Answer:
2-butanone = 72.11 g/mol (option F)
Propyl acetate = 102.13 g/mol (option C)
4-methyl-2-pentanone = 100.16 g/mol (option D)
Butyl acetate = 116.16 g/mol (option B)
Methanol = 32.04 g/mol (option E)
Ethanol = 46.07 g/mol (option A)
Explanation:
Step 1: Data given
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of O = 16.00 g/mol
Step 2:
2-butanone = C4H8O
⇒ 4*12.01 + 8*1.01 + 16.00 = 72.11 g/mol (option F)
Propyl acetate = C5H10O2
⇒ 5*12.01 + 10*1.01 + 2*16.00 = 102.13 g/mol (option C)
4-methyl-2-pentanone = C6H12O
⇒ 6*12.01 + 12*1.01 + 16.00 = 100.16 g/mol (option D)
Butyl acetate = C6H12O2
⇒ 6*12.01 + 12*1.01 + 2*16.00 = 116.16 g/mol (option B)
Methanol = CH3OH = CH4O
⇒ 12.01 + 4*1.01 + 16.00 = 32.04 g/mol (option E)
Ethanol = C2H5OH = C2H6O
⇒ 2*12.01 + 6*1.01 + 16.00 = 46.07 g/mol (option A)
Scientist and Chemical Engineers
The approximate alcohol content is 210 ml.
Explanation:
It can be deduced from the question that each bottle is of 1000ml or 1 litre.
The first bottle is one half full means it has 500 ml of solution and it has 20% alcohol in it. So volume of alcohol in the solution is
20/100*500
=100 ml
The first bottle is one fifth full, so the volume of mixture is 1/5th of 1000ml
so it is 200ml having 30% alcohol
30/100*200
= 60 ml
The third bottle is one tenth full so its volume is 1/10*1000
100 ml. having 50% of alcohol
50/100*100
50 ml.
The alcohol content obtained from all these 3 litres is:
100+60+50
= 210 ml of alchohol is obtained from 800 ml of mixture.
You need to monitor the solution to see when the crystals start gathering at the bottom of the solution. You can slowly add alum until it stops dissolving. The point just before it starts its sedimentation at the bottom is the point when the solution is saturated.
Answer:
See Explanation
Explanation:
Note => 1st one should understand that for an 'acid' to be an acid and a 'base' to be a base, two requirements must be met, (1) the compound must have an ionizable Hydrogen for acids or Hydroxide for bases, and (2) must be in water and ionize delivering H⁺ ions from acids and OH⁻ ions from bases. The Arrhenius acids are characterized by having an ionizable hydrogen which when added into water increases the hydronium ion concentration (H₃O⁺). Arrhenius bases are characterized by having an ionizable hydroxide function (OH-).
Typically, the acids and bases are characterized as either strong or weak electrolytes. the Strong electrolytes ionize 100% in water and Weak electrolytes less than 100%.
The strong acids include HCl, HBr, HI, HNO₃, HClO₄ and H₂SO₄ (1st ionization step). Any acid (H-Anion) not a member of the strong 6 is a weak acid.
The strong Arrhenius Bases are Group IA and Group IIA Hydroxides except for Beryllium Hydroxide. Weak Arrhenius Bases are ammonia or ammonia derivatives (amines) in water.
=> NH₃ + H₂O => NH₄OH ⇄ NH⁺ + OH⁻.
The ammonia derivatives follow the same reactive nature in water.
=> RNH₂ + H₂O => RNH₃OH ⇄ RNH₃⁺ + OH⁻ where R- is a structural substrate; e.g., Methyl Amine => H₃C - NH₂ .
