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What volume of a 2.5M stock solution of acetic acid is required to prepare 100.0 milliliters of a 0.50M acetic acid solution?
Wiki User
∙ 11y ago
The answer is 20,15 mL.
Wiki User
∙ 11y ago
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What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare?
This depends on your experiment.
What volume of a 2.5 M stock solution of acetic acid is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
To determine the volume of the 2.5 M stock solution needed, you can use the dilution formula: M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. Rearrange the formula to solve for V1, which is the volume of the stock solution you need to prepare 100.0 milliliters of a 0.50 M solution. Substituting the values gives: V1 = (0.50 M * 100.0 mL) / 2.5 M = 20.0 milliliters. Therefore, you need 20.0 milliliters of the 2.5 M stock solution to prepare 100.0 milliliters of the 0.50 M solution.
How do you prepare 3 l of buffer?
Take 333 milliliters of your stock solution and dilute it to 1L with water.
How you are going to prepare a solutin containing 3 percent acetic acid and 97 percent water?
To prepare a solution containing 3% acetic acid and 97% water, you can add the required amount of acetic acid to the water based on the desired volume of the final solution. For example, to make 100mL of this solution, you would add 3mL of acetic acid to 97mL of water. Make sure to mix thoroughly to ensure homogeneity of the solution.
How do you prepare a solution that is 5000 PPM acetic acid?
add 2.4ml glacial aetic acid in one liter of d.m water
What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare?
This depends on your experiment.
What volume of a 2.5 M stock solution of acetic acid is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
To determine the volume of the 2.5 M stock solution needed, you can use the dilution formula: M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. Rearrange the formula to solve for V1, which is the volume of the stock solution you need to prepare 100.0 milliliters of a 0.50 M solution. Substituting the values gives: V1 = (0.50 M * 100.0 mL) / 2.5 M = 20.0 milliliters. Therefore, you need 20.0 milliliters of the 2.5 M stock solution to prepare 100.0 milliliters of the 0.50 M solution.
How do you prepare 3 l of buffer?
Take 333 milliliters of your stock solution and dilute it to 1L with water.
how to prepare 0.1 N Glacial acetic acid solution?
To prepare a 0.1 N glacial acetic acid solution, calculate the required mass by multiplying 0.1 moles by the molar mass of glacial acetic acid (60.05 g/mol). Weigh out the calculated mass and add it to a clean container. Dissolve the glacial acetic acid completely by stirring it with distilled water. Transfer the solution to a 1-liter volumetric flask and dilute it to the 1-liter mark with distilled water. Mix thoroughly, label, and store the solution properly, taking necessary safety precautions when handling glacial acetic acid.
20 ml of acetic acid ch3cooh is titrated with a solution of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
Using the balanced equation, CH3COOH + NaOH -> CH3COONa + H2O, we know that one mole of acetic acid reacts with one mole of NaOH at the equivalence point. Since 35 ml of 0.15 M NaOH are required to reach the equivalence point, this is equal to 35 ml * 0.15 mol/L = 5.25 mmol of NaOH. As the reaction is 1:1, the amount of acetic acid is also 5.25 mmol. Therefore, the concentration of the acetic acid solution is 5.25 mmol / 20 ml = 0.2625 mol/L.
20 ml of acetic acid is titrated with a solution of 0.15 M NaOH If 35 ml of NaOH are required to reach the equivalence point what is the concentration of the acetic acid solution?
The moles of NaOH at the equivalence point will equal the moles of acetic acid present in the solution. Therefore, using the volume and concentration of NaOH used at the equivalence point, you can calculate the moles of NaOH used. Then, based on the stoichiometry of the reaction, you can determine the moles of acetic acid, and finally, determine the concentration of the acetic acid solution.
How can we prepare .1N wij's solution from iodine monochloride?
Dissolve 16.235 g of ICl into 1000 ml solution with glacial acetic acid. The solution will be 0.1N Wij's Solution. However weighing is a very difficult task you need to have the required skill and sound analytical knowledge and detailed MSDS of ICl. Man Katuwal
How do you prepare wijs solution?
Iodine monochloride is soluble in alcohol, ether, acetic acid. ICl is prepared from iodine and chlorine.
30 ml of hydrofluoric acid hf is titrated with a solution of 0.10 m koh if 55 ml of koh is required to reach the equivalence point what is the concentration of the acetic acid solution?
Since hydrofluoric acid (HF) and KOH react in a 1:1 ratio, the number of moles of KOH is equal to the number of moles of HF. Thus, the number of moles of KOH used in the titration is 55 ml * 0.10 M = 5.5 mmol. This is also the number of moles of HF present in 30 ml, so the concentration of the hydrofluoric acid solution is 5.5 mmol / 30 ml = 0.183 M.
How do you prepare a solution that is 5000 PPM acetic acid?
add 2.4ml glacial aetic acid in one liter of d.m water
20ml of acetic acid is titrated with a solutuion of 0.15 m naoh if 35 ml of naoh are required to reach the equivalence point what is the concentration of the acetic acid solution?
.26
How can we react dehydrating agent with acetic acid?
Dehydration of acetic acid to prepare acetic anhydride occur at 8oo oC.
