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How can I dilute 50 percent dextrose to a 2.5 percent solution?
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Marcio Da Silva
How can I dilute 50 percent dextrose to a 2.5 percent solution?
Add 50% dextrose stock solution to water (or saline, see note below) using the formula M1V1 = M2V2, where M1=50%, M2=2.5%, V2=desired volume of 2.5% solution. Solve for V1 (volume of stock solution needed).
V1 = M2V2/M1 or V1 = 0.05V2 so for 1L of 2.5% use 50mL of 50% stock (just remember to remove 50mL from the 1L bag of normal saline first or your dilution will be incorrect).
NOTE: if this is for intravenous use, do NOT administer a 2.5% solution in sterile water, this solution is hypotonic and WILL cause blood cells to rupture. Using normal saline will make the solution hypertonic which will increase blood volume. While hypertonic solutions are generally safer, they still need to be administered with caution on a case-by-case basis. If you are uncertain or don’t have a good reason to administer a hypertonic solution, use a 5% dextrose solution in sterile water and administer by itself or in tandem with normal saline.
Add 50% dextrose stock solution to water (or saline, see note below) using the formula M1V1 = M2V2, where M1=50%, M2=2.5%, V2=desired volume of 2.5% solution. Solve for V1 (volume of stock solution needed).
V1 = M2V2/M1 or V1 = 0.05V2 so for 1L of 2.5% use 50mL of 50% stock (just remember to remove 50mL from the 1L bag of normal saline first or your dilution will be incorrect).
NOTE: if this is for intravenous use, do NOT administer a 2.5% solution in sterile water, this solution is hypotonic and WILL cause blood cells to rupture. Using normal saline will make the solution hypertonic which will increase blood volume. While hypertonic solutions are generally safer, they still need to be administered with caution on a case-by-case basis. If you are uncertain or don’t have a good reason to administer a hypertonic solution, use a 5% dextrose solution in sterile water and administer by itself or in tandem with normal saline.
What is the final volume of a 0.5 M of solution obtained diluting a 6M solution ofHCl? Its answer is 120 ml can anyone help in finding how is it possible?
So let me see if I understand. We’re starting with a 6 M solution and diluting it to a 0.5 M solution. And we want to know what the final volume will be. Do I have that right?
Did it occur to you that it matters what volume we start with?
The final concentration is 112" role="presentation">112 of the initial concentration, so the final volume will be 12× the original volume.
If the original volume is 10 mL, then the final volume will be 120 mL. But if the original volume is anything other than 10 mL, the final volume will be different, too.
What is the final volume of a 0.5 M of solution obtained diluting a 6M solution ofHCl? Its answer is 120 ml can anyone help in finding how is it possible?
So let me see if I understand. We’re starting with a 6 M solution and diluting it to a 0.5 M solution. And we want to know what the final volume will be. Do I have that right?
Did it occur to you that it matters what volume we start with?
The final concentration is 112" role="presentation">112 of the initial concentration, so the final volume will be 12× the original volume.
If the original volume is 10 mL, then the final volume will be 120 mL. But if the original volume is anything other than 10 mL, the final volume will be different, too.
Add 50% dextrose stock solution to water (or saline, see note below) using the formula M1V1 = M2V2, where M1=50%, M2=2.5%, V2=desired volume of 2.5% solution. Solve for V1 (volume of stock solution needed).
V1 = M2V2/M1 or V1 = 0.05V2 so for 1L of 2.5% use 50mL of 50% stock (just remember to remove 50mL from the 1L bag of normal saline first or your dilution will be incorrect).
NOTE: if this is for intravenous use, do NOT administer a 2.5% solution in sterile water, this solution is hypotonic and WILL cause blood cells to rupture. Using normal saline will make the solution hypertonic which will increase blood volume. While hypertonic solutions are generally safer, they still need to be administered with caution on a case-by-case basis. If you are uncertain or don’t have a good reason to administer a hypertonic solution, use a 5% dextrose solution in sterile water and administer by itself or in tandem with normal saline.
Add 50% dextrose stock solution to water (or saline, see note below) using the formula M1V1 = M2V2, where M1=50%, M2=2.5%, V2=desired volume of 2.5% solution. Solve for V1 (volume of stock solution needed).
V1 = M2V2/M1 or V1 = 0.05V2 so for 1L of 2.5% use 50mL of 50% stock (just remember to remove 50mL from the 1L bag of normal saline first or your dilution will be incorrect).
NOTE: if this is for intravenous use, do NOT administer a 2.5% solution in sterile water, this solution is hypotonic and WILL cause blood cells to rupture. Using normal saline will make the solution hypertonic which will increase blood volume. While hypertonic solutions are generally safer, they still need to be administered with caution on a case-by-case basis. If you are uncertain or don’t have a good reason to administer a hypertonic solution, use a 5% dextrose solution in sterile water and administer by itself or in tandem with normal saline.
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What is the final volume of a 0.5 M of solution obtained diluting a 6M solution ofHCl? Its answer is 120 ml can anyone help in finding how is it possible?
So let me see if I understand. We’re starting with a 6 M solution and diluting it to a 0.5 M solution. And we want to know what the final volume will be. Do I have that right?
Did it occur to you that it matters what volume we start with?
The final concentration is1 12 112 of the initial concentration, so the final volume will be 12× the original volume.
If the original volume is 10 mL, then the final volume will be 120 mL. But if the original volume is anything other than 10 mL, the final volume will be different, too.
What is the final volume of a 0.5 M of solution obtained diluting a 6M solution ofHCl? Its answer is 120 ml can anyone help in finding how is it possible?
So let me see if I understand. We’re starting with a 6 M solution and diluting it to a 0.5 M solution. And we want to know what the final volume will be. Do I have that right?
Did it occur to you that it matters what volume we start with?
The final concentration is1 12 112 of the initial concentration, so the final volume will be 12× the original volume.
If the original volume is 10 mL, then the final volume will be 120 mL. But if the original volume is anything other than 10 mL, the final volume will be different, too.
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