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A certain amount of hydrogen peroxide was dissolved in 100 ml of water and then titrated with 1.68m kmno4 how much h2o2 was dissolved if the titration required 22.3 ml of the kmno4 solution?
To calculate the amount of hydrogen peroxide (H2O2) dissolved, you can use the equation: moles of KMnO4 = moles of H2O2. Firstly, calculate the moles of KMnO4 (given concentration and volume). Then, use the balanced chemical equation to determine the moles of H2O2, as they have a 1:1 stoichiometric ratio. Finally, convert moles of H2O2 to grams using the molar mass to find the amount dissolved in the solution.
What if a 50.0 mL o a 0.500 M solution of H2O2 is decomposed what mass of O2 will be produced?
The chemical equation for the decomposition of H2O2 is 2 H2O2 -> 2 H2O + O2. This shows that two moles of H2O2 are required to produce each mole of O2. By definition, a 0.500 M solution of H2O2 contains 0.500 moles of H2O2 in each liter of solution. Solutions are always homogeneous; therefore, 50,0 mL of such a solution will contain (0.500)(50.0/1000) or 0.0250 moles of H2O2. As noted in the first paragraph, this will produce half as many, or 0.0125, moles of O2. The gram molar mass of O2 is twice the gram atomic mass of oxygen, or 31.9988. Therefore, decomposition of this amount of H2O2 will produce 31.9988 X 0.0125 or 0.400 gram of O2, to the justified number of significant digits.
What is the molarity of a 3.0 percent hydrogen peroxide H2O2 aqueous solution when the density is essentially 1.0g over mL?
If the density is 1.0 g/ml, one liter of the solution will weigh 1000 grams. 3.0 % of this mass or 30 grams of it is constituted of H2O2. The molar mass of H2O2 is 2 (1.008 + 15.999) = 34.014. The molarity of this solution is therefore 30/34.014 = 0.88, to the justified number of significant digits.
How many grams of hydrogen peroxide H2O2 must be added to 1500 ml of water to produce a concentration of 1.33 m molal solution Recall that the density of water is 1.0 gram?
To calculate the amount of hydrogen peroxide (H2O2) needed to make a 1.33 molal solution in 1500 ml of water, you first need to convert the volume of water to grams. Since the density of water is 1.0 g/ml, 1500 ml of water is equal to 1500 grams. Next, calculate the moles of H2O2 needed using the molality formula (molality = moles of solute / mass of solvent in kg). Then convert the moles to grams by multiplying by the molar mass of H2O2 (34.02 g/mol).
How much water would I add to a 50percent solution of H2O2 to make 500 ml of 3percent H2O2?
To make a 500 ml solution of 3% H2O2 from a 50% solution, you would need to dilute the 50% solution with water. You would add 325 ml of water to 175 ml of the 50% H2O2 solution to achieve a final volume of 500 ml with a concentration of 3% H2O2.
A certain amount of hydrogen peroxide was dissolved in 100 ml of water and then titrated with 1.68m kmno4 how much h2o2 was dissolved if the titration required 22.3 ml of the kmno4 solution?
To calculate the amount of hydrogen peroxide (H2O2) dissolved, you can use the equation: moles of KMnO4 = moles of H2O2. Firstly, calculate the moles of KMnO4 (given concentration and volume). Then, use the balanced chemical equation to determine the moles of H2O2, as they have a 1:1 stoichiometric ratio. Finally, convert moles of H2O2 to grams using the molar mass to find the amount dissolved in the solution.
What if a 50.0 mL o a 0.500 M solution of H2O2 is decomposed what mass of O2 will be produced?
The chemical equation for the decomposition of H2O2 is 2 H2O2 -> 2 H2O + O2. This shows that two moles of H2O2 are required to produce each mole of O2. By definition, a 0.500 M solution of H2O2 contains 0.500 moles of H2O2 in each liter of solution. Solutions are always homogeneous; therefore, 50,0 mL of such a solution will contain (0.500)(50.0/1000) or 0.0250 moles of H2O2. As noted in the first paragraph, this will produce half as many, or 0.0125, moles of O2. The gram molar mass of O2 is twice the gram atomic mass of oxygen, or 31.9988. Therefore, decomposition of this amount of H2O2 will produce 31.9988 X 0.0125 or 0.400 gram of O2, to the justified number of significant digits.
What is the molarity of a 3.0 percent hydrogen peroxide H2O2 aqueous solution when the density is essentially 1.0g over mL?
If the density is 1.0 g/ml, one liter of the solution will weigh 1000 grams. 3.0 % of this mass or 30 grams of it is constituted of H2O2. The molar mass of H2O2 is 2 (1.008 + 15.999) = 34.014. The molarity of this solution is therefore 30/34.014 = 0.88, to the justified number of significant digits.
How many grams of hydrogen peroxide H2O2 must be added to 1500 ml of water to produce a concentration of 1.33 m molal solution Recall that the density of water is 1.0 gram?
To calculate the amount of hydrogen peroxide (H2O2) needed to make a 1.33 molal solution in 1500 ml of water, you first need to convert the volume of water to grams. Since the density of water is 1.0 g/ml, 1500 ml of water is equal to 1500 grams. Next, calculate the moles of H2O2 needed using the molality formula (molality = moles of solute / mass of solvent in kg). Then convert the moles to grams by multiplying by the molar mass of H2O2 (34.02 g/mol).
The mass percent of hydrogen in hydrogen peroxide H2O2?
The mass percent of hydrogen in hydrogen peroxide (H2O2) is 5.88%. This is calculated by taking the total mass of hydrogen in one molecule of H2O2 (2.01 g) divided by the total molar mass of H2O2 (34.02 g/mol) and multiplying by 100.
How much water would I add to a 50percent solution of H2O2 to make 500 ml of 3percent H2O2?
To make a 500 ml solution of 3% H2O2 from a 50% solution, you would need to dilute the 50% solution with water. You would add 325 ml of water to 175 ml of the 50% H2O2 solution to achieve a final volume of 500 ml with a concentration of 3% H2O2.
What is pirana solution?
30% h2o2+h2so4
What is the balanced equation for potassium iodide and H2O2 solution?
H2O2 + 2 KI --> 2 KOH + I2
How do you calculate the molality of a solution?
To calculate the molality of a solution, you divide the moles of solute by the mass of the solvent in kilograms. The formula for molality is: Molality (m) moles of solute / mass of solvent (in kg).
An aqueous solution of glycerol C3H8O3 is 48.0 percent glycerol by mass and has a density of 1.120 g mL-1. Calculate the molality of the glycerol solution?
First, calculate the mass of glycerol in 100g of the solution: 48.0g glycerol/100g solution = 48.0%. Next, calculate the mass of water in 100g of the solution: (100g - 48.0g glycerol) = 52.0g of water. Calculate the moles of glycerol by dividing the mass of glycerol by its molar mass: 48.0g / 92.09g/mol = 0.521 mol. Calculate the molality by dividing the moles of solute by the mass of solvent in kg: 0.521 mol / 0.052 kg = 10 mol/kg.
Calculate the mole fraction of benzene in solution containing 30 percent by mass in carbon tetrachloride?
calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetra chlorid
H2o2 used to give stress?
H2o2 is used to give stress. The is also called hydrogen peroxide solution.
