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What is the molarity of the solution containing 5.0 moles of KCl in 2.0 L of solution?
Wiki User
∙ 11y ago
Molarity is moles per litre. So you have to convert volume to a litre. i.e. 0.5x2 is a litre. so you have to do the same to moles. 5x2 is 10 moles. as this is per litre, it is a 10 molar solution.
Wiki User
∙ 10y ago
Wiki User
∙ 15y ago2.00Litres is equal to 2.00dm3 Therefore, molarity = (5.00/2.00) mol/dm3 = 2.5 mol/dm3 = 2500 mol/cm3
Wiki User
∙ 12y agoMolarity = moles/liters
In this instance, simply divide 5.00 by 2.00
Make sure your answer has the correct number of significant figures and you'll come up with 2.50M
Wiki User
∙ 11y agoThe molarity of the given solution is 2.5 mol/L.
Wiki User
∙ 8y agoMolarity is number of moles in solute. So molarity of this is 0.5mol-1.
Wiki User
∙ 7y agoThe molarity is 0,5 M.
Wiki User
∙ 12y agobv
Wiki User
∙ 10y ago2m
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What is the molarity of a solution where 4.00 moles of Potassium Chloride is dissolved in 3.00 L of solution?
The molarity of a solution given by the number of moles divided by the volume it contains. Hence, the molarity of KCl is 4.00/3.00 = 1.33 mol/L.
How many grams of KCl are required to prepare 2.25L of a 0.75m KCl solution?
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
What is the molarity of a solution that contains 202 mol KCl in 7.98 L solution?
Molarity is moles per litre. Therefore if you divide by 7.98 you get it as moles per litre, i.e. molar. 202/7.98 is 25.31 molar.
How many grams of KCl are needed to make 100 ml of a 3.5M solution?
In a 3.4 M solution, there are 3.4 moles per liter. If you want to make 3 liters of solution, you'll need 3 liter * 3.4 moles/liter = 10.2 moles The molar mass of KCl is 39.098 g/mole K + 35.453 g/mole Cl = 74.551 g/mole KCl To get the number of grams, multiply the number of moles by the molar mass: 10.2 moles * 74.551 g/mole KCl = 760.4202 g = 0.760 kg
What is the molarity of a solution that contains 202 mol KCl in 7.98L solution?
Molarity means moles in a litre. So here we divide by moles by 7.98 to get moles in a litre. This gives us 25.3133 molar. This figure is very high (likely to be over saturation level in water), so I'm not sure if your figures are correct.
What is the molarity of a solution that contains .202 mol KCI in 7.98 L of solution?
Molarity = moles of solute/Liters of solution Molarity = 0.202 moles KCl/7.98 Liters = 0.253 M KCl solution ================
What is the molarity of a solution that contains 0.202 moles KCl in 7.98 liters of solution?
The molarity is 0,025.
What is the molarity of a solution made by dissolving 4.88 g of KCl in 423 mL of solution?
Need mole KCl first. 4.88 grams KCl (1 mole KCl/74.55 grams) = 0.06546 moles KCl =======================now, Molarity = moles of solute/Liters of solution ( 423 ml = 0.423 Liters ) Molarity = 0.06546 moles KCl/0.423 Liters = 0.155 M KCl ------------------
How many moles of KCL are present in 50.0ml of a 0.552 M solution?
Molarity = moles of solute/Liters of solution ( 50.0 ml = 0.05 Liters ) 0.552 M KCl = moles/.0.05 liters = 0.0276 moles of KCl
How many moles of KCl are needed to prepare 1.00 L of a 1.0M KCl solution?
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
What is the molarity of a solution that contains 345 moles KCL in 8.6 L solution?
.487 Kl
How many moles of KCl are contained in 121mL of a 1.68M KCl solution?
Molarity is moles of solute per L of solution.moles KCl = ( 1.68 M ) ( 0.121 L ) = ( 1.68 mol/L ) ( 0.121 L )moles KCl = 0.203 moles KCl
What is the molarity of a solution where 4.00 moles of Potassium Chloride is dissolved in 3.00 L of solution?
The molarity of a solution given by the number of moles divided by the volume it contains. Hence, the molarity of KCl is 4.00/3.00 = 1.33 mol/L.
How many grams of KCl are required to prepare 2.25L of a 0.75m KCl solution?
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
What is the molarity of the following solution 1.0 moles of KCl in 500mL of solution?
You need to bring this to a litre. If there is 1 mole in 500ml (using ratio), there will be 2 moles in a litre. So your molarity is 2.
How much 75.66MKCL is required toprepare 1L of solution?
I did not know that you could get a concentration of 75.66 M KCl, but; Molarity = moles of solute/Liters of solution 75.66 M KCl = moles KCl/1 liter = 75.66 moles of KCl 75.66 moles KCl (74.55 grams/1 mole KCl) = 5640 grams KCl that is about 13 pounds of KCl in 1 liter of solution. This is why I think there is something really wrong with this problem!
How many moles of KCl are contained in 0.635L of 2.2M KCl?
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
