Question

In today’s experiment you will need to make 15 mL of a 3.0 M HCl solution....

In today’s experiment you will need to make 15 mL of a 3.0 M HCl solution. You will be diluting from a stock solution of 4.5 M HCl. Use your dilution calculation (M1V1 = M2V2) to determine how much of the original stock solution you will need.  How much water will you be adding to the acidic solution?

Homework Answers

Answer #1

We will use equation,

M1 V1 = M2 V2

where,  

M1 = Initial molarity = 4.5 M

V1 = Initial volume = to be calculated.

M2 = Final molarity = 3 M

V2 = Final volyme = 15 mL

Putting this in above equation we get,

4.5 M x V1 = 3 M x 15 mL

4.5 M x V1 = 45 M/mL

therefore,

V1 = 45 M/mL / 4.5 = 10 mL

Therefore we must diluted 10 mL 4.5 M HCl solution to make 3 M 15 mL HCl solution. Total volume is 15 mL therefore additional 5 mL water will be added

Ans = 10 mL stck solution

5 mL water.

Know the answer?
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
Similar Questions
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 6.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you: 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
You have 375 mL of a 1.25 M potassium chloride solution, but you need to make...
You have 375 mL of a 1.25 M potassium chloride solution, but you need to make a 0.50 M potassium chloride solution. How many milliliters of water must you add to the original 1.25 M solution to make the 0.50 M potassium chloride solution? Note: Assume the volumes are additive. Anwer should be in mL of water.
1) How many moles of acid are there in 17 ml of a 7.1 M HCl...
1) How many moles of acid are there in 17 ml of a 7.1 M HCl solution? 2) 18 ml of a 1.0 M HCl solution was added to a flask and titrated against a solution of 3.8 M NaOH. How many ml of the NaOH solution was required to neutralize the acid? 3) What volume (in liters) of a 2.8 M NaOH solution would neutralize 4.8 moles of H2SO4 (diprotic)? 4) Using the formula M1V1 = M2V2, calculate the...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 7.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you 100 mL of 7.00×10−2M HCl , 100 mL of 5.00×10−2M NaOH , and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH . Once you realize...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 7.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...
You need to make an aqueous solution of 0.162 M iron(II) sulfate for an experiment in...
You need to make an aqueous solution of 0.162 M iron(II) sulfate for an experiment in lab, using a 250 mL volumetric flask. How much solid iron(II) sulfate should you add? ___ grams How many milliliters of an aqueous solution of 0.207 M copper(II) acetate is needed to obtain 7.15 grams of the salt? ____mL In the laboratory you dissolve 24.2 g of lead nitrate in a volumetric flask and add water to a total volume of 125 . mL....
A student has 100. mL of 0.20 M HCl solution. She takes 5.0 mL of this...
A student has 100. mL of 0.20 M HCl solution. She takes 5.0 mL of this solution, and adds it to 10.0 mL of water. She then takes 3.0 mL of this new solution for an experiment. What is the concentration of this solution?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT