CHEM 1A03 Study Guide - Final Guide: Ammonium Acetate, Ammonium Chloride, Sodium Acetate

42 views6 pages

maroondolphin567

12 Dec 2017

School

Department

Course

Professor

For unlimited access to Study Guides, a Grade+ subscription is required.

itsmealionline and 39769 others unlocked

CHEM 1A03 Full Course Notes

Verified Note

35 documents

Document Summary

Can qualitatively predict a solution as acidic or basic when dissolved in water. Another way is to imagine where ions came form in an acid-base reaction. Sodium ions could come from sodium hydroxide (strong base) Chloride ions could come from hcl (strong acid) Strong acid and strong base neutralize one another, results in neutral salt from the spectator ions and water. Ammonium chloride dissolves in water -> ammonium and chloride ions. Chloride does(cid:374)"t rea(cid:272)t (cid:449)ith (cid:449)ater, (cid:271)ut a(cid:373)(cid:373)o(cid:374)iu(cid:373) io(cid:374) is a (cid:449)eak a(cid:272)id a(cid:374)d rea(cid:272)ts to produ(cid:272)e ammonia and h3o+ A small amount of h3o+ is produced, therefore the salt is an acidic salt, (ph<7) Alternatively, can say ammonium chloride comes from reaction between ammonia and hcl (weak base reacts with strong acid) The strong acid overwhelms the weak base and final product is slightly acidic. We get sodium and acetate ions when sodium acetate is dissolved in water.

Related Questions

Fill the questions according to Data Table 7-2

5. balanced formula equation: for each combination of solutions that produced new product. write correct chemical formulas for the new compounds that could form from the ions present. Indicate which of the new compunds is a precipitate. If no reaction occurs, write NR.

6. complete ionic equation: write complete ionic equations for the precipitation reactions that you observed. show the reactants as ions, the precipitate as a solid, and the spectator ions as unchanged. balance each equation for mass and change. the total charge should be zero on each side of the equation.

7. net ionic equation: write the net ionic equations for each reaction in the preceding question.

Why do ionic compounds dissolve well in water? Select all that are true.

Question 5 options:

Because water and ionic compounds are both polar

Water molecules have partial charges that attract the ions in the solid compound, causing it to dissociate into separated ions

Because organic compounds are nonpolar

Water molecules can surround an ion, and neutralize the ion's charge using either it's partial positive or negative side.

The individual ions are solvated by water molecules which stabilizes the ions

2. Which compound is soluble in ether but not soluble in aqueous sodium hydroxide?

Question 2 options:

	ArOH
	Ar
	ArCOOH

Save

When you have a two-layer mixture of water and tert-butyl methyl ether, what physical property of these liquids assures you that the ether is the top layer?

Question 4 options:

low density was my answer was

You perform each extraction twice, first with 1 mL and second with 0.15 mL. Why is the second extraction necessary?

Question 8 options:

	several small extractions is better than one large one
	to remove any orgnaic material contaninating tube 2
	to remove any remaining neutral compound

7. Which of the following reactions is not favorable?

Question 7 options:

	ArCOOH + NaOH â ArCOO^-Na⁺ + H₂O
	ArOH + NaHCO₃ â ArO^-Na⁺ + CO₂ + H₂O
	ArCOOH + NaHCO₃ â ArCOO^-Na⁺ + CO₂ + H₂O

9.Why is phenol more acidic than an aliphatic alcohol?

Question 9 options:

	Its conjugates baseâs negative charge is localized on the oxygen
	Phenols have a stronger O-H bond
	Only the phenol can form hydrogen bonds
	Its conjugated base is stabilized by resonance

Which aqueous base reacts with a carboxylic acid but not with phenol? Why?

Question 10 options:

	Sodium bicarbonate, it is a weaker base and will only react with strong acids
	Sodium hydroxide, it is a strong base and will only react with strong acids
	Sodium bicarbonate, it is a weak base and will only react with weak acids
	Sodium hydroxide, it is a strong base and will only react with weak acids

CHEM 1A03 Study Guide - Final Guide: Ammonium Acetate, Ammonium Chloride, Sodium Acetate

CHEM 1A03 Full Course Notes

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 1A03 Lecture Notes - Lecture 8: Svante Arrhenius, Trioxidane, Amphoterism

CHEM 1A03 Study Guide - Final Guide: Lattice Energy, Heat Capacity, Solvation

CHEM 1A03 Lecture Notes - Lecture 3: Aluminium Oxide, Calcium Hydroxide, Noble Gas

Related Questions