M= moles in solution/liters
so plug in what you know
3.0M of KCl solution = moles in solution/ 2.0L
multiply both sides by 2.0L
moles solute = 1.5 moles KCl
so you need 1.5 moles KCl to prepare the solution
447 g KCl
Molarity is moles of solute
liters of solution.
3.00M = x mol
2.00 L
6 mol KCl converted to grams (molar mass = 74.5 g/mol) is 447 g KCl, with sig figs.
(X volume )(2.00M KCl ) = (500 ml )(0.100M KCl )
= 25 milliliters
moles of KCl=molarity of KCl solution * volume of KCl solution=4.0*1.00=4.0 moles
The answer is 66,18 mL.
1.0
25.0 mL
1.0 moles
4.0 moles
4 gram molecular weights (moles): However many grams four moles* of the solute is. * Hint: four moles of sodium chloride weighs less than four moles of sucrose.
Molarity = moles of solute/volume of solution. 1 liter = 1000 millilitetrs 3.00M = X Moles/1000ml = 3000 millimoles, or 3 moles NaCl 3 moles NaCl (58.44g NaCl/1mol NaCl ) = 175.32 grams needed. About 4/10 of a pound of salt.
This is a chemical calculation. there are 3.267 moles in this solution.
237.5 mL (200mL if you are keeping track of significant figures). Molarity is moles/liters. To make 900mL of a 2M solution, you need 1.8 moles of solute. There are 1.8 moles of solute in 237.5 mL of 8M solution.
moles KCl = ( M solution ) ( V solution in L )moles KCl = ( 2.2 mol KCl / L solution ) ( 0.635 L of solution )moles KCl = 1.397 moles KCl
Molarity = moles of solute/liters of solution or, for our purposes moles of solute = liters of solution * Molarity moles of AgNO3 = 0,50 liters * 4.0 M = 2.0 moles of AgNO3 needed --------------------------------------
10
Concentration of NaOH = 0.025 M = 0.025 Moles per Litre of SolutionVolume of Solution required = 5.00LWe can say therefore that:Number of Moles of NaOH needed to prepare the solution= Concentration of NaOH * Volume of Solution requiredTherefore:Number of Moles of NaOH needed to prepare the solution= 0.025M * 5.00L= 0.125molesFrom this we can say that 0.125 moles of NaOH are needed to prepare a 5.00 L solution with a concentration of 0.025M of NaOH.
4 moles or 160 g NaOH is required for one litre solution.
You need 2,4 g NaOH (0,06 moles).
500ml = 500cm3 = 0.5dm3 0.250M = 0.250mol/dm3 number of moles = molarity x volume number of moles = 0.250mol/dm3 x 0.5dm3 = 0.125mol 0.125mol of NaCl is needed to prepare the required solution.
7.18
0.125 Molar solution! Molarity = moles of solute/Liters of solution Algebraically manipulated, Moles of copper sulfate = 2.50 Liters * 0.125 M = 0.313 moles copper sulfate needed ===========================
599.6
Molarity = moles of solute/Liters of solution 0.75 M KCl = moles KCl/2.25 Liters = 1.6875 moles KCl (74.55 grams/1 mole KCl) = 126 grams of KCl needed
5mM = 0.005 moles 100 mL = 0.1 Liters Molarity = moles of solute/Liters of solution 0.005 M EDTA = X moles/0.1 Liters = 0.0005 moles EDTA =_____________ Now, look up the molecular formula for EDTA and find how many grams needed to add to your 100 mL.
4 gram molecular weights (moles): However many grams four moles* of the solute is. * Hint: four moles of sodium chloride weighs less than four moles of sucrose.