Explain how to make a 1 Normal solution H3PO4.
Technically, you can't make a solution with a known normality unless you know the reaction in which the H3PO4 will be used. Using the simple case,
normality = number equivalents/liter solution.
Therefore, one dissolves 1 equivalent (molar mass/3) grams in some water, add water to make a FINAL volume of 1,000 mL and that will be 1 N. You may not want 1 L of solution; therefore, half of that in 500 mL or 1/4 of that in 250 mL will be 1 N.
Well, if you want to make a 1 Normal solution of H3PO4, you're in for a real treat! Just follow these steps:
1. Find yourself a suitable container - make sure it's not too clownishly large or small. We don't want any acid spills or miniature explosions!
2. Get ready to do some math! A 1 Normal solution has a concentration of 1 mole of solute per liter of solution. So, if you're feeling adventurous, calculate the molecular weight of H3PO4 and convert it to grams.
3. Once you've got the hang of math, weigh out the calculated amount of H3PO4 and gently add it to a container. Avoid any clumsy spills – we wouldn't want your lab or kitchen looking like a circus!
4. Gradually add distilled water to the container while stirring. Keep stirring until the H3PO4 is fully dissolved. Remember, patience is key - no need to rush things.
5. Finally, adjust the volume to exactly 1 liter with more distilled water. Label your creation as a "1N H3PO4 Solution," especially if you plan to share it with others. Safety first, after all!
Remember, working with acids requires caution. Always wear safety goggles and protective gloves, and work in a well-ventilated area. If you're not confident in your chemistry skills, it's always a good idea to consult a professional. Stay safe, and happy experimenting!
To make a 1 Normal solution of H3PO4 (phosphoric acid), you will need to follow these steps:
Step 1: Determine the molecular weight of H3PO4
The molecular weight of H3PO4 is calculated by adding up the atomic masses of each element. In this case, hydrogen (H) has an atomic mass of approximately 1, phosphorus (P) has an atomic mass of approximately 31, and oxygen (O) has an atomic mass of approximately 16. Therefore, the molecular weight of H3PO4 is approximately 98 g/mol.
Step 2: Calculate the desired volume of the solution
To make a 1 Normal solution, the concentration is defined as one equivalent (gram equivalent weight) of solute per liter of solution. Since H3PO4 has three acidic protons, it can donate three equivalents per molecule. Therefore, to make a 1 Normal solution of H3PO4, you will need to dissolve approximately 98 grams of H3PO4 in enough water to make a final volume of 1 liter.
Step 3: Weigh the required amount of H3PO4
Using a digital balance or analytical balance, weigh out approximately 98 grams of H3PO4.
Step 4: Add the H3PO4 to a container
Transfer the weighed H3PO4 to a clean container, such as a beaker or flask.
Step 5: Add distilled water
Add distilled water to the container slowly while stirring until the total volume reaches 1 liter. Keep in mind that you may need more than 1 liter of water initially to dissolve the H3PO4, then adjust the final volume by adding water or more solution.
Step 6: Stir until complete dissolution
Continue stirring the solution until the solid H3PO4 has completely dissolved. This may take a few minutes.
Step 7: Label and store the solution
Once the H3PO4 is fully dissolved, label the container with the identity of the solution (1N H3PO4), the date it was prepared, and any other relevant information. Store the solution in a clean, labeled container with a tight-fitting cap. It is recommended to store the solution in a cool, dark place to extend its shelf life.
Please note that working with chemicals can be dangerous, and it is important to follow appropriate safety precautions, such as wearing gloves and goggles and working in a well-ventilated area. If you do not have the necessary equipment or expertise, it is recommended to seek assistance from a trained professional.
To make a 1 Normal solution of H3PO4 (phosphoric acid), you will need to calculate the amount of the compound needed to achieve the desired concentration. The term "Normal" refers to the number of equivalents of the solute compound in a liter of solution.
Here are the steps to prepare a 1 Normal solution of H3PO4:
1. Determine the molecular weight of H3PO4: Look up the atomic masses of hydrogen (H), phosphorus (P), and oxygen (O) in the periodic table. The molecular weight of H3PO4 is calculated by multiplying the atomic masses of each element by their respective subscript number, and then summing them up.
For H3PO4:
H = 1 atomic mass x 3 hydrogen atoms = 3 atomic mass
P = 31 atomic mass x 1 phosphorus atom = 31 atomic mass
O = 16 atomic mass x 4 oxygen atoms = 64 atomic mass
Molecular weight of H3PO4 = 3 + 31 + 64 = 98 g/mol
2. Calculate the number of moles of H3PO4 required: We want to prepare a 1 Normal solution, which means that for every liter of solution, there should be 1 mole of H3PO4. Since the molecular weight of H3PO4 is 98 g/mol, we need 98 grams of H3PO4 to make 1 mole of the compound.
3. Determine the volume of concentrated phosphoric acid needed: The concentration of the available phosphoric acid may vary, but for the purposes of this explanation, let's assume it is 85%.
The density of 85% H3PO4 is typically around 1.69 g/mL.
To calculate the volume needed, divide the desired mass of H3PO4 by the density:
Volume (mL) = Mass (g) / Density (g/mL).
For example, if you need 98 g of H3PO4:
Volume (mL) = 98 g / 1.69 g/mL ≈ 58 mL.
4. Dilute to the desired volume: Once you have measured the required volume of concentrated phosphoric acid (in this case, 58 mL), transfer it to a suitable container, such as a beaker or volumetric flask. Add distilled water to achieve the desired final volume, usually 1 liter.
Note: To ensure accuracy, it is recommended to use a volumetric flask rather than a beaker for dilution. Make sure to add the water slowly and mix well to ensure homogeneity.
And there you have it - a 1 Normal solution of H3PO4!