Question

Type your answers in all of the blanks and submit If 56 mL of a 1.20 M stock solution is dissolved in enough water to bring the total volume to 288 mL the new Molarity is 0.233 M If you now take 144mL of the stock solution and dilute it by adding 159 mL of water, what is the final concentration? 0.26 M

          Type your answers in all of the blanks and submit
If 56 mL of a 1.20 M stock solution is dissolved in enough water to bring the total volume to 288 mL the new Molarity is 0.233 M
If you now take 144mL of the stock solution and dilute it by adding 159 mL of water, what is the final concentration? 0.26 M

Type your answers in all of the blanks and submit
If 56 mL of a 1.20 M stock solution is dissolved in enough water to bring the total volume to 288 mL the new Molarity is 0.233 M
If you now take 144mL of the stock solution and dilute it by adding 159 mL of water, what is the final concentration? 0.26 M

Added by Eugenia S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ma Ednelyn Lim

08/31/2023

Step 1

We can use the formula: moles = Molarity × Volume moles = 1.20 M × 0.144 L = 0.1728 moles Now, we need to find the total volume of the solution after adding 159 mL of water. The total volume is: Total volume = 144 mL + 159 mL = 303 mL = 0.303 L Show more…

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If 56 mL of a 1.20 M stock solution is dissolved in enough water to bring the total volume to 288 mL, the new molarity is 0.233. If you now take 144 mL of the stock solution and dilute it by adding 159 mL of water, what is the final concentration? 0.26.