1. AQUEOUS ACIDS
AND
THEIR SALTS

2. Aqueous acids
Aqueous acids are the result of replacing the positive ion in a salt with hydrogen ion and then dissolving the compound in water. To visually do this on the computer is much easier than actually doing the same replacement reaction in the chemistry laboratory. However for naming purposes this will be the approach taken here.

3. There is a systematic process in the naming of inorganic acids
There is a systematic process in the naming of inorganic acids. Probably the most significant problem is the variation of oxidation numbers for the negative ions.
For example
Cl-1 chloride ion
NO3-1 nitrate ion
SO4-2 sulfate ion
PO4-3 phosphate ion

4. Another significant problem is that many of the other polyatomic ions with the same endings on their names have a different number of oxygen atoms attached to the central atom.
For example
chlorate ClO3-1
sulfate SO4-2
phosphate PO4-3
acetate C2H3O2-1

5. but a varying number of oxygen atoms
Rather than memorize all the polyatomic
Ions it is much more useful to learn their trends in the naming scheme. There are numerous patterns within a homologous series.
For example
ClO4-1 perchlorate
ClO chlorate
ClO chlorite
ClO hypochlorite
Cl chloride (not a polyatomic ion)
ClO4-1 perchlorate
ClO chlorate
ClO chlorite
ClO hypochlorite
Cl chloride
ClO4-1 perchlorate
ClO chlorate
ClO chlorite
ClO hypochlorite
Cl chloride
ClO4-1 perchlorate
ClO chlorate
ClO chlorite
ClO hypochlorite
Cl chloride
All the names contain chlor indicating that the ion contains chlorine
All the ions contain one chlorine atom
but a varying number of oxygen atoms
All have a minus one charge

6. The oxy-ions of chlorine, bromine and iodine all have these trends in common. Look for them below……
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
Perbromate BrO4-1
Bromate BrO3-1
Bromite BrO2-1
Hypobromite BrO-1
Periodate IO4-1
Iodate IO3-1
Iodite IO2-1
Hypoiodite IO-1
The most productive method of committing these ions to memory is first memorize the ones that have the _____ate ending. . This is the most common ending.

7. POLYATOMIC IONS Ions with -1 charge perbromate BrO4-1 bromate BrO3-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
thiocyanate SCN-1
acetate C2H3O2-1
permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
phthalate C8H4O4-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
peroxide O2-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1

8. The table below shows the prefixes and suffixes that tell the number of oxygen atoms present in the negative ion.
Salt
metal polyatomic ion # Oxygen atoms
________ per_____ate 4
________ _____ate 3
________ _____ite 2
________ hypo_____ite 1
________ _____ide 0

9. the aqueous acid names are simply an extension of the salt names.
REMEMBER
the aqueous acid names are simply an extension of the salt names.

11. Salt Aqueous Acid metal polyatomic ion hydrogen polyatomic ion
________ per_____ate
________ _____ate
________ _____ite
________ hypo_____ite
________ _____ide
Aqueous Acid
hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the metal per____ate salt into its
corresponding aqueous acid name:
1) The name of the metal is dropped
2) The -ate ending is replaced with –ic
3) The word acid is added to the name
For example:
potassium perchlorate > perchloric acid
KClO4(s) > HClO4 (aq)

12. Salt Aqueous Acid metal polyatomic ion hydrogen polyatomic ion
________ per_____ate
________ _____ate
________ _____ite
________ hypo_____ite
________ _____ide
Aqueous Acid
hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the metal _____ate salt into its
corresponding aqueous acid name:
1) The name of the metal is dropped
2) The -ate ending is replaced with –ic
3) The word acid is added to the name
For example:
sodium acetate > acetic acid
NaC2H3O2(s) > HC2H3O2(aq)

13. Salt Aqueous Acid metal polyatomic ion hydrogen polyatomic ion
________ per_____ate
________ _____ate
________ _____ite
________ hypo_____ite
________ _____ide
Aqueous Acid
hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the metal_____ite salt into its
corresponding aqueous acid name:
1) The name of the metal is dropped
2) The -ite ending is replaced with –ous
3) The word acid is added to the name
For example:
ammonium nitrite > nitrous acid
NH4NO2(s) > HNO2(aq)

14. Salt Aqueous Acid metal polyatomic ion hydrogen polyatomic ion
________ per_____ate
________ _____ate
________ _____ite
________ hypo_____ite
________ _____ide
Aqueous Acid
hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the metal hypo_____ite salt into its
corresponding aqueous acid name:
1) The name of the metal is dropped
2) The -ite ending is replaced with –ous
3) The word acid is added to the name
For example:
lithium hypoiodite > hypoiodous acid
LiIO (s) > HIO (aq)

15. Salt Aqueous Acid metal polyatomic ion hydrogen polyatomic ion
________ per_____ate
________ _____ate
________ _____ite
________ hypo_____ite
________ _____ide
Aqueous Acid
hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the metal _____ide salt into its
corresponding aqueous acid name:
1) The name of the metal is dropped
2) The -ide ending is replaced with hydro____ic
3) The word acid is added to the name
For example:
silver bromide > hydrobromic acid
AgBr(s) > HBr(aq)

16. The following exercises will deal
only with the names and formulas
of aqueous acids. The names and
formulas for the salts were studied
in detail in a previous lesson.

17. Example #1-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

18. Example #2-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

19. Example #3-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

20. Example #4-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

21. Example #5-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

22. Example #6-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

23. Example #7-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

24. Example #8-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

25. Example #9-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

26. Example #9-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

27. Example #10-Names to Formulas
chloric acid
Determine the formula & charge of the polyatomic ion
chlorate
2. Add hydrogen ions +1 -1 H
ClO3 =0
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript: (aq)

28. Examples #1- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

29. Examples #2- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

30. Examples #3- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

31. Examples #3- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

32. Examples #4- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

33. Examples #5- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

34. Examples #6- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

35. Examples #7- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

36. Examples #8- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

37. Examples #9- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

38. Examples #10- Formulas to Names
HBrO2(aq)
1. The hydrogen out front & the (aq) subscript indicates an acid
bromite
2. Determine the ion and it’s acid ending.
____________ acid
bromous acid
Final Name

41. Practice Problem #1 No, it contains more oxygen atoms
HIO4(aq)
Choose the correct name for the compound
1. iodic acid
No, it contains more oxygen atoms
2. iodous acid
No, it contains more oxygen atoms
3. periodic acid
Very good, click arrow to continue
4. hydrogen periodate
No, you need to use the acid name
5. none of the above
No, there is a correct answer
next problem
Ion list

42. Practice Problem #2 No, it has too many oxygen atoms
hydrobromic acid
Choose the correct formula for the compound
1. HBrO(aq)
No, it has too many oxygen atoms
HBr(aq)
Very good, click arrow to continue
3. HBrO3(aq)
No, you have too many oxygen atoms
4. HBrO2(aq)
No, you have too many oxygen atoms
5. none of the above
No, there is a correct answer
next problem
Ion list

43. POLYATOMIC IONS return Ions with -1 charge perbromate BrO4-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
thiocyanate SCN-1
acetate C2H3O2-1
permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
phthalate C8H4O4-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
peroxide O2-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1
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