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What volume of 0.1125 m k2cr2o7 would be required to oxidize 48.16 ml of 0.1006 na2so3 in acidic solution the product includes cr3 plus and SO42?
To find the volume of 0.1125 M K2Cr2O7 required, first balance the equation: 14H+ + 6Na2SO3 + K2Cr2O7 → 2Cr3+ + 3SO42- + 6Na+ + 2K+ + 7H2O. Then, use the mole ratio to calculate moles of Na2SO3 used, and finally the volume of K2Cr2O7 needed.
Why do you use 0.005M h2so4 solution for preparation of k2cr2o7 solution for UV calibration?
Because Cr2O72- ion is only stable for hydrolysis by keeping pH < 2.0(pH < 2.0 means [H+] > 0.01 M, which equals > 0.005 M H2SO4)To prevent the formation of chromate CrO42- ions in the equilibrium -below- keeping it to the left side (
How do you prepare a stock solution?
To prepare a stock solution, you need to measure a specific amount of solute and dissolve it in a specific volume of solvent to achieve a desired concentration. This concentrated solution can then be diluted as needed for use in experiments or applications.
Which is the best instrument to use to prepare a solution?
The best instrument to use to prepare a solution depends on the accuracy and volume of the solution needed. Common instruments include pipettes for precise measurements and volumetric flasks for accurate volume measurements. Additionally, a balance may be used to weigh out solid solutes for solution preparation.
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?
To prepare the 0.50M acetic acid solution, you can use the formula C1V1 = C2V2. Plugging in the values, you get (2.5M)(V1) = (0.50M)(100.0mL). Solving for V1 gives V1 = 20.0 mL. Therefore, 20.0 milliliters of the 2.5M stock solution is required to prepare 100.0 milliliters of the 0.50M acetic acid solution.
What volume of 0.1125 m k2cr2o7 would be required to oxidize 48.16 ml of 0.1006 na2so3 in acidic solution the product includes cr3 plus and SO42?
To find the volume of 0.1125 M K2Cr2O7 required, first balance the equation: 14H+ + 6Na2SO3 + K2Cr2O7 → 2Cr3+ + 3SO42- + 6Na+ + 2K+ + 7H2O. Then, use the mole ratio to calculate moles of Na2SO3 used, and finally the volume of K2Cr2O7 needed.
Why do you use 0.005M h2so4 solution for preparation of k2cr2o7 solution for UV calibration?
Because Cr2O72- ion is only stable for hydrolysis by keeping pH < 2.0(pH < 2.0 means [H+] > 0.01 M, which equals > 0.005 M H2SO4)To prevent the formation of chromate CrO42- ions in the equilibrium -below- keeping it to the left side (
How do you prepare a stock solution?
To prepare a stock solution, you need to measure a specific amount of solute and dissolve it in a specific volume of solvent to achieve a desired concentration. This concentrated solution can then be diluted as needed for use in experiments or applications.
Which is the best instrument to use to prepare a solution?
The best instrument to use to prepare a solution depends on the accuracy and volume of the solution needed. Common instruments include pipettes for precise measurements and volumetric flasks for accurate volume measurements. Additionally, a balance may be used to weigh out solid solutes for solution preparation.
Why use sodium chloride for medicine?
Sodium chloride is used to prepare the 0,9 % isotonic solution.
Use the term solvent and solute to describe how to prepare a salt solution?
The solute (NaCl) is dissolved in the solvent (water)
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?
To prepare the 0.50M acetic acid solution, you can use the formula C1V1 = C2V2. Plugging in the values, you get (2.5M)(V1) = (0.50M)(100.0mL). Solving for V1 gives V1 = 20.0 mL. Therefore, 20.0 milliliters of the 2.5M stock solution is required to prepare 100.0 milliliters of the 0.50M acetic acid solution.
How can you prepare 1N H2SO4 from H2SO4 95 percent?
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.
Prepare a working solution from a stock solution?
it is very easy to prepare working solution from a stock solution we use the formula for this purpose which is: C1V1 = C2V2 C1 is the concentration of the stock solution V1 required volume from the stock solution C2 concentration of the working solution V2 volume of the working solution
How do you prepare 0.01N solution of sodium thiosulphate?
To prepare a 0.01N solution of sodium thiosulfate, dissolve 2.48 grams of sodium thiosulfate pentahydrate (Na2S2O3·5H2O) in distilled water and make up the solution to 1 liter. This solution will be approximately 0.01N in strength. Remember to accurately weigh the compound and use a volumetric flask for precise dilution.
How do you prepare 0.02m Naoh from 1M Naoh solution?
To prepare 0.02M NaOH from 1M NaOH solution, you will need to dilute the 1M solution. Use the formula: C1V1 = C2V2, where C1 is the concentration of the stock solution (1M), V1 is the volume of the stock solution you will use, C2 is the desired concentration (0.02M), and V2 is the final volume of the diluted solution. Calculate the volume of 1M NaOH solution (V1) needed to make the desired 0.02M concentration and dilute it with water to reach the desired volume (V2).
How do you prepare a molar solution?
To prepare a molar solution, you need to measure the correct amount of solute (substance being dissolved) in grams and dissolve it in a specific volume of solvent (usually water) to reach the desired molarity. Molarity is the number of moles of solute per liter of solution. You can use the formula: Molarity (M) moles of solute / liters of solution.
