Is HClO3 a stronger acid than HClO2?
For these two reasons, ClO3 (-) is a weaker base than ClO2 (-), making HClO3 the stronger acid over HClO2. Why is HClO₄ more acidic than HClO?
Why is HClO3 more electronegative than HBrO3?
Comparing HClo3 and HBrO3 there are 3 oxygen atoms bound to the central halogen in each case causing a shift of electrons from the halogens to the oxygen. But halogens are electronegative and don’t like their electrons getting pulled from them. So they try to gain back any amount electron from nearby atoms. Their next best option?
Which is a stronger oxidizing agent HOCl or HClO4?
Explanation: hocl is stronger oxidizing agent than hclo4 because it has the lowest oxidation state and hence it is a stronger oxidizing agent.
Which is stronger HCl or HF?
A strong acid is an acid that completely disassociates in water, so HCl is strong and HF is weak. Note that fluorine’s electronegativity isn’t a major factor here. Hope that helps. Which is stronger HI or HClO4?
Which is stronger HClO or HClO3?
The acid is much stronger if the number of oxygen atoms is more. In HClO3 and HClO2, HClO3 has more oxygen therefore it is more acidic.
Which one is the strongest acid HClO HClO2 HClO3 HClO4?
And electronegativity of chlorine in turn is directly proportional to the oxidation state of chlorine. Thus, the order of acidic strength is HClO < HClO2 < HClO3 < HClO4 As the number of oxygen atoms attached to chlorine increases, acid strength increase.
Why is HClO stronger than HClO4?
If a proton is less strongly attached to any one of the oxygens, then you get a stronger acid. As the number of oxygens increases as you go from HClO to HClO4, the oxidation number of Cl increases.
Why is HClO3 more acidic than HOCl?
- In Chlorous acid, Cl=O. bond will withdraw the electron density from the negatively charged oxygen atom in the conjugate base, so the conjugate base will be more stable and hence the overall acidic strength of Chlorous acid will be more compared to Hypochlorous acid.
Is HClO a strong acid?
Since HClO is not one of these seven, and there is no -OH group present as there is in bases, HClO is a weak acid.
Which one of the following acids is the weakest HClO HBr HClO3 HCl?
HClO acid is weakest.HClO ⇌ H+ + ClO- Which is the weakest out of HF, HCl, HBr and HI?
Which acid is stronger HClO4 or HClO?
Within an oxyacid series such as HClO, HClO3, HClO2 and HClO4, as the number of oxygens bonded to the central atom increases, the oxidation number of the central atom increases causing a weakening of the O-H bond strength and an increase in the acidity. Most acidic: HClO4 > HClO3 > HClO2 > HClO.
Why is HClO a weak acid?
HClO is an acid as is has the proton that it can donate but it is a weak acid because it is not one the acid amoung the list of the strong acids.
Which is stronger oxidizing agent HOCl or HClO4?
Solution : Out of HOCl, `HClO_(2) HClO_(3) and HClO_(4),HOCl` is the strongest oxidising agent.
Which is the strongest acid in the following a HClO B HClO C Hocl D HClO3?
The HClO4 has the most oxygen atoms so it would have to be the strongest acid.
Which of the following is the correct order of acidic strength Hocl?
The decreasing order of acidic strength is HClO4>HClO3>HClO2>HClO.
Why is the O-H bond stronger on HClO?
Hence, the O-H bond on HClO will be stronger and, therefore, that H will be more reluctant to be released as a proton (H⁺).
How many oxygen atoms are in HClo3?
Comparing HClo3 and HBrO3 there are 3 oxygen atoms bound to the central halogen in each case causing a shift of electrons from the halogens to the oxygen.
What happens when the central chlorine atom is attached to the electron withdrawing oxygen atom/s?
The more the electron withdrawing oxygen atoms, more will be the electron withdrawing effect. Once the electron on the bonded hydrogen atom is pulled towards the oxygen atom, the hydrogen atom can be removed as hydrogen ion. If more oxygen atoms are present, then the combined withdrawal effect makes it easier for the formation of hydrogen ion. Hence electron withdrawal increases strength of the acid.
Why do you attach more oxygen atoms to the central atom in an oxyacid?
Attaching more oxygen atoms to the central atom in an oxyacid helps to distribute the negative charge of the conjugate base over a greater number of atoms. This makes the proton less strongly attracted to any one of the oxygen atoms in the conjugate base. Hence, you get a stronger acid.
What happens when an atom is attached to an OH bond?
Here, Electronegativity of atom X (F, Cl or Br or I) attached to O decreases down a group, polarity of OH bond decreases, acid strength decreases. It means more the electronegativity of the halogen atom, more the tendency to pull electron and weaker the O-H bond and hence proton (H+) can easily remove.
Which is more electronegative, bromine or chlorine?
Chlorine being more electronegative than Bromine it pulls the electron of hydrogen more strongly and hence has a higher tendency to release a H+ unit. Hence we can s
Do halogens have electrons?
But halogens are electronegative and don’t like their electrons getting pulled from them.
Which is stronger, HClO2 or HClO4?
The general rule is that the acid is stronger if it has more O atoms in a series such as this. HClO4, perchloric acid, is a very strong acid as is HClO3. HClO2 is a weak acid and HClO is even weaker.
How many oxygen atoms are in HClo3?
Comparing HClo3 and HBrO3 there are 3 oxygen atoms bound to the central halogen in each case causing a shift of electrons from the halogens to the oxygen.
How many protons does H2SO4 have?
H2SO4 has 2 protons to lose. After the first one is separated, we have the HSO4- ion. It’s hard, energetically, to pull a positive proton off of a negative ion, so HSO4- is unlikely to progress to SO4 2-. So even though sulfuric acid has 2 protons to lose, really only about 1 is removed. HSO4- is actually a weak conjugate base, so it raises the pKa of H2SO4.
What is the factor that stabilizes ClO3?
Another factor stabilizing ClO3 (-) over ClO2 (-) is the charge on the central atom, chlorine. If we approximate this charge by the oxidation number (+5 for ClO3 (-) and +3 for ClO2 (-)), we see that the Cl in ClO3 (-) has more attractive force to a negatively charged oxygen than the Cl in ClO2 (-). If you use formal charges (+2 for ClO3 (-) and +1 for ClO2 (-)), you come to the same conclusion.
Which bond draws the electrons from the oxygens bonded to the chlorine but not to the hydrogen?
In both, the oxygens bonded to the chlorine but not to the hydrogen draw the electrons in the O—H bond to
Which is more electronegative, bromine or chlorine?
Chlorine being more electronegative than Bromine it pulls the electron of hydrogen more strongly and hence has a higher tendency to release a H+ unit. Hence we can s
Which atom is bonded to the hydrogen atom?
In both of them, the hydrogen is bonded to one of the oxygens, which is in turn bonded to the central atom, chlorine, to which all of the other oxygens are attached.
Which acid is the strongest?
As another answer pointed out, HClO4 is the strongest acid in the series because the negative charge on the conjugate base (ClO 4 −) is resonance-stabilized over all four oxygens.
Which is the strongest oxidant?
Based on these standard reduction potentials, in acidic medium, HClO2 is the strongest oxidant, followed by HClO (i.e., “bleach”).
What happens when the central chlorine atom is attached to the electron withdrawing oxygen atom/s?
The more the electron withdrawing oxygen atoms, more will be the electron withdrawing effect. Once the electron on the bonded hydrogen atom is pulled towards the oxygen atom, the hydrogen atom can be removed as hydrogen ion. If more oxygen atoms are present, then the combined withdrawal effect makes it easier for the formation of hydrogen ion. Hence electron withdrawal increases strength of the acid.
Is ClO3 a resonance hybrid?
There is another factor stabilizing ClO3 (-) over ClO2 (-). These are both resonance hybrids (look here if you don’t understand this term). Resonance makes the three oxygen atoms in ClO3 (-) equal, so that each oxygen atom has -1/3 charge. Similarly, resonance gives each oxygen atom in ClO2 (-) a -1/2 charge. Since the negative charge is more spread out in ClO3 (-) than in ClO2 (-), this also makes ClO3 (-) a weaker conjugate base, and thus HClO3 the stronger acid,
Which is more electronegative, bromine or chlorine?
Chlorine being more electronegative than Bromine it pulls the electron of hydrogen more strongly and hence has a higher tendency to release a H+ unit. Hence we can s
Is hydrogen chloride the same as hydronium?
It depends on what your question really is. If you mean aqueous solutions, they are the same, as the acid is essentially hydronium, which is probably usually something like H5O2+. If you mean pure, hydrogen chloride in the liquid state is more difficult to consider because out is difficult to measure the acidity. Very strong acids need some other species to get acidity into some order, and the strength of very strong acids has traditionally been measured by their ability to stabilise carbenium ions, i.e. will it protonate the associated double bonded material? The problem with hydrogen chlorid
Is sulfuric acid stronger than concentrated?
When it comes to sulfuric acid, dilute sulfuric acid is stronger than a concentrated one. If you go to any industry, you will find that they are storing concentrated acids in stainless steel tanks and the concentration of the acid is not allowed to fall below 95%. This is because when concentrated acid comes in contact with an iron surface, it reacts to produce sulphates of iron which render the rest of the iron impassive thus protecting it. However, were you go on diluting it, a rather porous deposition develops on the steel walls. This promotes attack by the acid. Also, the activity of sulfuric acid increases with dilution. In case of weaker acids, the dissociation increases with dilution, which means that as more and more water is added, more hydrogen ions will be generated. By and large, dilute sulfuric acid is more harmful than concentrated sulfuric acid.
Which is stronger, HClO2 or HClO4?
The general rule is that the acid is stronger if it has more O atoms in a series such as this. HClO4, perchloric acid, is a very strong acid as is HClO3. HClO2 is a weak acid and HClO is even weaker. Thus we see more oxygen atoms means more possible strutures & which means stronger the acid. Likewise, is HClO a strong acid?
Which is the most acidic molecule?
Most acidic: HClO4 > HClO3 > HClO2 > HClO. For a series of oxyacids with the same number of oxygens but with different central atoms such as HOBr, HOCl, HOI, as the electronegativity of the central atom increases, the O-H bond strength weakens and the acidity increases. Most acidic: HOCl > HOBr > HOI :Least acidic.
Is phosphorus acid a liquid?
Phosphoric acid, when pure, is a solid at room temperature and normal pressure. However, an aqueous solution of 85 % H3PO4 is a viscous liquid. HCl is the strongest acid (indicated by the lowest pKa) followed by H2SO4 and HNO3. H3PO4 is the weakest of the acids.
Is HBrO4 a strong acid?
So, no, since HBrO3 and HBrO4 don't completely dissociate, they are not considered strong acids .
Is potassium chlorate an acid or base?
Potassium chlorate is an ionic compound that is dissociated into K+ and ClO3- ions. So potassium chlorate is neither an acid nor a base. It is a salt formed from the reaction of the acid HClO3 and the base KOH.
Is KOH an acid or a base?
Potassium hydroxide, KOH, is a strong base as it splits into its atoms and hydroxide ions in water solution. Is NaOH an acid or a base? Potassium hydroxide, NaOH, is a strong base as it splits into its atoms and hydroxide ions in water solution.
Is HClO stronger than HIO?
Beside this, is HClO or HBrO a stronger acid? HBrO is a little stronger than HIO because Br is stronger in electronegativity than I. HClO is a little stronger than HBrO because Cl is stronger in electronegativity than Br. HClO 2 is a little stronger than HClO because it contains two electronegative oxygens.
