This site is specifically for my students, but others are welcome to come and peruse it. for tennis lovers-- http://www.hi10spro.blogspot.com
ac calendar
Wednesday, September 29, 2010
Debate Practice
i leave on Oct 9 for Khon Kaen for a family vacation. I want to practice the Tuesday through Thursday before I go
Wednesday, September 22, 2010
Monday, September 20, 2010
Ch 16 Review Questions
molarity
Calculate the molarity of each of the following solutions.
a. 0.40 mol of NaCl dissolved in 1.6 L of solution
20.2 g of potassium nitrate, KNO3, in enough water to make 250.0 mL of
solution
dilution
You must prepare 300.0 mL of 0.750M NaBr solution using 2.00M NaBr stock solution. How many milliliters of stock solution should you use?
5. In order to dilute 1.0 L of a 6.00M solution of NaOH to 0.500M solution
how
much water must you add?
v/v
6. What is the concentration in percent by volume, %(v/v), of the following
solutions?
a. 60.0 mL of methanol in a total volume of 500.0 mL
b. 25.0 mL of rubbing alcohol (C3H7OH) diluted to a volume of 200.0 mL
with water
7. How many grams of solute are needed to prepare each of the following
solutions?
a. 1.00 L of a 3.00% (m/m) NaCl solution?
b. 2.00 L of 5.00% (m/m) KNO3 solution?
How many particles in solution are produced by each formula unit of potassium carbonate, K2CO3?
3. How may moles of particles would 3 mol Na2SO4 give in solution?
Calculate the mole fraction of solute in each of the following solutions.
a. 3.0 moles of lithium bromide, LiBr, dissolved in 6.0 moles of water
Find the molality of each of the following solutions.
a. 2.3 moles of glucose dissolved in 500.0 g of water
b. 131 g of Ba(NO3)2 dissolved in 750.0 g of water
Calculate the molarity of each of the following solutions.
a. 0.40 mol of NaCl dissolved in 1.6 L of solution
20.2 g of potassium nitrate, KNO3, in enough water to make 250.0 mL of
solution
dilution
You must prepare 300.0 mL of 0.750M NaBr solution using 2.00M NaBr stock solution. How many milliliters of stock solution should you use?
5. In order to dilute 1.0 L of a 6.00M solution of NaOH to 0.500M solution
how
much water must you add?
v/v
6. What is the concentration in percent by volume, %(v/v), of the following
solutions?
a. 60.0 mL of methanol in a total volume of 500.0 mL
b. 25.0 mL of rubbing alcohol (C3H7OH) diluted to a volume of 200.0 mL
with water
7. How many grams of solute are needed to prepare each of the following
solutions?
a. 1.00 L of a 3.00% (m/m) NaCl solution?
b. 2.00 L of 5.00% (m/m) KNO3 solution?
How many particles in solution are produced by each formula unit of potassium carbonate, K2CO3?
3. How may moles of particles would 3 mol Na2SO4 give in solution?
Calculate the mole fraction of solute in each of the following solutions.
a. 3.0 moles of lithium bromide, LiBr, dissolved in 6.0 moles of water
Find the molality of each of the following solutions.
a. 2.3 moles of glucose dissolved in 500.0 g of water
b. 131 g of Ba(NO3)2 dissolved in 750.0 g of water
Chem review EP 5
Find the percent by mass of water in
NiCl2 * 6H2O.
In your own words, explain hydrogen bonds.
Draw a diagram of the hydrogen bonding between three water molecules.
Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
Draw a diagram of the hydrogen bonding between three water molecules.
Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
Identify the solute and solvent in a dilute aqueous solution of potassium chloride.
Which of the following compounds are soluble in water? Which are insoluble?
a. CaCl2
b. N2
c. HBr
d. NH4C2H3O2
Write the formulas for the following hydrates.
a. Calcium sulfate dihydrate
b. Cobalt(II) chloride hexahydrate
NiCl2 * 6H2O.
In your own words, explain hydrogen bonds.
Draw a diagram of the hydrogen bonding between three water molecules.
Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
Draw a diagram of the hydrogen bonding between three water molecules.
Explain why the density of ice at 0°C is less than the density of liquid water at 0°C.
Identify the solute and solvent in a dilute aqueous solution of potassium chloride.
Which of the following compounds are soluble in water? Which are insoluble?
a. CaCl2
b. N2
c. HBr
d. NH4C2H3O2
Write the formulas for the following hydrates.
a. Calcium sulfate dihydrate
b. Cobalt(II) chloride hexahydrate
Sunday, September 19, 2010
Boys Win SHC Debate Challenge
Monday, September 13, 2010
ep 6 Powerpoint review text only
Identify the following acids as monoprotic, di-protic, or triprotic. Explain your reasoning. H2CO3
What is true about the relative concentrations of hydrogen ions and hydroxide ions in each kind of solution?
basic
How many moles of HCl are required to neutralize aqueous solutions of these bases?
2 mol NH3
Write complete balanced equations for the following acid-base reactions?
H2SO4(aq) + KOH(aq) →
What substances are combined to make a buffer?
What is the molarity of sodium hydroxide if 10.0 mL of the solution is neutralized by each of the following 2.00M solutions?
56.0 mL of HCl
predict
Acidic solution?
Naming acids
Hydrochloric
HBr
Acid Nomenclature Flowchart
What is true about the relative concentrations of hydrogen ions and hydroxide ions in each kind of solution?
basic
How many moles of HCl are required to neutralize aqueous solutions of these bases?
2 mol NH3
Write complete balanced equations for the following acid-base reactions?
H2SO4(aq) + KOH(aq) →
What substances are combined to make a buffer?
What is the molarity of sodium hydroxide if 10.0 mL of the solution is neutralized by each of the following 2.00M solutions?
56.0 mL of HCl
predict
Acidic solution?
Naming acids
Hydrochloric
HBr
Acid Nomenclature Flowchart
EP 4 Review Powerpoint text only
How many valence electrons are in each atom?
Carbon
Know your Bonds
Ionic
Covalent
Polar covalent
Coordinate covalent
Network solid
Write the correct chemical formula for the compounds formed from each pair of ions.
K+,S2−
Write formulas for each compound.
barium chloride
VSEPR
Two bonding atoms, one lone pair
Properties of metals
Sea of electrons
formula
Write the formula for these binary compounds.beryllium chloride
Naming acids
Give the names of these acids. HNO2
Carbon
Know your Bonds
Ionic
Covalent
Polar covalent
Coordinate covalent
Network solid
Write the correct chemical formula for the compounds formed from each pair of ions.
K+,S2−
Write formulas for each compound.
barium chloride
VSEPR
Two bonding atoms, one lone pair
Properties of metals
Sea of electrons
formula
Write the formula for these binary compounds.beryllium chloride
Naming acids
Give the names of these acids. HNO2
Test Review ep 5 text only
Test Review EP 5 Sept 2010
Gary Sakuma
Like dissolves like
What is a polar molecule?
Water
Dissolves ionics, sugars, not lipids, methane, hydrocarbons
Formulae and percent
calcium chloride dihydrate
Percent by water
Solubility is affected by
Temperature
Pressure
size
Mole fraction problem
Calculate the mole fraction of each component in a solution of 1.50 mol ethanoic acid (CH3COOH) in 12.00 mol of water.
Colligative properties
What is the freezing point of a solution of 20.0 g of CCl4 dissolved in 500.0 g of benzene? The freezing point of benzene is 5.48°C; Kf is 5.12°C/m.
m/m problem
Calculate the grams of solute required to make the following solutions.
1100 g of saline solution (0.90% NaCl (m/m))
molarity
How many grams of NaCl would you need to make 500 ml of 3.0M
Concentration of Solute
The amount of solute in a solution is given by its concentration.
Molality
What is the molality of 5 moles of KCl in 500 ml of water
Two Other Concentration Units
V/V problems
What is the concentration (in % (v/v)) of the following solutions?
55 mL of ethanol (C2H5OH) is diluted to a volume of 250 mL with water.
Calculating Concentrations
Calculate molality
Boiling Point Elevation and Freezing Point Depression
∆T = K•m•i
i = van’t Hoff factor = number of particles produced per molecule/formula unit. For covalent compounds, i = 1. For ionic compounds, i = the number of ions present (both + and -)
Compound Theoretical Value of i
glycol 1
NaCl 2
CaCl2 3
Ca3(PO4)2 5
Boiling Point Elevation and Freezing Point Depression
∆T = K•m•i
Change in Boiling Point
Dissolve 62.1 g of glycol (1.00 mol) in 250. g of water. What is the boiling point of the solution?
Kb = 0.52 oC/molal for water (see Kb table).
Solution ∆TBP = Kb • m • i
1. Calculate solution molality = 4.00 m
2. ∆TBP = Kb • m • i
∆TBP = 0.52 oC/molal (4.00 molal) (1)
∆TBP = 2.08 oC
BP = 100 + 2.08 = 102.08 oC (water normally boils at 100)
Freezing Point Depression
Calculate the Freezing Point of a 4.00 molal glycol/water solution.
Kf = 1.86 oC/molal (See Kf table)
Solution
∆TFP = Kf • m • i
= (1.86 oC/molal)(4.00 m)(1)
∆TFP = 7.44
FP = 0 – 7.44 = -7.44 oC (because water normally freezes at 0)
Freezing Point Depression
At what temperature will a 5.4 molal solution of NaCl freeze?
Solution
∆TFP = Kf • m • i
∆TFP = (1.86 oC/molal) • 5.4 m • 2
∆TFP = 20.1 oC
FP = 0 – 20.1 = -20.1 oC
Solution Molality
How many grams of potassium iodide must be dissolved in 500.0 grams of water to produce a 0.060 molal KI solution
.5 kg H20 * .6 mole KI/1 kg H2O *
166.0 gKI/1 mol KI
= answer
Types of problems on exam
Ch 15 and 16 vocabulary and reading
Mass/Mass m/m
Volume/volume v/v
Hydrates percent water and writing formulae
Molarity
Molality
Freezing point depression/boiling point elevation T=k m I
Gary Sakuma
Like dissolves like
What is a polar molecule?
Water
Dissolves ionics, sugars, not lipids, methane, hydrocarbons
Formulae and percent
calcium chloride dihydrate
Percent by water
Solubility is affected by
Temperature
Pressure
size
Mole fraction problem
Calculate the mole fraction of each component in a solution of 1.50 mol ethanoic acid (CH3COOH) in 12.00 mol of water.
Colligative properties
What is the freezing point of a solution of 20.0 g of CCl4 dissolved in 500.0 g of benzene? The freezing point of benzene is 5.48°C; Kf is 5.12°C/m.
m/m problem
Calculate the grams of solute required to make the following solutions.
1100 g of saline solution (0.90% NaCl (m/m))
molarity
How many grams of NaCl would you need to make 500 ml of 3.0M
Concentration of Solute
The amount of solute in a solution is given by its concentration.
Molality
What is the molality of 5 moles of KCl in 500 ml of water
Two Other Concentration Units
V/V problems
What is the concentration (in % (v/v)) of the following solutions?
55 mL of ethanol (C2H5OH) is diluted to a volume of 250 mL with water.
Calculating Concentrations
Calculate molality
Boiling Point Elevation and Freezing Point Depression
∆T = K•m•i
i = van’t Hoff factor = number of particles produced per molecule/formula unit. For covalent compounds, i = 1. For ionic compounds, i = the number of ions present (both + and -)
Compound Theoretical Value of i
glycol 1
NaCl 2
CaCl2 3
Ca3(PO4)2 5
Boiling Point Elevation and Freezing Point Depression
∆T = K•m•i
Change in Boiling Point
Dissolve 62.1 g of glycol (1.00 mol) in 250. g of water. What is the boiling point of the solution?
Kb = 0.52 oC/molal for water (see Kb table).
Solution ∆TBP = Kb • m • i
1. Calculate solution molality = 4.00 m
2. ∆TBP = Kb • m • i
∆TBP = 0.52 oC/molal (4.00 molal) (1)
∆TBP = 2.08 oC
BP = 100 + 2.08 = 102.08 oC (water normally boils at 100)
Freezing Point Depression
Calculate the Freezing Point of a 4.00 molal glycol/water solution.
Kf = 1.86 oC/molal (See Kf table)
Solution
∆TFP = Kf • m • i
= (1.86 oC/molal)(4.00 m)(1)
∆TFP = 7.44
FP = 0 – 7.44 = -7.44 oC (because water normally freezes at 0)
Freezing Point Depression
At what temperature will a 5.4 molal solution of NaCl freeze?
Solution
∆TFP = Kf • m • i
∆TFP = (1.86 oC/molal) • 5.4 m • 2
∆TFP = 20.1 oC
FP = 0 – 20.1 = -20.1 oC
Solution Molality
How many grams of potassium iodide must be dissolved in 500.0 grams of water to produce a 0.060 molal KI solution
.5 kg H20 * .6 mole KI/1 kg H2O *
166.0 gKI/1 mol KI
= answer
Types of problems on exam
Ch 15 and 16 vocabulary and reading
Mass/Mass m/m
Volume/volume v/v
Hydrates percent water and writing formulae
Molarity
Molality
Freezing point depression/boiling point elevation T=k m I
Friday, September 10, 2010
photo highlights of ASDC2010
The ASDC2010 was a great journey for our students. Our first International competition, our students got to battle the various other schools from other countries.

The three boys were Tanachai ep 6/2, Chaya EP 6/1, and Kasidej EP4/2

ASDC 2010
Highlights of the tournament: The Boys beat TU in the final round. We finished 3-4, an outstanding first time at International Competition. Mr. Gary made the play-offs as an adjudicator judging up to the Semis in the tournament.

The three boys were Tanachai ep 6/2, Chaya EP 6/1, and Kasidej EP4/2

ASDC 2010
Highlights of the tournament: The Boys beat TU in the final round. We finished 3-4, an outstanding first time at International Competition. Mr. Gary made the play-offs as an adjudicator judging up to the Semis in the tournament.
Tuesday, September 7, 2010
Boys of AC Battle On in Asian Schools Debate Championships 2010
Young EP 4/2 Kasidej along with veterans EP 6/1 Chaya and EP 6/2 Tanachai face a large obstacle in the field of 11 countries with past Champions from Korea, World School players from Srilanka, last year's Champions from the Philippines, India, Malaysia, Indonesia, and others. It's been a great tournament so far with the boys standing at 2-3 going into the Final day.
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About Me
- Gary Hi10spro Sakuma
- I have played for 25 years and coached for the last 17 years--certified United States Professional Tennis Association Professional One--worked for Punahou Schools-voted the #1 Sports School in the United States, as a Program Supervisor, in charge of coaching the High Performance Players as well as coordinating programs for K-12 and Tennis Pro Education.