To prepare 1M H2SO4 solution, you would need to dilute concentrated sulfuric acid (approximately 18M) by adding the appropriate amount of water. To make 1L of 1M H2SO4 solution, you would mix approximately 55.5 mL of concentrated sulfuric acid with about 944.5 mL of water in a volumetric flask while taking proper safety precautions.
To completely neutralize 100ml of 1M H2SO4, you would need an equal number of moles of NaCl. H2SO4 is a diprotic acid, so it will require 2 moles of NaCl to neutralize 1 mole of H2SO4. Therefore, you would need 2 moles of NaCl for every mole of H2SO4. With a 1M solution of H2SO4 in 100ml, you have 0.1 moles of H2SO4. Therefore, you would need 0.2 moles of NaCl. The molar mass of NaCl is approximately 58.44g/mol, so you would need approximately 11.7 grams of NaCl to completely neutralize the 1M H2SO4 solution.
To completely neutralize 100 ml of 1M H2SO4, you would need an equal number of moles of NaCl. H2SO4 is a diprotic acid, so you need 2 moles of NaCl for each mole of H2SO4. Therefore, you would need 2 moles of NaCl, which is equal to 117 grams (2 x molar mass of NaCl) to neutralize 100 ml of 1M H2SO4.
To prepare 1N H2SO4 from 95% H2SO4, you would first need to dilute the 95% H2SO4 with water by adding the appropriate amount of water to achieve the desired concentration. To calculate the volume of 95% H2SO4 needed to make 1N solution, you need to use the formula: (Normality of stock solution) * (Volume of stock solution) = (Normality of diluted solution) * (Volume of diluted solution). Adjust the volumes accordingly to prepare the desired 1N solution.
To prepare a 0.25N solution of H2SO4, you would need to dilute concentrated sulfuric acid (typically around 95-98% purity) with water. For example, to prepare 1L of 0.25N H2SO4, you would mix 20.6mL of concentrated H2SO4 with approximately 980mL of water. Always add acid to water slowly and carefully while stirring to avoid splashing and heat generation.
If water is present in the volumetric flask when transferring the H2SO4 solution from the pipette, the final concentration of H2SO4 will be diluted. This is because the water will mix with the H2SO4 solution, increasing the total volume in the flask without adding more H2SO4 molecules. As a result, the concentration of H2SO4 will be lower than intended.
To completely neutralize 100ml of 1M H2SO4, you would need an equal number of moles of NaCl. H2SO4 is a diprotic acid, so it will require 2 moles of NaCl to neutralize 1 mole of H2SO4. Therefore, you would need 2 moles of NaCl for every mole of H2SO4. With a 1M solution of H2SO4 in 100ml, you have 0.1 moles of H2SO4. Therefore, you would need 0.2 moles of NaCl. The molar mass of NaCl is approximately 58.44g/mol, so you would need approximately 11.7 grams of NaCl to completely neutralize the 1M H2SO4 solution.
To completely neutralize 100 ml of 1M H2SO4, you would need an equal number of moles of NaCl. H2SO4 is a diprotic acid, so you need 2 moles of NaCl for each mole of H2SO4. Therefore, you would need 2 moles of NaCl, which is equal to 117 grams (2 x molar mass of NaCl) to neutralize 100 ml of 1M H2SO4.
You could titrate equal volumes of 1M solution of NaOH and 1M solution of HCl to obtain 1M solution of NaCl.
To prepare 1N H2SO4 from 95% H2SO4, you would first need to dilute the 95% H2SO4 with water by adding the appropriate amount of water to achieve the desired concentration. To calculate the volume of 95% H2SO4 needed to make 1N solution, you need to use the formula: (Normality of stock solution) * (Volume of stock solution) = (Normality of diluted solution) * (Volume of diluted solution). Adjust the volumes accordingly to prepare the desired 1N solution.
You need 252 g sulfuric acid.
Mix 120 g sulfuric acid with water to 1000 mL.
To prepare a 0.25N solution of H2SO4, you would need to dilute concentrated sulfuric acid (typically around 95-98% purity) with water. For example, to prepare 1L of 0.25N H2SO4, you would mix 20.6mL of concentrated H2SO4 with approximately 980mL of water. Always add acid to water slowly and carefully while stirring to avoid splashing and heat generation.
If water is present in the volumetric flask when transferring the H2SO4 solution from the pipette, the final concentration of H2SO4 will be diluted. This is because the water will mix with the H2SO4 solution, increasing the total volume in the flask without adding more H2SO4 molecules. As a result, the concentration of H2SO4 will be lower than intended.
how 2.5N H2SO4 prepared from concentrated H2SO4
Remember M1V1=M2V2, where M is molarity and V is volume. M1/M2=V2/V1, 10/1=v2/v1, For diluting the acid, we can add acid to water. So, assuming that 10M H2SO4 is having 1ml of water, we should add 1M of H2So4 to 10ml of water.
To prepare 1M Tris-HCl from a 10mM solution, you would need to dilute the 10mM solution by a factor of 100. This means you would mix 1 part of the 10mM solution with 99 parts of water to achieve a final concentration of 1M Tris-HCl.
To prepare 1M sulfuric acid (H2SO4), you would need to dilute concentrated sulfuric acid with water carefully while stirring. Do this by adding the concentrated acid slowly to water, never the other way around, to prevent violent splattering. Always handle concentrated sulfuric acid with extreme caution, as it is highly corrosive.