Molarity and Solution Stoichiometry

What mass of AgBr is formed when 35.5 mL of 0.184 M AgNO₃ is treated with an excess (extra) of aqueous hydrobromic acid?

• 53.6 g of AgBr

• 1.44 g of AgBr

• 1.23 g of AgBr

• 34.5 g of AgBr

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

18.26 mL of a 1.50M HCl reacts with excess (extra) Mg(OH)₂. Calculate the mass of Mg(OH)₂ needed for the reaction.

Mg(OH)₂ + 2 HCl -> 2 H₂O + MgCl₂

• 4.68 g Mg(OH)₂

• 0.798 g Mg(OH)₂

• 0.0274 Mg(OH)₂

• 1.07 g Mg(OH)₂

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of NaOH?

Molarity = moles / liters

• 0.8 M

• 1.5 M

• 3.0 M

• 6.0 M

True or False. You must convert grams to moles to do stoichiometry.

• True

• False

Tags

NGSS.HS-PS1-7

If you are going to solve a molar ratio problem, how do you set it up?

a

b

c

d

Given Moles A

Moles B

Calculated Moles B

Moles A

Tags

NGSS.HS-PS1-7

Locate the following on the example stoichiometry calculation.

a

b

c

d

mole to gram ratio for Al

mole to gram ratio for AlCl3

what was given to start

mole to mole ratio

Tags

NGSS.HS-PS1-7

What is the molarity of a solution that contains 5 moles of solute in 2 liters of solution?

• 2.5 M

• 5 M

• 10 M

• 0.4 M

Where is the mole to gram ratio for Al in this set up? (pick one)

Tags

NGSS.HS-PS1-7

Where is the mole to mole ratio in this set up? (pick one)

Tags

NGSS.HS-PS1-7

Where is the mole to gram ratio for AlCl3 in this set up? (pick one)

Tags

NGSS.HS-PS1-7