How to prepare 0.1M 100mL AgNo3 (MW = 169.8731 g/mol)
So, what we have is,
M=0.1M
V=100mL/0.1L
MW=169.8731g/mol
Weight = ?
Formula:-
mol = M x V = Weight / MW
thus weight = M x V x MW
= 0.1 x 0.1 x 169.8731 (mol/L x g/mol x L)
= 1.69g
Measure 1.69g of AgNO3 and put inside a 100mL volumetric flask. top up with distilled H2O until 100mL. Siap!
The easiest way is to get a litre volumetric flask. Find out the molarity or the %V/V. If you have molarity, it is a simple exercise to find out how much you need by dilution factor.. If you have %V/V, you need to get the density. This gives you the weight per volume. Then you can get the moles per volume via no. moles is mass/molecular weight. You can now work out the molarity of the stock by bringing the volume to 1000. Now you do the same as before, i.e. dilution factor.
Molecular weight multiplied by 0.1
17 g per litre
The strength of a solution may be described as a percentage or volume, where 1% hydrogen peroxide releases 3.3 volumes of oxygen during decomposition.Thus, a 3% solution is equivalent to 10 volume and a 6% solution to 20 volume, etc. Answer taken from Wikipedia 19/01/2009
.01% of australia
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