[joe900]

Could you please tell me, if THERE REACTIONS ARE CORRECT?

1) preparation of sodium chlorate :
NaCl + 3H2O = NaClO3 + 3H2

2) preparation of potassium chlorate from sodium chlorate:
NaClo3 + KCl = NaCl + KClO3

3) how to prepare

A. barium chlorate:
BaO +Cl2O5 = BaCl2O6

B.nickel chlorate:
have no idea

4) methods of preparation of any bromate, iodate and compare it with chlorate:

e.g.
6 NaOH (hot) + 3Br2 = NaBrO3 + 5 NaBr + 3H2O

NaI + 3H2O = electrolysis 3H2 (cathode) + NaIO3 (anode)

NaCl + 3H2O = NaClO3 + 3H2

how to compare methods of preparation this compounds?
and what are the differemces in reactivity of products: bromate, iodate and chlorate?

5) how to prepare KIO3 from Cl2, KI and K2CO3:

2KI + Cl2 = 2KCl + I2
3K2CO3 + 3 H2O + 3I2 = KIO3 + 5 KI +3H2CO3


THANKS IN ADVANCE!!

[Arkcon]

Could you please tell me, if THERE REACTIONS ARE CORRECT?

1) preparation of sodium chlorate :
NaCl + 3H2O = NaClO3 + 3H2

OK, this one is simply ridiculous.  You've simply balanced the atoms, but this reaction simply won't go forward.  Table salt dissolves in water, it doesn't become a highly energetic, oxidizing compound.

[joe900]

I have found it in literature:

"Industrially, sodium chlorate is produced by the electrolysis of a hot sodium chloride solution:
NaCl + 3 H2O → NaClO3 + 3 H2
This reaction progresses in heat (at least 70 degrees Celsius), and controlled pH."

[Arkcon]

Ah.  But you did leave out the electricity driving the reaction that you wanted, didn't you?

[unsu]

1) preparation of sodium chlorate :
NaCl + 3H2O = NaClO3 + 3H2

Here you forgot to specify the conditions: electrolysis without diaphragm

2) preparation of potassium chlorate from sodium chlorate:
NaClO3 + KCl = NaCl + KClO3

Yes, this is possible because KClO3 is much less soluble in water than NaClO3

3) how to prepare
A. barium chlorate:
B.nickel chlorate:

It can be prepared from barium chloride (common reagent) and NaClO3 (produced industrially in large scale):
BaCl2 + 2NaClO3 = 2NaCl + Ba(ClO3)2
Barium chlorate can be crystallized from solution.
For nickel(II) chlorate I would suggest similar reaction.

4) methods of preparation of any bromate, iodate and compare it with chlorate:

KClO3 can be prepared by 1) reaction between NaClO3 and KCl; 2) by passing Cl2 gas through hot KOH solution; 3) by electrolysis of aqueous KCl without diaphragm

KBrO3 can also be prepared by 1) reaction Br2 + KOH (or K2CO3) = KBrO3 + KBr + H2O
2) electrolysis aqueous KBr without diaphragm; 3) by reaction of Br2 with excess Cl2 in KOH:
Br2 + 5Cl2 + 12KOH = 2KBrO3 + 10KCl + 6H2O (80 °C)

KIO3 can be prepared from KI:
electrolysis of aqueous KI without diaphragm: KI + 3H2O = KIO3 + 3H2
or by reaction between KI and KClO3: KI + KClO3 = KIO3 + KCl
or oxidation with excess chlorine:
KI + 3Cl2(excess) + 6KOH = KIO3 + 6KCl + 3H2O
(KIO3 can be isolated by crystallization)
or from 3I2 + 6KOH = KIO3 + 5KI + 3H2O

and what are the differemces in reactivity of products: bromate, iodate and chlorate?

Analyze the Frost diagrams for halogens and compare standard reduction potentials for XO₃^-/X₂. For Cl, Br and I the values of E° are 1.468, 1.478 and 1.195 V respectively.
The oxidizing ability of XO₃^- is decreasing in order: BrO₃^- ≈ ClO₃^- > IO₃^-. The bromates are the strongest oxidizing agents.
2KBrO3 + I2 = 2KIO3 + Br2
2KBrO3 + Cl2 = 2KClO3 + Br2
2KClO3 + I2 = 2KIO3 + Cl2

5) how to prepare KIO3 from Cl2, KI and K2CO3:

Chlorine liberates I2 from KI and then it oxidizes I2 to iodate:
2KI + Cl2 = I2 + 2KCl
Cl2(excess) + I2 + 12K2CO3 + 6H2O = 2KIO3 + 10KCl + 12KHCO3

PS electrolysis with diaphragm would give you a regular chloralkali process, where NaOH is produced and it does not come into contact with Cl2 gas, so there is no reaction between NaOH and Cl2 to produce NaClO3

[snorkack]

3) how to prepare
A. barium chlorate:
B.nickel chlorate:

It can be prepared from barium chloride (common reagent) and NaClO3 (produced industrially in large scale):
BaCl2 + 2NaClO3 = 2NaCl + Ba(ClO3)2
Barium chlorate can be crystallized from solution.
For nickel(II) chlorate I would suggest similar reaction.

But this depends on the specifics of solubility of nickel chlorate, the nickel salt used and the corresponding sodium salt.
A problem with using sodium salts to produce other salts is that sodium has few poorly soluble salts to drive formation of the desired salts.