Molarity and Solution Stoichiometry

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

• 60
• 4.9
• 612
• 20

How many moles of BaCl₂ are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

• 1.15
• 0.0672
• 0.0336
• 2.30

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

• 53.6
• 1.44
• 1.23
• 34.5

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

• 113.3 mol

• 1.13 mol

• .113mol

• 0.06375mol

• 63.75mol

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

• 113.3 mol

• 1.13 mol

• .113mol

• 0.06375mol

• 63.75mol

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

Tags

NGSS.HS-PS1-7

How many grams of water could form in this reaction 85mL of 0.75M KOH?

• 1.15g

• 282g

• 31.9g

• 113.g

Tags

NGSS.HS-PS1-7

What would the molarity of the solution be if 0.475 mol of KNO₃ were formed in this reaction and the final volume of the solution was 595mL

• 0.798M

• 1.25M

• 282.6M

• 7.98x10^-4M

Tags

NGSS.HS-PS1-7

Molarity is:

• moles per liter of solution

• written with a unit of M

• calculated by dividing the moles of a substance by the liters of solvent

• all of the above

To convert liters of a solution to moles, one should:

• divide by the molarity

• multiply by the molarity

• multiply by the molar mass

• divide by the molar mass then multiply by the speed of light squared