How Much Do You Know About Chemical Solubility?
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Always Soluble?
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Alkali metal ions: Li+, Na+, K+, Rb+, Cs+
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Ammonium: NH4+
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CO32-
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Nitrogen NO2
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Chemistry revolves around solutes and solubility. How much do you know about chemical solubility? Play this quiz to assess your knowledge of solubility rules. Chemistry is a complex subject to master. Do you know what are solute, solvent, and solution? The quiz contains various questions and facts that will help you ace chemical solubility concepts. Take the online quiz to See moretest yourself and learn more. If you like the quiz, share it with your friends and family. All the best!
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- 2.
Always soluble?
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CO3 (2-), PO4 (3-),CLO3 (1-)
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CL-, Br-, I-
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ClO3(1-), CLO4(1-)
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NaOH+ KOH= COOH+Na2CO3
Correct Answer
A. ClO3(1-), CLO4(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.Rate this question:
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- 3.
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!
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2AgNO3(aq) +Na2SO4(aq) = 2NaNO3(aq) + Ag2SO4(s)
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BaCl2(aq) + ZnSO4(aq) = ZnCl2(s) + BaSO4(aq)
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NaNO3 + KOH = KNO3(aq) + NaOH(aq)
Correct Answer
A. 2AgNO3(aq) +Na2SO4(aq) = 2NaNO3(aq) + Ag2SO4(s)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.Rate this question:
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- 4.
Insoluble?F-
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True
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False
Correct Answer
A. FalseExplanation
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.Rate this question:
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- 5.
Which of the following polyatomic ions that contain oxygen are soluble?
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NO3-
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ClO3-
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CO3 (2-)
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C2O4(2-)
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ClO4-
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C2H3O2-
Correct Answer(s)
A. NO3-
A. ClO3-
A. ClO4-
A. C2H3O2-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.Rate this question:
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- 6.
Insoluble?K2CO3
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True
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False
Correct Answer
A. False -
- 7.
Which of the following are insolubility exceptions for Cl- ?
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Ag+
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Hg2 (2+)
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K+
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Pb (2+)
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Sr (2+)
Correct Answer(s)
A. Ag+
A. Hg2 (2+)
A. Pb (2+)Explanation
potassium is an alkali
Sr(2+) is not an exception for Cl, however it is an exception for SO4 (2-)Rate this question:
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- 8.
Insoluble?
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O(2-)
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OH-
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PO4(3-)
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S(2-)
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C2O4(2-)
Correct Answer(s)
A. O(2-)
A. OH-
A. PO4(3-)
A. S(2-)
A. C2O4(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.Rate this question:
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- 9.
Which of the following are not a soluble ions
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H2
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Na+
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Cl-
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Br
Correct Answer
A. H2 -
- 10.
Generally insoluble: O(2-) OH(-) CO3(2-) NO3(-)
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True
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False
Correct Answer
A. FalseExplanation
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.Rate this question:
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- 11.
Which of the following is not an polyatomic ions?
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C2H3O2 (-)
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NO3 (-)
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NH4(+)
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CO
Correct Answer
A. COExplanation
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.Rate this question:
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- 12.
Exceptions for I (-):Ag(+)Pb(2+)Hg2(2+)
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True
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False
Correct Answer
A. TrueExplanation
HINT: the exceptions are the same for Cl-, Br-, and I- (all are halogens, missing F)Rate this question:
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- 13.
Exceptions for SO4(2-)
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Alkali metal ions
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Ca(2+)
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Sr(2+)
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Ba(2+)
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Pb(2+)
Correct Answer(s)
A. Ca(2+)
A. Sr(2+)
A. Ba(2+)
A. Pb(2+)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+Rate this question:
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- 14.
Soluble exceptions for O(2-) and OH(-):alkali metal ionsNH4(+)Ca(2+)Sr(2+)Ba(2+)
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True
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False
Correct Answer
A. TrueExplanation
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.Rate this question:
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Current Version
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Aug 15, 2024Quiz Edited by
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Oct 11, 2010Quiz Created by
Ajernigan
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