How Much Do You Know About Chemical Solubility?

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.

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.

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.

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.

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.

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

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.

Explanation
O(2-) (Oxygen with a charge of -2): This ion typically forms compounds with metals, creating oxides, but it is generally not soluble in water.
OH(-) (Hydroxide ion): Hydroxide ions are the conjugate base of water (H2O), and they are weak bases. They are indeed soluble in water, and the resulting solution is called an alkaline or basic solution. However, the solubility can vary depending on the specific compound.
CO3(2-) (Carbonate ion): Carbonate ions can form insoluble compounds with many metal cations. Calcium carbonate (CaCO3) and lead(II) carbonate (PbCO3) are examples of insoluble carbonates.
NO3(-) (Nitrate ion): Nitrate ions are typically soluble in water. Compounds containing nitrate ions are often soluble and do not form significant precipitates.
So, while the solubility of some compounds can be affected by various factors, the statement is generally true for the ions mentioned, with the exception of OH(-) being generally soluble in water.

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.

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

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+

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.