6. Chemical Quantities & Aqueous Reactions

Osmolarity

what is the molarity of Cl- in each solution?
a. 0.200 M NaCl

Calculating the Osmolarity of a Solution

what is the molarity of Cl- in each solution?
c. 0.100 M AlCl3

What is the molarity of each ion in a solution prepared by dissolving 0.550 g of Na2SO4, 1.188 g of Na3PO4, and 0.223 g of Li2SO4 in water and diluting to a volume of 100.00 mL?

Calculate the concentration of each ion in the following 
solutions obtained by mixing: (b) 60.0 mL of 0.100 M ZnCl2 
with 5.0 mL of 0.200 M Zn(NO3)2, 
Assume that the volumes are additive.

Unit 3 Osmolarity

(a) Which will have the highest concentration of sodium ions:
0.25 M NaCl, 0.15 M Na2CO3, or 0.075 M Na3PO4?

An aqueous solution contains 1.2 mM of total ions. (a) If the
solution is NaCl(aq), what is the concentration of chloride
ion?

Refer to the figure to answer questions 4 and 5. The images are a molecular representation of three different substances, AX3, AY3, and AZ3, dissolved in water. (Water molecules are omitted for clarity.) 
What are the molar concentrations of A ions and X ions in a 0.500 M solution of AX3? (LO 4.7)
(a) 0.500 M A and 0.500 M X 
(b) 0.500 M A and 0.167 M X 
(c) 1.500 M A and 0.500 M X 
(d) 0.500 M A and 1.500 M X

Osmolarity Example 3

How many bromide ions are present in 65.5 mL of 0.210 M GaBr3&nbsp;solution?

Osmolality Vs Osmolarity (with a mnemonic)

Using Molarity of compounds and L of solutions, moles of ions&nbsp;can be calculated.

Calculate the concentration of each ion in the following 
solutions obtained by mixing: (c) 4.2g of CaCl2 in 150.0mL 
of 0.02 M KCl solution. 
Assume that the volumes are additive.

What is the total molar concentration of ions in each of the following solutions, assuming complete dissociation? 
(b) A 0.355 M solution of AlCl3

Which of the following solutions will have the highest concentration of bromide ions?

Osmolarity Example 2

Ignoring protolysis reactions, indicate the concentration 
of each ion or molecule present in the following solutions: 
(b) 5 * 10-4 M CuCl2

What is the molarity of NO3- in each solution?
a. 0.150 M KNO3
b. 0.150 M Ca(NO3)2
c. 0.150 M Al(NO3)3

Consider two solutions, the first being 50.0 mL of
1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH.
When the two solutions are mixed in a constant-pressure
calorimeter, a precipitate forms and the temperature of the
mixture rises from 21.5 to 27.7 °C. (a) Before mixing, how
many grams of Cu are present in the solution of CuSO4?

What is the mass of chloride ions in 375.0 mL of solution with a magnesium chloride concentration of 0.250 M? (LO 4.2)
(a) 3.32 g
(b) 47.3 g 
(c) 23.6 g
d) 6.65 g

what is the molarity of Cl- in each solution?
b. 0.150 M SrCl2

What is the total molar concentration of ions in each of the following solutions, assuming complete dissociation? 
(a) A 0.750 M solution of K2CO3

Osmolarity from Molarity of compound:

Chemistry Basics:  Osmolarity, Osmolality and Tonicity

What is the total molar concentration of ions in each of the following solutions?
(a) A 1.250 M solution of CH3OH

Direct Calculation of Osmolarity:

Osmolarity vs Osmolality

Calculate the concentration of each ion in the following
solutions obtained by mixing: (a) 32.0 mL of 0.30 M KMnO4
with 15.0 mL of 0.60 M KMnO4
Assume that the volumes are additive.

Osmolarity Example 1

Ignoring protolysis reactions, indicate the concentration 
of each ion or molecule present in the following solutions: 
(d) a mixture of 35.0 mL of 0.010 M Na2CO3 and 
50.0 mL of 0.200 M K2SO4. Assume the volumes are additive.

What is the total molar concentration of ions in each of the following solutions?
(b) A 0.225 M solution of HClO4

An aqueous solution contains 1.2 mM of total ions. (b) If the solution is FeCl3(aq), what is the concentration 
of chloride ion?

How many milligrams of nitride ions are required to prepare 820 mL of 0.330 M Ba3N2 solution?

Ringer’s solution, used in the treatment of burns and wounds, is prepared by dissolving 4.30 g of NaCl, 0.150 g of KCl, and 0.165 g of CaCl2 in water and diluting to a volume of 500.0 mL. What is the molarity of each of the component ions in the solution?

(b) Which will contain the greater number of moles of sodium ion:
20.0 mL of 0.15 M NaHCO3 or 15.0 mL of 0.04 M Na2S?

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17. Acid and Base Equilibrium

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[BOOK CHEM] Clutch Version

Solutions

Solutions represent homogeneous mixtures made of 2 or more components that form a uniform composition.&nbsp;

Osmolarity (ionic molarity) represents the number of moles of ions per liter of solution.&nbsp;

Gas Evolution Equations

A Gas Evolution Equation is a molecular equation that involves the creation of specific gases.&nbsp;

Molecular Equations

Molecular Equations show reacting molecules involved in a chemical reaction.&nbsp;

Complete Ionic Equations

Complete Ionic Equations show aqueous compounds as fully dissociated ions.&nbsp;

Solubility Rules

The Solubility Rules are a convenient set of guidelines to help us determine if a compound will be soluble or insoluble.

Molarity

Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.&nbsp;

Electrolytes

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.&nbsp;

Solution Stoichiometry

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Calculate Oxidation Numbers

Calculating Oxidation Numbers is the first pivotal step in understanding redox reactions.&nbsp;

Dilutions

In Dilutions, a solvent (usually water) is added to a concentrated solution.&nbsp;

Redox Reactions

Redox Reactions (oxidation-reduction reactions) involve transference of an electron(s) between reactants.

Activity Series

Activity Series is a list of single displacement reactions in order of reactivity.

Balancing Redox Reactions: Acidic Solutions

Balancing Redox Reactions requires a new approach that accounts for the transfer of electrons between reactants.

Balancing Redox Reactions: Basic Solutions

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.