If you started with 24.75 ml of a hydrogen peroxide solution that contained 3.85 % H2O2 by mass, what would be the volume of this gas in ml at STP? The density of the solution is 1.0 g/ml and the molar volume of a gas at STP is 22.4 L/mol. (Put your answer in 3 significant figures)
If you started with 24.75 ml of a hydrogen peroxide solution that contained 3.85 % H2O2...
Hydrogen peroxide, H2O2, is available in stores as a 3.5% v/v solution on water. What volume of hydrogen peroxide is present in 243 mL of this solution? Give your answer to two significant figures. Answer in mL H2O2
3. The density of 30 % (w/w) aqueous hydrogen peroxide (H2O2, MW = 38 g/mole) is 1.05 g/mL. Recall that this solution consists of H2O2 and water (a) What's the molarity (M) of 30 % (w/w) aqueous hydrogen peroxide? (20 points) a. 7.29 b. 8.29 C. 9.29 d. 10.29 e. 11.29 (b) How much volume (mL) of 30 % (w/w) hydrogen peroxide (H2O2, MW = 38 g/mole) is required if you want to prepare 1.0 M of 1000 ml solution?...
The concentration of hydrogen peroxide, H2O2, in a solution is determined by titrating a 13.0 mL sample of the solution with permanganate ion, producing manganese(II) ion and oxygen gas. Part A Enter the balanced chemical equation for the redox reaction that occurs in acidic solution. Part B If it takes 16.6 mL of 0.127 M permanganate solution to reach the equivalence point, what is the molarity of the hydrogen peroxide solution?
A solution or hydrogen peroxide is 26.3 H2O2 by mass and has a density of 1.11 g/cm3 the molarity of the solution is
Over time, hydrogen peroxide, H2O2, degrades into water and oxygen gas. A bottle of hydrogen peroxide is expired and you need to determine the concentration. A titration is performed using the following equation: 3 H2O2(aq) + 2 NaMnO4(aq) → 3 O2(g) + 2 MnO2(aq) + 2 NaOH(aq) + 2 H2O(l) Note that permanganate ion, MnO4-, is purple, while manganese (IV) ion, Mn4+, is colorless. A quantity of 683 mL of 3.44 M NaMnO4 was measured and placed in a beaker. The solution...
A 60 ppm solution of hydrogen peroxide is 60 mg of H2O2 per 1000 g of solution. Assuming that the density of this solution is 1.00 g/ml, convert this concetration from ppm to molarity.
Reaction 1 (10 mL undiluted 1.0% IKI and 5 mL undiluted 3% H2O2) Reaction 2 (10 mL diluted 0.5% IKI and 5 ml undiluted 3% H2O2) Reaction 3 (10 mL undiluted 1.0% IKI and 5 mL diluted 2.25% H2O2) 13. Answer the following. ( a) How many moles of H2O2 are present in Reactions 1 and 2? Show your work (include units). Hint: The initial H2O2 solution is 3% m/v (mass/volume) hydrogen peroxide in water. That means that 3 g...
• 21. A student titrates a 2.00 mL sample of hydrogen peroxide solution, HoOz(aa), according to the reaction 2 MnO2(aq) +5H20_ag) +6H*(aq) 2 Mni?"(aq) +502(9) +8H200- The supply bottle of H2O2 is labelled as *3.00% by volume" (3.00 mL of H2O2 per 100 mL of solution), which the student calculates to have [H2O) = 1.24 M. a) What volume of 0.0496 M MnO is required for the titration? b) What volume of O2(g) at STP is produced during the reaction?
by titration with permanganate solution. The 13) Hydrogen peroxide, H2O2, can be determined by titration with permans reaction is: 2 MnO4 (aq) + 5 H2O2(aq) + 6 H+ + 502(g) + 2 Mn2(aq) + 8 H20 ate 5.0 mL of a H2Oz(aq) If it required 80.0 mL of 0.0220 molar MnO4 (aq) solution to titrate 5.0 m solution, what is the molarity of the H2O2(aq) solution?
2. A student performed the experiment described in this module, using 5.00 mL of a 2.50% H2O2 solution with a density of 1.01 g mL-1. The water temperature was 24°C, and the barometric pressure in the labora- tory was 30.50 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 43.70 mL of O2.(8) Calculate the number of moles of H2O2 reacting (9) Calculate the number of moles of collected O2 (10) Calculate the molar volume of O2...