Dilutions Worksheet 1

Which of these solutions is more concentrated?

• A

• B

Tags

NGSS.HS-PS1-5

• Which of these solutions is more dilute?

• A

• B

What is the molarity of a solution of NH₄Cl prepared by diluting 0.5 L of a 3.79 M NH₄Cl solution to 2.00 L?

• 7.58 M

• 0.26 M

• 2.66 M

• 0.9475 M

• A 2.0 L, 3.8 M solution of FeSO₄ has 7.0 L of water poured into it.  What is the molarity of the new diluted solution? (Hint:  Read the volume info very carefully!)

• 1.08 M

• 0.84 M

• 0.53 M

• 13.3 M

Tags

NGSS.HS-PS1-7

If I add water to 100 mL of a 0.35 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?

• 0.14 M

• 0.28 M

• 0.52 M

• 0.23 M

How much water would I need to add to 500 mL of a 4.4 M KCl solution to make a 1.0 M solution?

hint: remember to find the difference after running your calculation

• 1,200 mL

• 1,700 mL

• 2,200 mL

• 1,500 mL

85.0 mL of a solution of NaOH is diluted to a final volume of 270.0 mL and the new molarity is 0.500 M. Calculate the original molarity of the base.

• 1.59 M

• 42.5 M

• 0.157 M

• 4.25 M

Tags

NGSS.HS-PS1-7

220.0 mL of a solution of NaOH is diluted by adding 250.0 mL of water to produce a new molarity of 0.15 M. Calculate the molarity of the base.

• 0.17 M

• 0.28 M

• 0.71 M

• 0.32 M

A 0.350 M solution is concentrated by evaporation to a reduced final volume of  100.0 mL and a molarity of 0.925 M. Calculate the original volume.

• 37.83 mL

• 264.3 mL

• 373.8 mL

• 62.4 mL

What is the molarity of a solution of NH₄Cl prepared by diluting 500.00 mL of a 3.79 M NH₄Cl solution to 2.00 L? hint: volume 1 and volume 2 units must match

• 0.95 M

• 1.895 M

• 1.516 M

• 0.29 M