Chapter 14b Standard Solutions & Indicators

Which of the following is NOT a property of primary standards?

• They are stable (do not react with gases and water).

• They are white, crystalline powders.

• They are pure (which means that the molar mass used in calculations is valid).

• They are inexpensive.

How many mL of 10.8 M HCl are required to make 100.0 mL of 3.00 M acid?
(c₁V₁ = c₂V₂)

Hint: remember to use the correct number of significant figures.

• 27.8 mL
• 27.78 mL
• 2.8 mL
• 278 mL

What would the molarity of a solution be if you took 10 mL of a 13 M stock solution and made a 300 mL solution?

• 390M

• 230M

• 0.43M

• 0.26M

What volume of water must be added to 10 mL of 2.5 M H₂SO₄ solution to create a diluted solution with a concentration of 1 M.

• 25 mL

• 15 mL

• 10 mL

• 5 mL

Tags

NGSS.HS-PS1-7

Dilution of concentrated solutions is performed frequently in laboratories to make experiments safer and more practical.

• True

• False

Tags

NGSS.HS-PS1-5

The mass of sodium carbonate (Na₂CO₃) required to create a 0.25 M solution with a volume of 250 mL is

• 0.25 g

• 26.5 g

• 6.625 g

• 0.0625 g

Tags

NGSS.HS-PS1-5

The equivalence point is when acids and bases are added in the correct mole ratios.

• True

• False

All indicators will produce an end point close to the equivalence point for all combinations of acid/base titrations.

• True

• False

An appropriate indicator to use when the equivalence point for a titration is 3.5 is

• phenolphthalein.

• methyl red.

• methyl orange.

• bromothymol blue

An appropriate indicator to use when the equivalence point for a titration is 9 is

• phenolphthalein.

• methyl red.

• methyl orange.

• bromothymol blue