To prepare a 0.02 M solution of HCl, you would need to dilute concentrated HCl solution with a calculated amount of water. For example, to prepare 1 liter of 0.02 M HCl solution, you would mix 4.2 ml of concentrated HCl (12 M) with 995.8 ml of water. Always add acid to water slowly and with stirring to avoid splattering.
0.02M=20mM(multiply x1000)
From a 1M stock HCL I shall prepare 100ml of 20mM HCl by the following equation
V1N1=V2N2
100mlx20mM=1000mMx"V2"
V2=100x20/1000
=2ml.
So add 2ml of 1M stock HCl plus 98ml of water to make 100ml of 0.02M HCL; this formula applies for any amount/concentration of solution. Hope this help you.
To prepare 1N HCl solution, you need to dilute concentrated HCl (usually 37% w/w) with water to get the desired concentration. For a 1N HCl solution, you would mix 1 part of concentrated HCl with 9 parts of water (ratio of 1:9). The volume needed would depend on the final volume required and the concentration of the concentrated HCl you start with.
To find the molarity, first calculate the number of moles of HCl present: 85.6 g / 36.46 g/mol = 2.35 mol Then, divide the moles by the volume in liters: Molarity = 2.35 mol / 0.385 L ≈ 6.10 M. Thus, the molarity of the solution is approximately 6.10 M.
To prepare 500ml of 0.12N HCl solution, you will need to dilute a concentrated hydrochloric acid solution. To do this, measure out 2.5ml of concentrated HCl (37% w/w) and dilute it to 500ml with distilled water. Be sure to wear appropriate safety equipment and handle the acid with caution.
To find the volume of the 2.00 M HCl stock solution needed, we use the formula M1V1 = M2V2. Rearranging for V1 gives us V1 = (M2 * V2) / M1, where M2 is the desired concentration (0.50 M), V2 is the final volume (150 mL), and M1 is the stock concentration (2.00 M). Plugging in the values gives V1 = (0.50 M * 150 mL) / 2.00 M = 37.5 mL. You will need 37.5 mL of the 2.00 M HCl stock solution to make a 150 mL solution of 0.50 M HCl.
To find the moles of HCl consumed, we first calculate the moles of HCl in 25 mL of 4 M solution: 25 mL * 4 mol/L = 100 mmol. Since CaCO3 is in excess, it reacts with all the HCl.
100 M HCl don't exist.
make sure to sudy it alot
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.
To prepare a 0.100 M HCl solution from a 1.50 M HCl solution, you need to use the dilution formula, which is M1V1 = M2V2. You would need to use (V_1 = \frac{M_2V_2}{M_1}) to calculate the volume needed. Plugging in the values, you would need to use ( V_1 = \frac{0.100 M \times 2.00 L}{1.50 M} = 0.133 L or 133 mL) of the 1.50 M HCl solution.
To prepare a hydrochloric acid (HCl) solution, you can dilute concentrated hydrochloric acid with water. Always add the acid to water slowly while stirring, never add water to acid, as it can cause splattering. Be sure to wear appropriate protective gear and work in a well-ventilated area when handling HCl.
you need to make 1000 times dilutions, this could be done in multi-steps: transfer 1 ml 0.1 M HCl into 100 ml volumetric flask and complete volume with water --------(1) from solution (1) transfer 2 ml into 20 ml volumetric falsk and complete volume with water, this is 0.0001 M HCL.
To find out how much 25 M HCl must be diluted to prepare 1.5 L of 4.1x10-2 M HCl, you can apply the dilution formula: M1V1 = M2V2. Plug in the values to find the initial volume of 25 M HCl that needs to be diluted to prepare 1.5 L of 4.1x10-2 M HCl.
To prepare a 10 ml of a 25 M HCl solution, you would need to dilute the 1 M HCl solution by a factor of 25. You will need 0.25 ml of the 1 M HCl solution and 9.75 ml of solvent (usually water) to make a total volume of 10 ml for the 25 M HCl solution.
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.
To prepare a liter of 0.5N HCl solution, you would measure 50 mL of concentrated hydrochloric acid (37% HCl by mass) and dilute it to 1 liter with distilled water.
To prepare a 3.8 M HCl solution, you would need to measure 65.36 mol of HCl. You can then dilute this to a final volume of 17.2 L using water. Make sure to wear appropriate protective gear and handle the concentrated HCl solution with caution, as it is a strong acid.
To prepare 1000 mL of 1 M HCl solution from concentrated HCl (typically 37% w/w), you would need to dilute 88 mL of concentrated HCl with distilled water to reach the 1000 mL mark. This is because the concentrated HCl is about 12 M. Be sure to add the acid slowly to water while stirring, and always handle concentrated acids with caution due to their corrosive nature.