know whether I would use the w/v ...
1
vote
4answers
119 views

A simple equilibrium problem

Take the following simple equilibrium: $$\ce{CH3COOH + H2O <=> H3O+ + CH3COO-}$$ Ethanoic acid will act as a typical Brønsted-Lowry acid and donate a proton to water, forming a conjugate acid-...
0
votes
2answers
121 views

calculating pH - is my answer correct?

I'am working on this exercice, Is my answer correct? and can you please help me to solve the second part? exercice: 1/Calculate the ionization coefficient and pH (with two methods) of a 0.1M ...
-3
votes
2answers
136 views

What is the ionization constant, $K_a$, of the acid?

A 0.45 M solution of a weak acid, HX, has a pH of 4.5. What is the ionization constant, $K_a$, of the acid? Attempt at solution: [HX] is already given as 0.45 M. [H+] is given by $10^{-4.5}$. ...
-1
votes
1answer
56 views

Why does a weak base, which is also a salt, dissociate completely in water? [closed]

I'm answering a problem where $\ce{KOH}$ and $\ce{KOAc}$ dissociate nearly as much as each other in separate aqueous solutions at equal concentrations. The problem essentially assumed both completely ...
1
vote
0answers
61 views

Calculating the pH of a weak acid from the Kb of its conjugate base

I'd start off by saying it's been many years since I was in chemistry lessons and have forgotten much, but recently I have had to relearn a lot of basic chemistry. The following doesn't really impede ...
-2
votes
2answers
53 views

What's wrong in this?

While calculating pH of 10^-8M HCl, we take into account the H+ ions released by water. But water also releases OH-ions.So she shouldn't they neutralise the H+ ions?
1
vote
0answers
30 views

Is there a thermodynamic explanation for how a substance behaves based on its pKa and the solution’s pH?

If the pH of the solution is lower than the pKa of the compound, then the compound will be protonated, because pH is a measure of the concentration of protons, and low pH means a high proton ...
0
votes
0answers
14 views

Problem in terms of pC-pH plotting

I recently confronted a mission to plot a pC-pH graph('p' stands for the p-value notation, and 'C' stands for the concentration of a species), which meets the conditions below: Plot the pC-pH graph ...