To answer your question, let's look at pKa values of the acids! What is pKa? Just like pH was invented for the hydrogen ion concentration, pKa is the scale used to deal with the dissociation of acid. The more the dissociation, the stronger the acid. This means, lower the number, the more acidic the acid.
[math]HCl[/math] = -6.3 [math]HNO_3[/math] = -1.4
So, [math]HCl[/math] is more 'acidic' than [math]HNO_3[/math].
To answer your question, let's look at pKa values of the acids! What is pKa? Just like pH was invented for the hydrogen ion concentration, pKa is the scale used to deal with the dissociation of acid. The more the dissociation, the stronger the acid. This means, lower the number, the more acidic the acid.
[math]HCl[/math] = -6.3 [math]HNO_3[/math] = -1.4
So, [math]HCl[/math] is more 'acidic' than [math]HNO_3[/math].
What do you mean by powerful in respect of an acid ?
HNO3 is a strong acid which dissociates completely
H3PO4 is a weak acid that dissociates only partially
In solutions with the identical molarity , there will be a higher concentration of H+ ions in the HNO3 solution than there is in the H3PO4 solution. The HNO3 will have a lower pH - it is a stronger acid.
What do you mean by powerful in respect of an acid ?
HNO3 is a strong acid which dissociates completely
H3PO4 is a weak acid that dissociates only partially
In solutions with the identical molarity , there will be a higher concentration of H+ ions in the HNO3 solution than there is in the H3PO4 solution. The HNO3 will have a lower pH - it is a stronger acid.
In reasonably dilute aqueous solution they are equally strong. It's sort of like asking whether pink or white grapefruits are more grapefruity. In mixes of concentrated acids nitric is protonated to form NO2+ so sulfuric seems stronger. To really tell one should research Ka’s in an acidic solvent such as dry acetic acid or SO2.
In reasonably dilute aqueous solution they are equally strong. It's sort of like asking whether pink or white grapefruits are more grapefruity. In mixes of concentrated acids nitric is protonated to form NO2+ so sulfuric seems stronger. To really tell one should research Ka’s in an acidic solvent such as dry acetic acid or SO2.
Hot and concentrated sulphuric acid can also gradually dissolve cupric sulphide by the following redox reaction.
CuS + 4H2SO4 = CuSO4 + 4SO2 + 4H2O
But dilute H2SO4 is non-oxidising, and so it is unable to attack the insoluble CuS effectively.
In case of nitric acid (HNO3), even the dilute acid has strong oxidising properties and so it can more easily react with the insoluble sulphide at high temperatures.
Hot and concentrated sulphuric acid can also gradually dissolve cupric sulphide by the following redox reaction.
CuS + 4H2SO4 = CuSO4 + 4SO2 + 4H2O
But dilute H2SO4 is non-oxidising, and so it is unable to attack the insoluble CuS effectively.
In case of nitric acid (HNO3), even the dilute acid has strong oxidising properties and so it can more easily react with the insoluble sulphide at high temperatures.
Yes, sulphuric acid (H2SO4) is a stronger acid than nitric acid (HNO3) though both are typical strong acids.
(1) When conc.H2SO4 is mixed with conc.HNO3, the latter behaves as a proton acceptor or base!
H2SO4 + HNO3 → H2NO3(+) + HSO4(-)
The result of this direct encounter between the two clearly establishes that sulphuric acid is the boss when they are forced to co-exist.
(2) Again, hot sulphuric acid quite easily displaces nitric acid from the latter’s salts (nitrates).
NaNO3 + H2SO4 (hot, concentrated) → NaHSO4 + HNO3
But, being the weaker acid between the two, nitric acid cannot displace sulphuric acid from the latter’s salts (sulphates).
Yes, sulphuric acid (H2SO4) is a stronger acid than nitric acid (HNO3) though both are typical strong acids.
(1) When conc.H2SO4 is mixed with conc.HNO3, the latter behaves as a proton acceptor or base!
H2SO4 + HNO3 → H2NO3(+) + HSO4(-)
The result of this direct encounter between the two clearly establishes that sulphuric acid is the boss when they are forced to co-exist.
(2) Again, hot sulphuric acid quite easily displaces nitric acid from the latter’s salts (nitrates).
NaNO3 + H2SO4 (hot, concentrated) → NaHSO4 + HNO3
But, being the weaker acid between the two, nitric acid cannot displace sulphuric acid from the latter’s salts (sulphates).
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HCLO4>HCL>H2SO4>HNO3 decreasing order of acidic strength.
Hclo4 is more acidic all of the them because Oxygen is more electronegative and shows four different resonating structures.
HCLO4>HCL>H2SO4>HNO3 decreasing order of acidic strength.
Hclo4 is more acidic all of the them because Oxygen is more electronegative and shows four different resonating structures.
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To answer your question, let's look at pKa values of the acids! What is pKa?
Just like pH was invented for the hydrogen ion concentration, pKa is the scale used to deal with the dissociation of acid. The more the dissociation, the stronger the acid. This means, lower the number, the more acidic the acid.
[math]HCl[/math] = -6.3
[math]HNO_3[/math] = -1.4
So, [math]HCl[/math] is more 'acidic' than [math]HNO_3[/math].
To answer your question, let's look at pKa values of the acids! What is pKa?
Just like pH was invented for the hydrogen ion concentration, pKa is the scale used to deal with the dissociation of acid. The more the dissociation, the stronger the acid. This means, lower the number, the more acidic the acid.
[math]HCl[/math] = -6.3
[math]HNO_3[/math] = -1.4
So, [math]HCl[/math] is more 'acidic' than [math]HNO_3[/math].
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H2SO4 is a stronger acid than HNO3
please upvote if it helps.
H2SO4 is a stronger acid than HNO3
please upvote if it helps.
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What do you mean by powerful in respect of an acid ?
HNO3 is a strong acid which dissociates completely
H3PO4 is a weak acid that dissociates only partially
In solutions with the identical molarity , there will be a higher concentration of H+ ions in the HNO3 solution than there is in the H3PO4 solution. The HNO3 will have a lower pH - it is a stronger acid.
What do you mean by powerful in respect of an acid ?
HNO3 is a strong acid which dissociates completely
H3PO4 is a weak acid that dissociates only partially
In solutions with the identical molarity , there will be a higher concentration of H+ ions in the HNO3 solution than there is in the H3PO4 solution. The HNO3 will have a lower pH - it is a stronger acid.
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In reasonably dilute aqueous solution they are equally strong. It's sort of like asking whether pink or white grapefruits are more grapefruity. In mixes of concentrated acids nitric is protonated to form NO2+ so sulfuric seems stronger. To really tell one should research Ka’s in an acidic solvent such as dry acetic acid or SO2.
In reasonably dilute aqueous solution they are equally strong. It's sort of like asking whether pink or white grapefruits are more grapefruity. In mixes of concentrated acids nitric is protonated to form NO2+ so sulfuric seems stronger. To really tell one should research Ka’s in an acidic solvent such as dry acetic acid or SO2.
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Hot and concentrated sulphuric acid can also gradually dissolve cupric sulphide by the following redox reaction.
CuS + 4H2SO4 = CuSO4 + 4SO2 + 4H2O
But dilute H2SO4 is non-oxidising, and so it is unable to attack the insoluble CuS effectively.
In case of nitric acid (HNO3), even the dilute acid has strong oxidising properties and so it can more easily react with the insoluble sulphide at high temperatures.
Hot and concentrated sulphuric acid can also gradually dissolve cupric sulphide by the following redox reaction.
CuS + 4H2SO4 = CuSO4 + 4SO2 + 4H2O
But dilute H2SO4 is non-oxidising, and so it is unable to attack the insoluble CuS effectively.
In case of nitric acid (HNO3), even the dilute acid has strong oxidising properties and so it can more easily react with the insoluble sulphide at high temperatures.
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Let me ask you what are the similarities, sure they are both acids but they have a lot of differences.
Let me ask you what are the similarities, sure they are both acids but they have a lot of differences.
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Hard to say because it doesn’t exist.
Hard to say because it doesn’t exist.
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