Chemistry Jeopardy

Molarity

100

What is Molarity?

Molarity = moles solute / L solution

200

How many moles are in 2.0 L of a 0.50 M NaCl solution?

1.0 mol

300

How many milliliters of 0.75 M HCl are needed to make 0.150 moles of HCl?

200 mL

400

100 mL of 4.3 M NaCl is diluted to 250 mL. What is the new concentration?

M₁V₁=M₂V₂

1.72 M

500

How many mL of 0.50 M HCl are required to completely react with 4.0 g of NaOH?
(Molar mass NaOH = 40.0 g/mol) 

HCl + NaOH → NaCl + H₂O

200 mL

Acids & Bases

100

Classify the following as acid, base, or neither:

a) HBr
b) NaOH
c) NaCl

HBr = Acid
NaOH = Base
NaCl = Neither (salt)

200

Which is the stronger acid?

a) HCl
b) CH₃COOH

HCl (strong acid)
CH₃COOH is weak.

300

Identify each as strong electrolyte, weak electrolyte, or non-electrolyte:

a) HNO₃
b) NH₃
c) C₆H₁₂O₆ (glucose)

HNO₃ = Strong electrolyte
NH₃ = Weak electrolyte
Glucose = Non-electrolyte

400

Which of the following are strong bases?

a) KOH
b) Ba(OH)₂
c) Al(OH)₃
d) NaOH

Strong bases: KOH, Ba(OH)₂, NaOH

500

Classify each substance as:

• Strong acid
• Weak acid
• Strong base
• Weak base
• Non-electrolyte

a) H₂SO₄
b) HF
c) LiOH
d) NH₃
e) C₂H₅OH (ethanol)

H₂SO₄ = Strong acid
HF = Weak acid
LiOH = Strong base
NH₃ = Weak base
Ethanol = Non-electrolyte

Precipitate

100

Will a precipitate form when NaCl(aq) and AgNO₃(aq) are mixed?

Yes, AgCl forms a precipitate.

200

Will a precipitate form when KNO₃(aq) and NaCl(aq) are mixed?

No,
All nitrates (NO₃⁻) are soluble.
All alkali metal salts (Na⁺, K⁺) are soluble.

300

When CaCl₂(aq) and Na₂CO₃(aq) are mixed, does a precipitate form?
If yes, name it.

Yes.
CaCO₃

400

Two solutions are mixed: BaCl₂(aq) and Na₂SO₄(aq).

• Will a precipitate form?

• What is it?

Yes, BaSO₄

500

Two aqueous solutions are mixed:

• Lead(II) nitrate
• Potassium iodide

1. Will a precipitate form?

2. Write the formula of the precipitate (Net ionic equation).

Yes, Pb²⁺ + 2I⁻ → PbI₂

Net Ionic Equations

100

What is a spectator ion?

An ion that appears unchanged on both sides of a reaction and cancels out in the net ionic equation.

200

Write the net ionic equation for:

NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

Na⁺ + Cl⁻ + Ag⁺ + NO₃⁻ → AgCl(s) + Na⁺ + NO₃⁻

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

300

Write the net ionic equation for:

CaCl₂(aq) + Na₂CO₃(aq) → CaCO₃(s) + 2NaCl(aq)

Ca²⁺ + 2Cl⁻ + 2Na⁺ + CO₃²⁻ → CaCO₃(s) + 2Na⁺ + 2Cl⁻

Ca²⁺(aq) + CO₃²⁻(aq) → CaCO₃(s)

400

Write the net ionic equation for:

BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2NaCl(aq)

Ba²⁺ + 2Cl⁻ + 2Na⁺ + SO₄²⁻ → BaSO₄(s) + 2Na⁺ + 2Cl⁻

Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)

500

Write the net ionic equation for:

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

H⁺ + Cl⁻ + Na⁺ + OH⁻ → Na⁺ + Cl⁻ + H₂O(l)

H⁺(aq) + OH⁻(aq) → H₂O(l)

Molarity 2.0

100

50.0 mL of 1.00 M HCl reacts with 40.0 mL of 1.00 M NaOH.

HCl + NaOH → NaCl + H₂O

Which reactant is limiting?

NaOH

200

75.0 mL of 0.80 M AgNO₃ reacts with 50.0 mL of 1.20 M NaCl.

AgNO₃ + NaCl → AgCl(s) + NaNO₃

How many moles of AgCl form?

0.060 mol AgCl

300

100.0 mL of 0.50 M H₂SO₄ reacts with 150.0 mL of 0.40 M NaOH.

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

Which reactant is limiting?

NaOH

400

200.0 mL of 0.60 M HCl reacts with 150.0 mL of 0.50 M Ca(OH)₂.

2HCl + Ca(OH)₂ → CaCl₂ + 2H₂O

1. Identify the limiting reactant.

2. How many grams of CaCl₂ form?

(Molar mass CaCl₂ = 111 g/mol)

HCl 

6.66 g CaCl₂  

500

125.0 mL of 0.90 M BaCl₂ reacts with 100.0 mL of 1.10 M Na₂SO₄.

BaCl₂ + Na₂SO₄ → BaSO₄(s) + 2NaCl

1. Identify the limiting reactant.

2. How many grams of BaSO₄ form?
   (Molar mass BaSO₄ = 233 g/mol)

Na₂SO₄ 

25.6 g BaSO₄