A solution is prepared by dissolving 20.5 g of NaOH in 130.0 g of water. The NaOH solution has a density of 1.15 g/mL. Part A What is the mass percent (m/m) of the NaOH solution? 13.6 % (m/m) Submit Previous Answers Correct Part B What is the total volume, in milliliters, of the solution? V = 131 mL Subimit Previous Answers Correct Part C What is the mass / volume percent (m/v) of the solution? HV ΑΣφ
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- PLEASE STATE A, B, C or D! Consider 2 aqueous solutions: H2O/NaCl and H2O/CH3OH. Which one will exhibit a positive/negative/no deviation compare to Raoult’s prevision: a.H2O/NaCl and H2O/CH3OH both exhibit a negative deviation b.H2O/NaCl and H2O/CH3OH both exhibit a positive deviation c.H2O/NaCl and H2O/CH3OH don’t exhibit any deviation d.H2O/NaCl negative deviation and H2O/CH3OH positive deviation e.H2O/NaCl positive deviation and H2O/CH3OH negative deviationWhat's the differences between two questions? Q1) How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations. -->Tap water 8Oz = 8 x 0.0296L = 0.2368L Hardness = 66.73ppm = 66.73mg/L CaCO3 1L has 66.73mg CaCO3 0.2368L has 66.73mg x 0.2368 = 15.8017mg MW of CaCO3 = 100g/mol MW of Ca = 40g/mol 100g CaCO3 has 40gf of Ca 15.8017mg CaCO3 has 40/100 x 15.8017mg Ca We would ingest 6.321mg of Ca. Q2) What percentage of the recommended daily dose of calcium (1,150 mg/day) does 1.0 L of your water provide? Show all calculations. --> 66.73mg/1150mg x 100 = 5.80% My Question) Why this calculation is wrong? I think this calculation is same with question 1. Isn't it? CaCO3 = 100g/mol, Ca = 40g/mol 100g CaCO3 has 40g Ca. 66.73 CaCO3 has 40/100 x 66.73mg Ca Ca = 26.70mg 26.70mg/1150mg x 100 = 2.32%What is normality of a solution containing 90g of HCI in 2600ml of solution? (Use the given information: MW:H=1g/mol, Cl=35g/mol)A. 0.00048 eq/molB. 0.48 eq/molC. 0.00096 eq/molD. 0.96 eq/mol
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