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How do you prepare 0.2 mol per liter HCl from concentrated HCL?
To prepare 0.2 mol/L HCl from concentrated HCl (e.g., 37% HCl), you would need to dilute the concentrated HCl with water in the appropriate ratio. Since the concentrated HCl usually has a density of around 1.19 g/mL, you can use the formula M1V1 = M2V2 to calculate the volume of concentrated HCl needed. After calculating the volume of concentrated HCl required, add water to make up the final volume of 1 liter to achieve a 0.2 mol/L HCl solution.
For Kovac's reagent what concentration of hydrochloric acid do you use?
Most recipes just specify 'concentrated' HCl. That could mean 32 % or 37 %. One or two specify 32 %. Now, HCl 32 % w/w = 37 % w/v and HCl 37 % w/w = 44 % w/v, and since the HCl in Kovacs Reagent is mixed 1:3 (by volume) with isoamyl alcohol, the final concentration of HCl will be 9.25 % w/v or 11 % w/v respectively. Further, some recipes specify a 1:3 mixture by mass - resulting in proportionally much less HCl. So it's not critical. I'm using 32 %.
What will be the pH of the solution formed by mixing 40ml of 0.1M HCl with 10ml of 0.45M NaOH?
To calculate the pH of the resulting solution when mixing HCl and NaOH, you need to determine the moles of each reactant. Use these values to find the limiting reagent and the excess reagent. Then, calculate the concentration of the excess reagent left in solution. Finally, use the concentrations of the excess reagent and water to determine the pH of the resulting solution.
What are the concentrations of HCl?
By dilution in water we can obtain a large range of hydrochloric acid concentrations depending on necessities. As bottled laboratory reagent HCl has concentrations of 25 %, 30-32 % and 37 % (fumans).
Why you use 85 ml Conc HCl for 1 M HCl?
To prepare 1 M hydrochloric acid (HCl) solution, you usually need to dilute concentrated HCl solution (~35-37% HCl) with water in a specific ratio. The specific volume of concentrated HCl needed depends on its concentration and the final volume of the 1 M solution you want to make. In this case, 85 ml of concentrated HCl is likely to be the volume needed to make 1 L of 1 M HCl solution.
A 250ml sample of 0.20M HCl is to be made by diluting the approximate amount of the concentrated reagent 11.7M what volume of the latter should be used?
To calculate the amount of concentrated 11.7M HCl needed to make a 250ml sample of 0.20M HCl, you can use the formula: M1V1 = M2V2 where M1 = 11.7M, V1 is the volume of concentrated HCl needed, M2 = 0.20M, and V2 = 250ml. Plugging in these values, you'll find that approximately 4.25ml of the concentrated 11.7M HCl reagent should be used.
How do you prepare 0.2 mol per liter HCl from concentrated HCL?
To prepare 0.2 mol/L HCl from concentrated HCl (e.g., 37% HCl), you would need to dilute the concentrated HCl with water in the appropriate ratio. Since the concentrated HCl usually has a density of around 1.19 g/mL, you can use the formula M1V1 = M2V2 to calculate the volume of concentrated HCl needed. After calculating the volume of concentrated HCl required, add water to make up the final volume of 1 liter to achieve a 0.2 mol/L HCl solution.
For Kovac's reagent what concentration of hydrochloric acid do you use?
Most recipes just specify 'concentrated' HCl. That could mean 32 % or 37 %. One or two specify 32 %. Now, HCl 32 % w/w = 37 % w/v and HCl 37 % w/w = 44 % w/v, and since the HCl in Kovacs Reagent is mixed 1:3 (by volume) with isoamyl alcohol, the final concentration of HCl will be 9.25 % w/v or 11 % w/v respectively. Further, some recipes specify a 1:3 mixture by mass - resulting in proportionally much less HCl. So it's not critical. I'm using 32 %.
What will be the pH of the solution formed by mixing 40ml of 0.1M HCl with 10ml of 0.45M NaOH?
To calculate the pH of the resulting solution when mixing HCl and NaOH, you need to determine the moles of each reactant. Use these values to find the limiting reagent and the excess reagent. Then, calculate the concentration of the excess reagent left in solution. Finally, use the concentrations of the excess reagent and water to determine the pH of the resulting solution.
What are the concentrations of HCl?
By dilution in water we can obtain a large range of hydrochloric acid concentrations depending on necessities. As bottled laboratory reagent HCl has concentrations of 25 %, 30-32 % and 37 % (fumans).
Why you use 85 ml Conc HCl for 1 M HCl?
To prepare 1 M hydrochloric acid (HCl) solution, you usually need to dilute concentrated HCl solution (~35-37% HCl) with water in a specific ratio. The specific volume of concentrated HCl needed depends on its concentration and the final volume of the 1 M solution you want to make. In this case, 85 ml of concentrated HCl is likely to be the volume needed to make 1 L of 1 M HCl solution.
How do you prepare 0.5M HCL from 37 percent HCL?
Depending if you want your % to be in volume and you have 100 mL then add 212.5mL to the HCl. If you want it by mass and you have 100g of HCl then add 212.5 g of water which is about 212.5 mL anyways. #swag
How do you prepare Schultz Reagent?
To prepare Schultz reagent, mix one part of concentrated sulfuric acid with nine parts distilled water. Allow the mixture to cool before use. This reagent is commonly used for the detection of proteins in biological samples.
How do you prepare 1N Hcl solution Dont tell in gL how much ml is required?
1N HCL is the same as 1 Molar HCl. You take the # of H ions and multiply by the molarity to get the Normality. Usually you buy HCl in concentrated form which is 12 Molar or 12 Normal HCL. You need to dilute the concentrated HCl to get the reduced concentration. Use the formula Molarity Initial x Volume Initial = Molarity Final x Volume Final ex. 12 M HCL x 10 ml = 1 M x 120 ml. So take 10 ml of concentrated HCl and add enough water to make 120 ml. This will give you 120 ml of 1 M (which is 1N) HCl. Venkat Reddy
Which is better to adjust pH 1N HCl or conc HCl?
It is better to use concentrated HCl to adjust pH as it is more efficient and allows for better control of the pH level compared to dilute 1N HCl. Additionally, concentrated HCl may require less volume to achieve the desired pH level.
How can you prepare borsches reagent in the lab?
To prepare Borsches reagent in the lab, mix equal volumes of concentrated sulfuric acid and glacial acetic acid in a fume hood. Then, slowly add 9 parts of water to the mixture while stirring constantly. Allow the reagent to cool before use.
How do you evaporate 0.1m HCL?
To evaporate 0.1M HCl solution, you can heat the solution to a temperature where the water component will evaporate, leaving behind the concentrated hydrochloric acid. Ensure proper ventilation as the fumes from concentrated HCl can be harmful. It is important to follow safety protocols and use appropriate equipment when working with concentrated acids.
