How Much Do You Know About Chemical Solubility?

1. Exceptions for I (-):
Ag(+)
Pb(2+)
Hg2(2+)

True

False

HINT: the exceptions are the same for Cl-, Br-, and I- (all are halogens, missing F)

Explanation

HINT: the exceptions are the same for Cl-, Br-, and I- (all are halogens, missing F)

2. Which of the following is not an polyatomic ions?

C2H3O2 (-)

NO3 (-)

NH4(+)

CO

CO is not a polyatomic ion because it is a diatomic molecule composed of two atoms (carbon and oxygen) rather than a single atom or a group of atoms with a charge. Polyatomic ions are formed when multiple atoms combine and carry a charge, such as C2H3O2 (-) and NO3 (-). NH4(+) is also a polyatomic ion, known as the ammonium ion.

Explanation

CO is not a polyatomic ion because it is a diatomic molecule composed of two atoms (carbon and oxygen) rather than a single atom or a group of atoms with a charge. Polyatomic ions are formed when multiple atoms combine and carry a charge, such as C2H3O2 (-) and NO3 (-). NH4(+) is also a polyatomic ion, known as the ammonium ion.

3. Insoluble?
K2CO3

True

False

not-available-via-ai

Explanation

not-available-via-ai

4. Always Soluble?

Alkali metal ions: Li+, Na+, K+, Rb+, Cs+

Ammonium: NH4+

CO32-

Nitrogen NO2

HINT: all of the polyatomic ions that are always soluble have a charge of negative 1 except for the ammonium ion which has a charge of positive 1.

Explanation

HINT: all of the polyatomic ions that are always soluble have a charge of negative 1 except for the ammonium ion which has a charge of positive 1.

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5. Which of the following are insolubility exceptions for Cl- ?

Ag+

Hg2 (2+)

K+

Pb (2+)

Sr (2+)

potassium is an alkali
Sr(2+) is not an exception for Cl, however it is an exception for SO4 (2-)

Explanation

potassium is an alkali
Sr(2+) is not an exception for Cl, however it is an exception for SO4 (2-)

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6. Generally insoluble: O(2-) OH(-) CO3(2-) NO3(-)

True

False

Among the given ions, most are generally insoluble, except for NO₃⁻ (nitrate). Nitrate ions are typically soluble in water, regardless of the metal cation they are paired with. In contrast, O²⁻ (oxide), OH⁻ (hydroxide), and CO₃²⁻ (carbonate) are usually insoluble unless paired with alkali metals or ammonium ions.

Explanation

Among the given ions, most are generally insoluble, except for NO₃⁻ (nitrate). Nitrate ions are typically soluble in water, regardless of the metal cation they are paired with. In contrast, O²⁻ (oxide), OH⁻ (hydroxide), and CO₃²⁻ (carbonate) are usually insoluble unless paired with alkali metals or ammonium ions.

7. Which of the following are not a soluble ions

H2

Na+

Cl-

Br

not-available-via-ai

Explanation

not-available-via-ai

8. Soluble exceptions for O(2-) and OH(-):
alkali metal ions
NH4(+)
Ca(2+)
Sr(2+)
Ba(2+)

True

False

The given answer is true because alkali metal ions (such as NH4(+), Ca(2+), Sr(2+), and Ba(2+)) are exceptions to the general rule that hydroxides (OH(-)) and peroxides (O(2-)) are insoluble. These alkali metal ions form soluble compounds with hydroxides and peroxides, unlike other metal ions.

Explanation

The given answer is true because alkali metal ions (such as NH4(+), Ca(2+), Sr(2+), and Ba(2+)) are exceptions to the general rule that hydroxides (OH(-)) and peroxides (O(2-)) are insoluble. These alkali metal ions form soluble compounds with hydroxides and peroxides, unlike other metal ions.

9. Always soluble?

CO3 (2-), PO4 (3-),CLO3 (1-)

CL-, Br-, I-

ClO3(1-), CLO4(1-)

NaOH+ KOH= COOH+Na2CO3

in answer choice one only CLO3 is always soluble but the rest are NEVER soluble. (Hint: you can tell because the other two ions in this option have higher than a 1- charge) In question two: all of these ions are soluble but not ALWAYS soluble. if they are paired with an ion that is never soluble then the compound is a solid.

Explanation

in answer choice one only CLO3 is always soluble but the rest are NEVER soluble. (Hint: you can tell because the other two ions in this option have higher than a 1- charge) In question two: all of these ions are soluble but not ALWAYS soluble. if they are paired with an ion that is never soluble then the compound is a solid.

10. Insoluble?
F-

True

False

The given answer is false because the term "insoluble" refers to a substance that cannot be dissolved in a solvent. Since the question only provides the term "insoluble" without any context or additional information, it is not possible to determine whether it is true or false. Hence, the correct answer cannot be determined based on the given information.

Explanation

The given answer is false because the term "insoluble" refers to a substance that cannot be dissolved in a solvent. Since the question only provides the term "insoluble" without any context or additional information, it is not possible to determine whether it is true or false. Hence, the correct answer cannot be determined based on the given information.

11. Which of the following polyatomic ions that contain oxygen are soluble?

NO3-

ClO3-

CO3 (2-)

C2O4(2-)

ClO4-

C2H3O2-

Polyatomic ions that contain oxygen are generally soluble, except for a few exceptions. In this case, NO3-, ClO3-, ClO4-, and C2H3O2- are soluble because they are all common ions that are generally soluble in water. On the other hand, CO3(2-) and C2O4(2-) are insoluble because they are carbonate and oxalate ions, respectively, which form insoluble salts with many cations.

Explanation

Polyatomic ions that contain oxygen are generally soluble, except for a few exceptions. In this case, NO3-, ClO3-, ClO4-, and C2H3O2- are soluble because they are all common ions that are generally soluble in water. On the other hand, CO3(2-) and C2O4(2-) are insoluble because they are carbonate and oxalate ions, respectively, which form insoluble salts with many cations.

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12. Exceptions for SO4(2-)

Alkali metal ions

Ca(2+)

Sr(2+)

Ba(2+)

Pb(2+)

hint: all of S02(2-) exceptions have a charge of (2+) and the alkali metal ions are ALWAYS soluble, they also have a charge of 1+

Explanation

hint: all of S02(2-) exceptions have a charge of (2+) and the alkali metal ions are ALWAYS soluble, they also have a charge of 1+

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13. Which of the following has the correct state lable in the equation? [(aq) or (s)] ("=" means yields) do not trust the state lables on the pre net ionic equations, they may try to fool you!

2AgNO3(aq) +Na2SO4(aq) = 2NaNO3(aq) + Ag2SO4(s)

BaCl2(aq) + ZnSO4(aq) = ZnCl2(s) + BaSO4(aq)

NaNO3 + KOH = KNO3(aq) + NaOH(aq)

In the first chemical equation, silver nitrate (AgNO3) reacts with sodium sulfate (Na2SO4) in an aqueous solution, yielding sodium nitrate (NaNO3) and silver sulfate (Ag2SO4), which precipitates as a solid. State labels indicate the physical states of substances before and after the reaction.

Explanation

In the first chemical equation, silver nitrate (AgNO3) reacts with sodium sulfate (Na2SO4) in an aqueous solution, yielding sodium nitrate (NaNO3) and silver sulfate (Ag2SO4), which precipitates as a solid. State labels indicate the physical states of substances before and after the reaction.

14. Insoluble?

O(2-)

OH-

PO4(3-)

S(2-)

C2O4(2-)

The given answer lists various ions, including O(2-), OH-, PO4(3-), S(2-), and C2O4(2-). These ions are all negatively charged and are commonly found in chemical compounds. The suffix "-ate" in PO4(3-) and C2O4(2-) indicates that these ions are polyatomic ions. Overall, the answer correctly identifies these ions as being insoluble, meaning they do not readily dissolve in water.

Explanation

The given answer lists various ions, including O(2-), OH-, PO4(3-), S(2-), and C2O4(2-). These ions are all negatively charged and are commonly found in chemical compounds. The suffix "-ate" in PO4(3-) and C2O4(2-) indicates that these ions are polyatomic ions. Overall, the answer correctly identifies these ions as being insoluble, meaning they do not readily dissolve in water.

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