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Molarity Practice Problems, Level 1: Complete the problems below, show all work, submit to Schoology 1. What is the molarity of a solution prepared from 2.5 moles of solute dissolved in water with a final volume of 1500 mL? 2. What volume of a 0.75M solution would you need to pour out in order to have 0.050 moles of solute? 3. If your beaker contains 100 mL of a 0.50M solution, how many moles of solute do you have? 4. If you dissolve 0.35 moles of solute in water and your solution has a volume of 600 mL, what is the molarity of your solution? And, some molar mass questions: 5. How many moles are present in 250.0 grams of ammonium nitrate (NH4NO3)? 6. How many grams are present in a 2.6 moles sample of potassium bromide (KBr)?

          Molarity Practice Problems, Level 1: Complete the problems below, show all work, submit to Schoology
1. What is the molarity of a solution prepared from 2.5 moles of solute dissolved in water with a final volume of 1500 mL?
2. What volume of a 0.75M solution would you need to pour out in order to have 0.050 moles of solute?
3. If your beaker contains 100 mL of a 0.50M solution, how many moles of solute do you have?
4. If you dissolve 0.35 moles of solute in water and your solution has a volume of 600 mL, what is the molarity of your solution?
And, some molar mass questions:
5. How many moles are present in 250.0 grams of ammonium nitrate (NH4NO3)?
6. How many grams are present in a 2.6 moles sample of potassium bromide (KBr)?

Show more…

Molarity Practice Problems, Level 1: Complete the problems below, show all work, submit to Schoology
1. What is the molarity of a solution prepared from 2.5 moles of solute dissolved in water with a final volume of 1500 mL?
2. What volume of a 0.75M solution would you need to pour out in order to have 0.050 moles of solute?
3. If your beaker contains 100 mL of a 0.50M solution, how many moles of solute do you have?
4. If you dissolve 0.35 moles of solute in water and your solution has a volume of 600 mL, what is the molarity of your solution?
And, some molar mass questions:
5. How many moles are present in 250.0 grams of ammonium nitrate (NH4NO3)?
6. How many grams are present in a 2.6 moles sample of potassium bromide (KBr)?

Added by Edwin W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Supreeta N

05/13/2023

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Molarity Practice Problems, Level 1: Complete the problems below, show all work, submit to Schoology 1. What is the molarity of a solution prepared from 2.5 moles of solute dissolved in water with a final volume of 1500 mL? 2. What volume of a 0.75M solution would you need to pour out in order to have 0.050 moles of solute? 3. If your beaker contains 100 mL of a 0.50M solution, how many moles of solute do you have? 4. If you dissolve 0.35 moles of solute in water and your solution has a volume of 600 mL, what is the molarity of your solution? And, some molar mass questions: 5. How many moles are present in 250.0 grams of ammonium nitrate (NH4NO3)? 6. How many grams are present in a 2.6 moles sample of potassium bromide (KBr)?

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Transcript

00:01 Hello students, we have some questions on solutions.

00:03 In the first question we have been given that 2 .5 moles are present in a total volume of 1500 ml.

00:15 We have to calculate the molarity.

00:17 So, we know that molarity is equal to number of moles present in one liter of solution.

00:25 If the volume is given in then we will have to multiply it by 1000.

00:30 So, here molarity will be equal to number of moles divided by volume and we will multiply it by 1000.

00:39 So, molarity will be 1 .67 molar.

00:45 Now, let's move to the second question.

00:48 In second question we have given the molarity.

00:50 We have to calculate what volume of this solution will have this amount of moles.

00:55 So, molarity is moles per liter.

00:58 So, we can say that 0 .75 moles are present in one liter.

01:05 Therefore, 0 .05 moles will be present in 1 by 0 .75 multiplied by 0 .05 liters.

01:16 This will give us 0 .067 liters or we can say 67 milliliters.

01:23 This will be the correct answer.

01:25 Now, let's move to the third question.

01:28 In third question we have been given molarity of solution is 0 .05.

01:32 We have to calculate number of moles in 100 ml.

01:35 So, number of moles will be equal to concentration multiplied by volume in liters.

01:42 This is in milliliters.

01:44 We will divide it by 10 raised to the power 3.

01:46 So, this will give us number of moles.

01:49 So, number of moles will be 0 .005 moles.

01:56 This will be the correct answer...

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