CH-1010 Chapter Notes - Chapter 8: Chemical Equation, Strong Electrolyte, Spectator Ion

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14 Nov 2016

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Molarity (m)- the number of moles of solute per liter of solution: m=n/v; also called molar concentration. Standard solution- a solution of known concentration that is used in chemical analysis. Dilution- the process of lowering the concentration of a solution by adding more solvent. Electrode- a solid electrical conductor that is used to make contact with a solution or other nonmetallic component of an electrical circuit. Electrolyte- a material that conducts electricity because it contains free ions; ionic solutions and molten salts are examples of electrolytes. Strong electrolyte- an ionic substance that dissociates completely when it dissolves in water. Nonelectrolyte- a molecular substance that does not dissociate into ions when it dissolves in water. Hydronium ion (+)- an h+ion plus a water molecule, h2o; the form in. Bronsted-lowry model- defines acids as h+ ion donors and bases as h+ion which the hydrogen ion is found in an aqueous solution.

Related Questions

The Behavior of Substances in Water

Part 1:

Ammonia, NH₃, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols.
From everyday experience, you are probably aware that table sugar (sucrose), C₁₂H₂₂O₁₁, is soluble in water. When sucrose dissolves in water, it doesn’t form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water.
Both NH₃ and C₁₂H₂₂O₁₁ are soluble molecular compounds, yet they behave differently in an aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte.
Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water.
Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes?
Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte.
Classify each of the following substances as either ionic or molecular:

KCl
NH₃
CO₂
MgBr₂
HCl
Ca(OH)₂
PbS
HC₂H₃O₂

For those compounds above that, you classified as ionic, use the solubility rules to determine which are soluble.
The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water.
Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water?
How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer.
Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m
Are NaCl and HI strong electrolytes because they have similar behavior in an aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case.

Part 2:

You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water.

AX (aq) + H₂O (l) → AH₂O⁺ (aq) + X⁻ (aq)

AY (aq) + H₂O (l) → AH₂O⁺ (aq) + Y⁻ (aq)

Explain how the relative amounts of AX ( aq ) and AY ( aq ) would compare if you had a beaker of water with AX and a beaker of water with AY.
How would the relative amounts of X⁻ ( aq) and Y⁻ ( aq) in the two beakers compare? Be sure to explain your answer.

indigolouse566

What distinguishes (on an atomic/molecular level) electrolytes from non-electrolytes?
i. Ability to conduct electricity
ii. Ionic compounds dissociate into ions
iii. Substance that dissolves in water to yield a solution that conducts electricity
iv. Molecular compounds ionize into ions
v. Acids and bases are the 2 types of molecular compounds which are electrolytes
a) i, ii, iii, and v only
b) all of i, ii, iii, iv, and v
c) i only
d) i, ii, iii, and iv only
e) i and ii only

What is the total concentration of all ions (the sum of their individual concentrations) in aqueous solutions of the following?

Hint: Each substance is an electrolyte that dissociates in water to produce ions. Use the link table of polyatomic ions if you do not recognize the polyatomic ion. For example, Na₂SO₄ -> 2Na¹⁺ + SO₄^2- when it dissolves, so a 1 M soln of Na₂SO₄ is 2M in Na¹⁺ and 1M in SO₄^2- and the total concentration of ions is 2 M + 1 M = 3M.

0.0760-M CaCl₂	_____________ M
0.0160-M Na₂SO₄	_____________ M
0.0740-M K₂Cr₂O₇	_____________ M

CH-1010 Chapter Notes - Chapter 8: Chemical Equation, Strong Electrolyte, Spectator Ion

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