(100ml)(0.125M NaOH) = (500ml)(X Molarity)
Molarity = 0.025 M
Diluted and concentrated solutions.
The molarity is 0,1 M.
less then 0.01M
Solutions with low concentrations of solutes are called diluted.
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
Solutions that have a small amount of solute.
Diluted and concentrated solutions.
The molarity is 0,1 M.
(126)(1.3)=163.8 divide 163.8 by 450 = .364 which is the answer
The moon. Come on!
less then 0.01M
Solutions with low concentrations of solutes are called diluted.
Ask a doctor, mentioning the chemical; generally: - for acid solutions: wash with a diluted basic solution - for basic solutions: wash with a diluted acidic solution
initial molarity*initial volume= final molarity*final volume Initial molarity= 1.50M Initial volume= 20.00ml Final Volume=150.0ml Thus final molarity =1.50M*20ml/150ml=0.200M. New molar concentration= final molarity
pH is actually a measure of hydrogen ion concentration, similar to how molarity is a measure of the concentration of other solutions. The pH of the acid will become more neutral, in this case higher if it's being diluted with water.
0.6m
Use c1*V1=c2*V2 to calculate:(this goes for ANY molarity, not only for acetic acid as questioned)5(M) * 2(L) = x(M) * 7.5(L) , so x = molarity of the diluted = 1.3 M