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What is the resulting molarity when 100.00mL of a 0.125 M NaOH solutions is diluted to 500mL?
Wiki User
∙ 13y ago
(100ml)(0.125M NaOH) = (500ml)(X Molarity)
Molarity = 0.025 M
Wiki User
∙ 13y ago
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What are the types of solutions according to solubility?
Diluted and concentrated solutions.
What is the molarity of iron III nitrate made from 10 ml of a 1.00 M solution and then diluted by adding 90 ml of water?
The molarity is 0,1 M.
How much solute is in diluted solutions?
less then 0.01M
Solutions with low concentrations of solutes are concentrated?
Solutions with low concentrations of solutes are called diluted.
If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
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
What are diluted solutions?
Solutions that have a small amount of solute.
What are the types of solutions according to solubility?
Diluted and concentrated solutions.
What is the molarity of iron III nitrate made from 10 ml of a 1.00 M solution and then diluted by adding 90 ml of water?
The molarity is 0,1 M.
If 120 mL of a 1.0 M glucose solution is diluted to 450.0 mL what is the molarity of the diluted solution?
(126)(1.3)=163.8 divide 163.8 by 450 = .364 which is the answer
What are some example of diluted solutions?
The moon. Come on!
How much solute is in diluted solutions?
less then 0.01M
Solutions with low concentrations of solutes are concentrated?
Solutions with low concentrations of solutes are called diluted.
What do if tongue burned with chemical?
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
If 20.00mL of a 1.50M solution of KBr is diluted to a final volume of 150.0mL what is the new molar concentration?
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
How does the pH of a concenterated acid change when it is diluted?
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.
What is the molarity of a solution prepared when 75.0 ml of a 4.00 m kcl solution is diluted to a volume of 0.500 l?
0.6m
What concentration of ch3co2h will you have if 2L of a 5M solution diluted to a volume of 7.5L?
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
