lakeland solutions review
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Lakeland Solutions Review. Click on a question to begin. Question 1. Try Again. Review the definition of Molarity. Try Again. Correct!. Molarity is the moles of solute per liter of solution. Next Question. Question 2. Try Again. - PowerPoint PPT PresentationTRANSCRIPT
Lakeland Solutions Review
Click on a question to begin1 6 11
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Molarity is defined as the
A) moles of solute per kilogram of solvent
B) moles of solute per liter of solution
C) mass of a solution D) volume of a solvent
Question 1
Try Again
Try Again
• Review the definition of Molarity
Correct!
• Molarity is the moles of solute per liter of solution
Next Question
Under which conditions of temperature andpressure is a gas most soluble in water?
A) high temperature and low pressure
B) low temperature and low pressure
C) high temperature and high pressure
D) low temperature and high pressure
Question 2
Try Again
Try Again
• Think about the best conditions to keep carbonation in pop
Correct!
• The best conditions are high pressure and low temperature. These produce a situation where the gas will be forced into the liquid
Next Question
What is the molarity of a solution of NaOH if2 liters of the solution contains 4 moles of NaOH?
A) 0.5 M B) 2.0 M
C) 8.0 M D) 80 M
Question 3
Try Again
Try Again
• Molarity is moles of solute per liter of solution
Correct!
• There are 4 moles of solute in 2 liters of solution. Molarity is moles divided by liters so 4/2 = 2 M
Next Question
A substance that conducts an electrical currentwhen dissolved in water is called
A) A catalyst B) A non-electrolyte
C) A metalloid D) An electrolyte
Question 4
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Try Again
• Review your solutions vocabulary
Correct!
• An electrolyte is a solution that can conduct electricity
Next Question
Compared to a 2.0 M aqueous solution of NaClat 1 atmosphere, a 3.0 M aqueous solution ofNaCl at 1 atmosphere has aA) Lower boiling point and higher
freezing pointB) Lower boiling point and lower freezing point
C) Higher boiling point and lower freezing point
D) Higher boiling point and higher freezing point
Question 5
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Try Again
• The addition of a solute changes the vapor pressure of a solution. The more solute dissolved, the greater the change in colligative properties.
Correct!
• The 3.0 M solution has more solute dissolved than the 2.0 M solution. This means that there will be a greater boiling point elevation and freezing point depression
Next Question
A 3.0 M HCl(aq) solution contains a total of
A) 3.0 grams of HCl per liter of solution
B) 3.0 grams of HCl per mole of solution
C) 3.0 moles of HCl per liter of solution
D) 3.0 moles of HCl per mole of solution
Question 6
Try Again
Try Again
• Review the definition of molarity
Correct!
• 3.0 M means that there are 3.0 moles per liter of solution
Next Question
What is the total number of grams of HI in0.500 liter of 1.00 M HI?
A) 1.00 g B) 64.0 g
C) 0.5 g D) 128.0 g
Question 7
Try Again
Try Again
• Use the molarity equation to solve for number of moles and then convert to grams
Correct!
• Molarity = moles/liters so 1.00 M = x/0.50 L. X = 0.500 mol. Convert 0.500 mol to grams of HI (mass = 128 g) to get 64 grams.
Next Question
Which 1-molal aqueous solution has the lowestfreezing point?
Question 8
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Try Again
• The lowest freezing point will have the lowest vapor pressure. The more ions present, the lower the vapor pressure.
Correct!
• The beaker contains the most ions which will reduce vapor pressure the most.
Next Question
What is the molarity of a solution that contains0.50 mole of NaOH in 0.50 liter of solution?
A) 1.00 M B) 0.25 M
C) 2.00 M D) 0.50 M
Question 9
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Try Again
• Remember that Molarity is moles per liter
Correct!
• 0.50 mol/0.50 liters is 1.00 M
Next Question
What is the total number of moles of solute in2.0 liters of 3.0 M NaOH?
A) 1.0 mole B) 2.0 mole
C) 3.0 mole D) 6.0 mole
Question 10
Try Again
Try Again
• Molarity equals moles of solute divided by liters of solution.
Correct!
• 3.0 M = x/2.0 L so x = (3.0)(2.0) = 6.0 mole
Next Question
Given the Ksp expression: Ksp = [A3+]2 [B2–]3
Which reaction is represented by the expression?
A) A2B3(s) 3A3+(aq) + 2B2–(aq) B) A2B3(s) 2A3+(aq) + 3B2–(aq)
C) A3B2(s) 3A3+(aq) + 2B2–(aq) D) A3B2(s) 2A3+(aq) + 3B2–(aq)
Question 11
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Try Again
• The exponents in the expression tell you how many of each ion are present in the compound
Correct!
• The exponents in the expression mean that there are 2 A and 3 B in the solid.
Next Question
As the pressure on a gas confined above a liquidincreases, the solubility of the gas in the liquid
A) increases B) decreases
C) Remains the same D) Not enough information
Question 12
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Try Again
• Think about what is the best way to keep carbonation in pop.
Correct!
• Increasing pressure increases the solubility of a gas in a liquid
Next Question
Which preparation produces a 2.0 M solution ofC6H12O6? [molecular mass = 180.0]
A) 90.0 g of C6H12O6 dissolved in 500.0 mL of solution
B) 90.0 g of C6H12O6 dissolved in 1000. mL of solution
C) 180.0 g of C6H12O6 dissolved in 500.0 mL of solution
D) 180.0 g of C6H12O6 dissolved in 1000. mL of solution
Question 13
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Try Again
• Convert the grams of sugar to moles and divide by the liters in order to determine molarity
Correct!
• 180 grams of C6H12O6 is equal to 1 mole. 1 mole divided by 0.5 L (500 mL) is 2.0 M.
Next Question
As a solute is added to a solvent, what happens to the freezing point and the boiling point of the solution?
A) The freezing point decreases and the boiling point decreases.
B) The freezing point increases and the boiling point increases.
C) The freezing point increases and the boiling point decreases.
D) The freezing point decreases and the boiling point increases.
Question 14
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Try Again
• The addition of a solute causes a change in vapor pressure resulting in boiling point elevation and freezing point depression
Correct!
• The addition of a solute causes the boiling point to go up and the freezing point to go down.
Next Question
A bottle of rubbing alcohol is labeled 70% v/v. If the bottle contains 591 mL, how much rubbing alcohol is in the bottle?
A) 591 mL B) 70 mL
C) 413.7 mL D) 177.3 mL
Question 15
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Try Again
• %v/v = volume of solute x 100 volume of solution
Correct!
• 70 = x x 100 x = 413.7 mL 591
Next Question