0
To standardize 0.5 M HCl, you would typically titrate it using a primary standard solution such as sodium carbonate (Na2CO3). By titrating a known volume of the HCl with the sodium carbonate solution and using the mole ratio between the two, you can calculate the exact concentration of the HCl solution. This process ensures that the concentration of the 0.5 M HCl is accurate for future use in experiments.
What else can I help you with?
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
How do you standardise 0.1M HCl?
To standardize 0.1 M HCl, you would first need to titrate it against a solution of known concentration, usually sodium hydroxide (NaOH). By carefully adding the NaOH solution to the HCl solution until the reaction is complete, you can determine the exact concentration of the HCl solution. This process allows you to adjust the concentration of the HCl solution to the desired 0.1 M.
What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
To find the volume of 12.0 M HCl needed to make 75.0 mL of 3.50 M HCl, you can use the formula C1V1 = C2V2. Substituting in the given values, you will find that approximately 21.9 mL of 12.0 M HCl is required.
How do you make 25 ml of a 0.0010 M HCl starting with 0.010 M HCl?
V = volume, M = molarity V1M1=V2M2 (25 mL)(0.0010 M) = (x)(0.010 M) x = (25 mL)(0.0010 M)/(0.010 M) x = 2.5 mL To make a 25 mL 0.0010 M HCl solution with 0.010 M HCl, you would measure out 2.5 mL of the 0.010 M HCl in a 25 mL graduated cylinder (or laboratory equipment of your choice) and then add 22.5 mL of distilled water.
What is the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
How do you standardise 0.1M HCl?
To standardize 0.1 M HCl, you would first need to titrate it against a solution of known concentration, usually sodium hydroxide (NaOH). By carefully adding the NaOH solution to the HCl solution until the reaction is complete, you can determine the exact concentration of the HCl solution. This process allows you to adjust the concentration of the HCl solution to the desired 0.1 M.
Why you need to standardize HCl solution?
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
Is 1 m HCl is more reactive than 4m HCl?
1 m HCl is not more reactive than 4m HCl, but 4m HCl is more concentrated.
What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
To find the volume of 12.0 M HCl needed to make 75.0 mL of 3.50 M HCl, you can use the formula C1V1 = C2V2. Substituting in the given values, you will find that approximately 21.9 mL of 12.0 M HCl is required.
How do you make 25 ml of a 0.0010 M HCl starting with 0.010 M HCl?
V = volume, M = molarity V1M1=V2M2 (25 mL)(0.0010 M) = (x)(0.010 M) x = (25 mL)(0.0010 M)/(0.010 M) x = 2.5 mL To make a 25 mL 0.0010 M HCl solution with 0.010 M HCl, you would measure out 2.5 mL of the 0.010 M HCl in a 25 mL graduated cylinder (or laboratory equipment of your choice) and then add 22.5 mL of distilled water.
What is the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
How do you standardization 1N hcl?
To standardize 1N HCl (hydrochloric acid), you would typically use a primary standard base, such as sodium hydroxide (NaOH), of known concentration to titrate the HCl solution. By carefully titrating the HCl with the NaOH, you can determine the exact concentration of the HCl solution. This information can then be used to adjust the concentration of the HCl solution as needed to make it accurately 1N.
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
Standardization of Hcl using Borax?
You can standardize a hydrochloric acid (HCl) solution using borax (sodium borate) by titrating a known concentration of HCl with a solution of borax. The reaction between HCl and borax can be used to determine the exact concentration of the HCl solution. By accurately measuring the volume of the titrant and using stoichiometry, you can calculate the concentration of the HCl solution.
What volume of 3.0 M HCl sould be obtained to prepare 100 mL of 1.0 M HCL?
To prepare 100 mL of 1.0 M HCl from a 3.0 M stock solution, you can use the formula: (M_1V_1 = M_2V_2). Solving for V1: (3.0 M)(V1 mL) = (1.0 M)(100 mL), thus V1 = 33.3 mL. So, you would need to measure out 33.3 mL of the 3.0 M HCl solution and then dilute it to 100 mL to obtain 1.0 M HCl.
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.
