Just compare the densities of both water and CH2Cl2. Water is less dense and will be in the top (aqueous) layer. CH2Cl2 is more dense and will be on the bottom (organic) layer. Density H2O = 1.00 g/cm3 Density CH2Cl2 = 1.33 g/cm3
Silver nitrate will react with chloride ions present in the test and standard solutions to form Silver chloride (AgCl) which is insoluble in aqueous solutions and will precipitate. this precipitate will be present as cloudiness in glass cylinders used and then we can compare this cloudiness between the test and standard solutions.
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Yes, the vapour pressure of water at 10°C is 1.2 kPa and at 50°C is 12.3 kPa.
when you go up in the air the more pressure you feel it is the same when you go deeper under water
Just compare the densities of both water and CH2Cl2. Water is less dense and will be in the top (aqueous) layer. CH2Cl2 is more dense and will be on the bottom (organic) layer. Density H2O = 1.00 g/cm3 Density CH2Cl2 = 1.33 g/cm3
its different
Silver nitrate will react with chloride ions present in the test and standard solutions to form Silver chloride (AgCl) which is insoluble in aqueous solutions and will precipitate. this precipitate will be present as cloudiness in glass cylinders used and then we can compare this cloudiness between the test and standard solutions.
who am i?
A solution is a homogeneous liquid, a suspension is not homogeneous.
You can compare peer pressure with self pressure like when you talk yourself into something like cutting or even killing yourself.
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The answer is separation.. :D
Compare and contrast the properties of dilute and concentrated solutions is because you can dilute you solvent into a solution and then you have a concentrated solution.
Cu2+ + 2AgNO3 --------> Cu(NO3)2 + 2 Ag+, due to high charge density for Copper ion as compare to Silver ion the reverse is not possible in aqueous solution.
in a solution, the atoms of a solid or gas completely separate and mix with the liquid.
A solution with a pH of 7 compared to a solution with a pH of 9 would be more acidic.