All Questions
41
questions
-3
votes
1
answer
106
views
Can acids contain OH-? [closed]
Given that a solution contains $\ce{OH-}$ ions can we sufficiently determine the substance is a base? From my understanding, an acid may still contain $\ce{OH-}$ ions. However, the concentration of $\...
-2
votes
2
answers
483
views
Can ions be acids or bases?
Consider a sulfate ion, its considered a weak base. Yet I thought bases and acids were compounds meaning they were always electrically neutral? Why is a sulfate ion then considered a base? And how ...
- 61
-1
votes
1
answer
1k
views
Why does acetate ion react with water? [closed]
When NaCl is added to water, it dissociates into $\rm{Na^+}$ and $\rm{Cl^-}$. The newly formed $\rm{Na^+}$ and $\rm{Cl^-}$ do not react with water.
When $\rm{CH_3COONa}$ (sodium acetate) is added to ...
- 171
0
votes
2
answers
1k
views
Why doesn't base/acid reacting with water create a salt?
An acid/base nwutralization will create a salt + water. If one uses water itself as the acid or base, and have an acid/base neutralization, how come that doesn't create a salt?
For example:$$ \ce{HCN(...
- 205
1
vote
1
answer
99
views
Basic behavior of ammonia in aqueous medium [closed]
Thanks to the reversible reaction
$$\ce{NH3 + H2O <=> NH4+ + OH-},\tag{R1}$$
we know that ammonia acts as a weak base. However, I was wondering why it ends up forming ammonium $\ce{NH4+}$ and ...
- 121
1
vote
2
answers
1k
views
How to make acetic acid more volatile so that it can be removed by vigorous aeration of an acetic acid-water mixture? [closed]
I want to remove acetic acid from a mixture of acetic acid and water by aeration. The concentration of acetic acid is 200 ppm (mg/L). The pH of the water is more than 5. I want to reduce the acetic ...
1
vote
3
answers
314
views
How to decrease the percent of ammonia that is converted to the ammonium ion in water? [closed]
Ammonia is a weak base that reacts with water according to this equation:
NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH −(aq)
Will Fe(NO3)3 decrease the ...
- 129
-2
votes
2
answers
689
views
What is the pH of HCl solution at $10^{-8}$M? [duplicate]
After using the negative logarithmic value of $\ce{H^+}$ ion concentration, I get a value of pH that results in base. Can you please help me?
Thank you in advance
- 7
1
vote
1
answer
732
views
Are aspartic acid and glutamic acid at physiological pH present in zwitterionic form?
I am wondering whether aspartic acid and glutamic acid at physiological pH are present in zwitterionic form? In my textbook it says that all aminoacids at $\textrm{p}H$ of 7.4 or 7 are in zwitterion ...
- 21
10
votes
1
answer
10k
views
How does the HCl-KCl Buffer work?
I have just been studying the $\ce{HCl}$-$\ce{KCl}$ 'buffer', but there are still quite a few things I am uncertain about. I would appreciate any help in clearing up some questions I have.
What I ...
- 445
22
votes
3
answers
3k
views
How was it concluded that the H3O+ rather than H+ is the "acid" ion?
I suspect that initially, scientists believed that the acid ion was $\ce{H^+}$ since $\ce{H2}$ is released through electrolysis, right? But what experiment was done to change the standpoint to assume ...
- 369
2
votes
1
answer
1k
views
How does one classify aqueous solutions of ions as acidic, basic and neutral?
The following is a homework question:
Classify the aqueous solutions of the following ions as acidic, basic or neutral:
$\ce{C6H5NH3+, Cl- , Fe^3+ , Mg^2+ , HSO4- , NO3- , NH4+ , Al^3+...
- 1,161
-2
votes
2
answers
87
views
What do we call ions without basic and acidic properties
According to Brønsted theory,
Acids are substances (molecules and ions) donating $\ce{H+}$
Bases are substances (molecules and ions) receiving $\ce{H+}$
I've been trying to find a complete Brønsted-...
- 383
1
vote
1
answer
1k
views
Why is the inside of a cell both more acidic and more negative than its environment?
In a very simplistic way of thinking, an acidic solution has more positively charged $\ce{H+}$ ions present, whereas a basic solution has more negatively charged $\ce{OH-}$ ions present.
Can that be ...
- 1,118
3
votes
0
answers
546
views
Enthalpy change of chromate-dichromate reaction
I am a uni study doing chemistry. I have taken a little bit in highschool before, but not in a while.
In a (nonassessed) practical, we have to predict how heating a chromate/dichromate solution:
$$\...
- 445
2
votes
1
answer
3k
views
Is aluminium amphoteric?
In my book it says that aluminium can react with water as a base when it's in the form $\ce{[Al(OH)2(OH2)4]^+}$.
And this way as an acid: $\ce{[Al(OH2)_6]^3+}$.
So ... does it depend on with which ...
- 43
0
votes
2
answers
6k
views
Calculating the pH of a mixture of Na2HPO4 and Na3PO4?
I know there are more questions about this on the forum, but I was just wondering: when we mix both solutions, would we have to consider the equilibria corresponding to $\mathrm{p}K_\mathrm{a2}$ and $\...
- 257
-2
votes
3
answers
123
views
Can other molecules than H+ cause a kind of acid reaction?
In our body there are plenty of other positive ions like $\ce{Na+, K+}$ and $\ce{Ca^2+}$. Can they have a similar acid reaction as $\ce{H+}$ ions can do? If not why is just $\ce{H+}$ considered as ...
- 515
1
vote
1
answer
1k
views
Effect of pH on volatility (odor) of organic acid
Based on two assumptions:
Ionic solutes can generally be considered nonvolatile
As the pH of a solution of organic acid is increased, an increasing percentage of it is deprotonated, or ionized (...
- 11
2
votes
2
answers
11k
views
Is H+ (in an aqueous solution) = H3O+? [duplicate]
I was learning about autoionization in science and my science teacher wrote $\ce{H3O+}$ as $\ce{H+}$ — now, my intuition would lead me to assume that:
$$\ce{H3O+} = \ce{H+}$$
But, $\ce{H+}$ is just ...
- 409
4
votes
1
answer
2k
views
Is the concentration of negative ions always equal to that of positive ions?
Is there any way in which a solution can have more negative charge than positive charge, or vice versa? For example, in the context of acid-base chemistry, is there any scenario in which $[\ce{H+}]\ne[...
- 1,292
3
votes
1
answer
4k
views
Reversibility of an acid's reaction with water depending on its strength
This is how my chemistry professor compared reaction of a weak and a strong acid with water:
$$\ce{HCl + H2O -> H3O+ + Cl- + Heat}$$
In this case $\ce{H2O}$ breaks the bond between $\ce{H}$ ...
- 183
13
votes
1
answer
11k
views
Can H4O 2+ form?
Like $\ce{NH4+}$ ,Is there any possibility of formation of $\ce{H4O^{2+}}$ (of tetrahedral structure)?
My theory is: it can be formed by osmosis setup where heavy acids like $\ce{H3PO4}$ or $\ce{...
- 1,232
11
votes
2
answers
545
views
Why quaternary nitrogen but not tertiary oxygen?
Why do quaternary ammonium ions with a partially positive nitrogen form fairly readily and are often stable but tertiary oxygens, apparently called oxonium ions, are more rare/less stable? The trend ...
- 1,690
0
votes
2
answers
178
views
hydroxide ion in water -- How does the dynamic change?
It's well known that $\ce{H+}$ ions in water always form $\ce{H3O+}$ ions. Likewise, $\ce{OH-}$ should exist always as $\ce{H3O2-}$ ion. If I am correct at this point, how would the dynamics be ...
- 429
0
votes
1
answer
548
views
Is it possible for monobasic and dibasic potassium phosphate to complete break down into phosphates? [closed]
Here is the picture of monobasic potassium phosphate:
And here is the picture of dibasic potassium phosphate:
Is it possible for the phosphorous-containing anions to further break down into ...
- 19
1
vote
1
answer
150
views
Understanding a passage related to salt buffer
Passage from my textbook:
Are reactions possible among any of the solution components; is so, what is their stoichiometry?
Suppose that you are asked to calculate $[\ce{OH-}]$ in a solution that is ...
- 697
1
vote
2
answers
6k
views
What is the reason for strong acids/bases dissociating in water?
I have read that the actual definition of a strong acid is one which will fully dissociate in water, so please do not turn the problem on its head when answering. It is also my understanding that ...
- 429
13
votes
2
answers
8k
views
Why does the ionic product of water remain constant after addition of non-neutral solute?
In my textbook, it is given that the ionic product of water $K_\mathrm{w}$ remains constant even when a non-neutral solute such as an acid is added to it.
$$K_\mathrm{w} = \ce{[H3O+][OH-]}$$
When a ...
- 295
3
votes
2
answers
1k
views
Acidity of oxonium ion
How was the pKa value (-1.7) for the oxonium ion determined? Why does it correspond to the minimum pH value accessible in water? What reaction does it represent?
- 14.4k
3
votes
2
answers
42k
views
How is the dissolution of acetic acid that makes its aqueous solution a poor electrolyte?
I'm having a difficulty understanding the following quote from Wikipedia - Dissociation:
Acetic acid is extremely soluble in water, but most of the compound dissolves into molecules, rendering it a ...
- 203
0
votes
2
answers
390
views
Hydrogen peroxide from water
Is it possible that $\ce{2 OH-}$ from water could react to form $\ce{H2O2}$?
I mean most autoionization forms $\ce{H3O+}$ and $\ce{OH-}$.
However I think it is possible that $\ce{H-}$ and $\ce{OH+}$ ...
- 2,121
18
votes
2
answers
11k
views
How should the hydrated proton be represented in chemical equations?
I learned the equation
$$\ce{H2O + H+ -> H3O+}$$
And I know $\ce{H+}$ and $\ce{H3O+}$ really mean the same thing. But I am confused as to when I should use $\ce{H+}$ and when I should use $\ce{...
- 4,703
3
votes
1
answer
302
views
Why do strong acids dissociate (almost) fully on a molecular level?
In the Brønsted-Lowry theory, strong acids $\ce{HA}$ dissociate using water and react into hydronium ions and the conjugate bases $\ce{A-}$. However I never understood in the strong acids case what ...
- 163
0
votes
1
answer
970
views
What happens when oxidizing Ni(OH)2 with a strong base?
In an aqueous solution, Nickel oxyhydroxide is oxidised with a 1:1 ratio of aqueous Sodium hydroxide. My goal is to produce Nickel oxyhydroxide ($\ce{NiOOH}$).
Strong Base: $\ce{NaOH + H2O \...
- 111
3
votes
1
answer
427
views
In a redox reaction, why does more than one oxidation state of an element form?
Consider the reaction 100ml 10M $\ce{NaOH_{(aq)}} +$ 100ml 10M $\ce{NaHSO3_{(aq)} +}$ 100mL 0.01M $\ce{KMnO4_{(aq)}}$
In the picture posted here, the left columns give information on the Molarity of ...
- 720
0
votes
1
answer
196
views
How to determine the reaction of a strong electrolyte? [closed]
I'm told the $\ce{KMnO4}$ is a strong electrolyte.
How can I figure out how the reaction looks like?
- 101
14
votes
2
answers
169k
views
What are the products of the dissociation of sodium bicarbonate in water? What is the relative pH of the solution?
I had a recent question on a test that asked what the products would be if sodium hydrogen carbonate were dissolved in water. I had a few candidate answers
$\displaystyle\ce{NaHCO3 -> Na+ + HCO3-}$...
- 371
5
votes
2
answers
3k
views
Calculating approximate pH of polyprotic acids
When I took up ionic equilibria and titrations after a long break, I found it hard to solve the questions regarding pH calculations of polyprotic acds. Consider these two questions as examples:-
...
- 6,795
5
votes
2
answers
4k
views
Does the hydrolysis speed increase when more H+ ions are in the solution?
In hydrolysis of polysaccharides, does the hydrolysis speed increase when more $\ce{H+}$ ions are present in the solution?
So if I were to use $\ce{H2SO4}$ instead of $\ce{HCl}$ (same volumes) then $\...
user2117
-1
votes
2
answers
7k
views
Why is there a charge on COOH⁻¹?
The dissociation of formic acid ($\ce{HCOOH}$) is:
$$
\ce{HCOOH -> H+ + COOH-}
$$
Why is there a charge on $\ce{COOH^{-1}}$
though? Is it achieved through:
$$1\times(\ce{C^{4+}}) + 2\times(\ce{O^...
- 9