Question

A) If 350 mL of 0.90 M HNO3 is diluted to 450 mL, what is the...

A) If 350 mL of 0.90 M HNO3 is diluted to 450 mL, what is the molarity of the resulting solution?

B) How many milliliters of water must be added to 152 mL of 1.50 M HCl to give 1.00 M HCl? (Assume the volumes are additive.)

0 0
Add a comment Improve this question Transcribed image text
Answer #1

Final a- (450) Fina Va

Add a comment
Know the answer?
Add Answer to:
A) If 350 mL of 0.90 M HNO3 is diluted to 450 mL, what is the...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • How many milliliters of 10.5 M HCl(aq) are needed to prepare 740.0 mL of 1.00 M...

    How many milliliters of 10.5 M HCl(aq) are needed to prepare 740.0 mL of 1.00 M HCl(aq)? A 61.0 mL aliquot of a 1.20 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 113 mL of water. What is the final concentration? Assume the volumes are additive. concentration:

  • of 10 > A 37.0 mL aliquot of a 0.400 M stock solution must be diluted...

    of 10 > A 37.0 mL aliquot of a 0.400 M stock solution must be diluted to 0.100 M. Assuming the volumes are additive, how much water should be added? volume of water: volume of water:

  • 76.0 mL of a 1.50 M solution is diluted to a total volume of 248 mL....

    76.0 mL of a 1.50 M solution is diluted to a total volume of 248 mL. A 124-mL portion of that solution is diluted by adding 151 mL of water. What is the final concentration? Assume the volumes are additive. Number

  • 2. Calculate the molarity (M) of 30.0 g of NaOH in 350 mL of NaOH solution....

    2. Calculate the molarity (M) of 30.0 g of NaOH in 350 mL of NaOH solution. Show all the step by step work: 3. Calculate the amount of solute, in moles, grams or milliliters, needed to prepare the following solutions. Show all the step by step solution: a. 1.00 L of a 3.00 M NaCl solution (moles of solute) b. 2.00 L of a 1.50 M NaOH solution (grams of solute) c. Milliliters of 1.50 M NaCl solution to obtain...

  • A 75.0 mL aliquot of a 1.50 M solution is diluted to a total volume of...

    A 75.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 208 mL. A 104 mL portion of that solution is diluted by adding 185 mL of water. What is the final concentration? Assume the volumes are additive. concentration: M

  • A 70.0 mL aliquot of a 1.50 M solution is diluted to a total volume of...

    A 70.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 248 mL. A 124 mL portion of that solution is diluted by adding 117 mL of water. What is the final concentration? Assume the volumes are additive.

  • A 67.0 mL aliquot of a 0.400 M stock solution must be diluted to 0.100 M....

    A 67.0 mL aliquot of a 0.400 M stock solution must be diluted to 0.100 M. Assuming the volumes are additive, how much water should be added?

  • A 51.0 mL aliquot of a 1.50 M solution is diluted to a total volume of...

    A 51.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 288mL A 144mLportion of that solution is diluted by adding 175mL of water. What is the final concentration? Assume the volumes are additive.

  • In the laboratory, a student dilutes 11.0 mL of a 7.94 M hydrobromic acid solution to...

    In the laboratory, a student dilutes 11.0 mL of a 7.94 M hydrobromic acid solution to a total volume of 300.0 mL. What is the concentration of the diluted solution? How many milliliters of 9.56 M hydrochloric acid solution should be used to prepare 2.50 L of 0.500 M HCL? In the laboratory, a student adds 56.5 mL of water to 13.2 mL of a 0.875 M nitric acid solution. What is the concentration of the diluted solution? Assume the...

  • As a technician in a large pharmaceutical research firm, you need to produce 450. mL of...

    As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.93. The pKa of H2PO4− is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? (Assume additive volumes.) A beaker with 2.00×102 mLmL...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT