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6. The first part of the lab is to standardize your NaOH. The buret you will use can dispense a maximum of 50.00 mL. Approximately how much KHP should you weigh out for the standardization? To determine this, consider: * In order to have as many significant figures as possible, you want at least 0.1 g of KHP. It is easier to weigh out larger masses. * Similarly, to have as many significant figures as possible, you want to dispense at least 10.00 mL of NaOH to neutralize the KHP * It is wasteful, and will also take a long time, if you need to dispense a large volume of NaOH to neutralize the KHP, so you want to use less than half the buret's volume. * It is important to leave some margin for error when designing protocols. You only know the approximate concentration of NaOH, it could be slightly less or more than 0.1 M With these considerations in mind, choose a reasonable volume of NaOH and calculate what mass of KHP (204.22 g/mol) will neutralize that volume of NaOH. (In lab, you should dispense NaOH quickly to approximately 5 mL less than that volume, and then proceed slowly from there to the endpoint.)

          6. The first part of the lab is to standardize your NaOH. The buret you will use can dispense a maximum of 50.00 mL. Approximately how much KHP should you weigh out for the standardization? To determine this, consider:

* In order to have as many significant figures as possible, you want at least 0.1 g of KHP. It is easier to weigh out larger masses.

* Similarly, to have as many significant figures as possible, you want to dispense at least 10.00 mL of NaOH to neutralize the KHP

* It is wasteful, and will also take a long time, if you need to dispense a large volume of NaOH to neutralize the KHP, so you want to use less than half the buret's volume.

* It is important to leave some margin for error when designing protocols. You only know the approximate concentration of NaOH, it could be slightly less or more than 0.1 M

With these considerations in mind, choose a reasonable volume of NaOH and calculate what mass of KHP (204.22 g/mol) will neutralize that volume of NaOH. (In lab, you should dispense NaOH quickly to approximately 5 mL less than that volume, and then proceed slowly from there to the endpoint.)

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6. The first part of the lab is to standardize your NaOH. The buret you will use can dispense a maximum of 50.00 mL. Approximately how much KHP should you weigh out for the standardization? To determine this, consider:

* In order to have as many significant figures as possible, you want at least 0.1 g of KHP. It is easier to weigh out larger masses.

* Similarly, to have as many significant figures as possible, you want to dispense at least 10.00 mL of NaOH to neutralize the KHP

* It is wasteful, and will also take a long time, if you need to dispense a large volume of NaOH to neutralize the KHP, so you want to use less than half the buret's volume.

* It is important to leave some margin for error when designing protocols. You only know the approximate concentration of NaOH, it could be slightly less or more than 0.1 M

With these considerations in mind, choose a reasonable volume of NaOH and calculate what mass of KHP (204.22 g/mol) will neutralize that volume of NaOH. (In lab, you should dispense NaOH quickly to approximately 5 mL less than that volume, and then proceed slowly from there to the endpoint.)

Added by David H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Sri K

05/14/2022

Step 1

Since 1 mole of KHP reacts with 1 mole of NaOH, and the concentration of NaOH is 0.1 M, we can use the formula: \[ \text{Volume of NaOH (L)} = \frac{\text{Moles of KHP}}{\text{Concentration of NaOH (M)}} \] Given that we need at least 0.1 g of KHP, which is Show more…

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The first part of the lab is to standardize your NaOH. The buret you will use can dispense a maximum of 50.00 mL. Approximately how much KHP should you weigh out for the standardization? To determine this, consider: In order to have as many significant figures as possible, you want at least 0.1 g of KHP. It is easier to weigh out larger masses. Similarly, to have as many significant figures as possible, you want to dispense at least 10.00 mL of NaOH to neutralize the KHP. It is wasteful, and will also take a long time, if you need to dispense a large volume of NaOH to neutralize the KHP, so you want to use less than half the buret's volume. It is important to leave some margin for error when designing protocols. You only know the approximate concentration of NaOH; it could be slightly less or more than 0.1 M. With these considerations in mind, choose a reasonable volume of NaOH and calculate what mass of KHP (204.22 g/mol) will neutralize that volume of NaOH. (In the lab, you should dispense NaOH quickly to approximately 5 mL less than that volume, and then proceed slowly from there to the endpoint.)

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Transcript

00:01 You high students let me explain you the question here so in in this particular question we have to standardize a solution of nah oh h this solution of nahoh is having the concentration 0 .2 molar here we are using the primary standard is potassium hydrogen thalate so it having the molar must do 0 .2 gram per mole so here here we have to determine the mass of potassium hydrogen pallet, it utilized 20 ml, naoh titrant.

00:40 So this is the question.

00:42 These are the, so this is the table.

00:45 So this particular table, it is standardization.

00:49 So during the standardization of 0 .2 molar naoh titrent.

00:54 Then this is the standardization of 0 .2 molar titterent.

01:00 So this table it is standardization of 0 .2 molar titrate that is using calorimetric indicator.

01:14 So here coming to the solution, so here the reaction.

01:23 So this is the potassium hydrogen thallate.

01:28 So potassium hydrogen c .o .o.

01:33 N .a.

01:34 And o minus.

01:38 A plus plus water this is the reaction so here the concentration of n aoha concentration of n a o h point two molar volume so volume of n a o h it is utilized that is 20 m l and milly moles of n a oh h so how to find milly modes of n a o h that is molarity into volume volume we have to take in m l so that is molarity 0 .2 molar into 20 so that is equal to that is equal to 4 millimoles 4 millie moles to be utilized to be utilized so from the reaction so that is milly moles of milly moles reacted n .a.

02:32 Ohh that is equal to milly moles of ahp required potassium hydrogen thallate required so that is an millimoles of khp so millimoles of khp that is equal to 4 millimoles of milly moles of khp because we know that millimoles of a reactor de novoh it is 4 millimoles even millimals of khp it is equal to 4 millimoles that means uh moles of khp that is equal to 4 into 10 to power of minus 3 moles so molar mass of hb, so molar mass of hb, that is 204 .2 gram per molar...

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