Solution Stoichiometry (Molarity)

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

AgNO₃ + HBr --> HNO₃ + AgBr

• 53.6

• 1.44

• 1.23

• 34.5

How many mL of 0.5M HNO₃ would be needed to react with 85mL of 0.75M KOH?

• 127.5mL

• 0.1275mL

• 31.9mL

• 0.031875mL

CaCO₃ + 2 HCl --> CaCl₂ + H₂O + CO₂

What volume (in mL) of 1.35 M HCl will be needed to completely react with 3.82 g of solid CaCO₃?

• 56.5 mL

• 47.2 mL

• 61.6 mL

• 34.7 mL

• 124 mL

FeS (s) + 2 HCl (aq) --> H₂S (g) + FeCl₂ (aq)

If 145 mL of HCl is needed to completely react with 25 g of iron (II) sulfide, what is the concentration of the HCl solution?

• 3.1 M

• 0.68 M

• 2.7 M

• 9.0M

• 3.9 M

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7

18.26 mL of a 1.50M hydrochloric acid reacts with excess magnesium hydroxide. Calculate the mass of magnesium hydroxide 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

How many milliliters of 2.4 M H₃PO₄ solution are needed to react with 45 g Zn?

2 H₃PO₄ + 3 Zn --> Zn₃(PO₄)₂ + 3 H₂

• 2400 mL

• 190 mL

• 290 mL

• 1700 mL

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

• 0.8 M

• 1.5 M

• 3.0 M

• 6.0 M

The concentration of a mixture can be increased in which of the following ways?

• Heating the mixture

• Adding more water “solvent”

• Adding more powder “solute”

• Stirring the mixture

Tags

NGSS.HS-PS1-5

How many grams of H₃PO₄ are in 175 mL of a 3.5 M solution of H₃PO₄?

• 60. grams

• 4.9 grams

• 612 grams

• 20 grams

How many moles would be in 85mL of 0.75M KOH?

• 113.3 mol

• 1.13 mol

• .113 mol

• 0.064 mol

• 63.75 mol

Tags

NGSS.HS-PS1-7