Chemistry Jeopardy SINGLE JEOPARDY

Solutions Electrolytes Equilibrium Molarity Acid-Base 100 100 100 100 100 200 200 200 200 200 300 300 300 300 300 400 400 400 400 400 500 500 500 500 500

A solution must consist of a solute and ? Question A-1 A solution must consist of a solute and ?

Answer Solvent.

Question A-2 If a substance was insoluble, could you make a solution with it? EXPLAIN.

No, it could not be a solute if it can not dissolve. Answer No, it could not be a solute if it can not dissolve.

Ex.) Pure substance, ionic compound, etc… Question A-3 Properly classify a solution in terms of the classification of matter? Ex.) Pure substance, ionic compound, etc…

Would be a homogenous mixture. Answer Would be a homogenous mixture.

What is the mathematical expression for concentration? Question A-4 What is the mathematical expression for concentration?

Answer M=moles of solute/total volume of solution. (M=moles/Liters is acceptible)

Question A-5 What is the difference between a stock solution and a diluted solution?

Answer A stock solution is more concentrated, has more solute, less solvent than a diluted solution.

What kind of electrolyte is NaCl, strong, weak or non? Question B-1 What kind of electrolyte is NaCl, strong, weak or non?

Answer Strong

What would NaCl(s) look like dissociated? Question B-2 What would NaCl(s) look like dissociated?

Answer Na+ and Cl-

What are the 7 molecules that full disociate? Question B-3 What are the 7 molecules that full disociate?

HCl HBr HI HNO3 H2SO4 HClO4 HClO3 Answer HCl HBr HI HNO3 H2SO4 HClO4 HClO3

Question B-4 What kind of electrolyte would have ionized and non ionized particles in solution?

Answer Weak

Question B-5 Arrange the following from most conductive to least conductive: HCl, H2SO4, Li3N, C2H6, HC2H3O2

Answer Li3N H2SO4 HCl HC2H3O2 C2H6

What kind of arrow is used in an equilibrium chemical equation? Question C-1 What kind of arrow is used in an equilibrium chemical equation?

Answer Double sided 

CaCO3(s) CaO(s)+ CO2(g) Question C-2 What would the equilibrium constant expression be for the following reaction? CaCO3(s) CaO(s)+ CO2(g)

Answer k= [CO2]

Use the following equation to answer the question. Question C-3 Use the following equation to answer the question. N2(g) + 3H2(g)  2NH3(g) If hydrogen was added, what way would the equilibrium shift?

Answer Shift right or forward

Use the following equation to answer the question. Question C-4 Use the following equation to answer the question. N2(g) + 3H2(g)  2NH3(g) If the volume of the container decreased, which way would the equilibrium shift?

Answer Shift right or forward

Use the following equation to answer the question. Question C-5 Use the following equation to answer the question. N2(g) + 3H2(g)  2NH3(g) If argon gas was added to the system in a rigid container, what way would the equilibrium shift?

Answer It wouldn’t. The addition of Ar gas wouldn’t affect the concentrations of the species in the reaciton.

What is the molarity of a solution that has 2 moles in 2.0L? Question D-1 What is the molarity of a solution that has 2 moles in 2.0L?

Answer 1.0M

Question D-2 What would the molarity be of a solution that was created with 55.5g of calcium chloride in 500.0mL of water

Answer 1.0M

How many moles of HCl would exist in 600.0mL of a 3.0M solution? Question D-3 How many moles of HCl would exist in 600.0mL of a 3.0M solution?

Answer 1.8 moles

Question D-4 How many liters would a sample containing 0.75 moles and having a concentration of 2.0M be?

Answer 0.375L

Question D-5 Calculate how many mL of an 16.0M stock solution you would need to create 200.0mL of a 0.6M dilution?

Answer 7.5mL

What element does every acid have to have? Question E-1 What element does every acid have to have?

Answer Hydrogen

What is the conjugate base of nitric acid? Question E-2 What is the conjugate base of nitric acid?

Answer NO3-

In the following reaction is water acting as an acid or base? Question E-3 In the following reaction is water acting as an acid or base? NH3 + H2O  NH4+ + OH-

Answer Acid

Question E-4 Why is it that every bronsted lowry base can not be considered an arrhenius base?

Answer A substance that can accept an H+ does not always have to ionize to produce OH- ions.

Question E-5 One sample containing 200.0mL of a 0.6M HCl solution was mixed with another sample containing 250.0mL of a 0.45M solution. After the acid-base reaction was complete what would the [H+] and [OH-] be?.

Answer [H+]=0.0167 [OH-]=0