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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
How many moles of KCl are contained in 1.7L of a 0.83M KCl solution?
moles KCL = ( M solution ) ( L of solution )moles KCl = ( 0.83 mol KCl / L ) ( 1.7 L ) = 1.41 moles 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 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 ------------------
What is the molarity of a solution that contains 345 moles KCL in 8.6 L solution?
The molarity of the solution is 40.1 M. This is calculated by dividing the moles of solute (345 mol KCl) by the volume of solution in liters (8.6 L).
When 5 grams of KCl are dissolved in 50. grams of water at 25C the resulting mixture can be described as?
This is a solution of 10 g KCl/100 g water.
50 g of potassium chloride (KCl) are added to 100 mL of water. All but 10 g of the KCl dissolves. Which equilibrium situation becomes established in the resulting solution?
The remaining 10 g of KCl forms a saturated solution in water, meaning the solution is in dynamic equilibrium with solid KCl dissolving and KCl ions re-crystallizing at the same rate. The resulting solution will contain both dissolved K+ and Cl- ions in equilibrium with undissolved KCl crystals.
What mass of KCl would be needed to form a saturated solution if the KCl was dissolved in 200 g of water at 80 C?
The solubility of KCl in water at 80°C is approximately 380 g/L. To form a saturated solution, you would need to dissolve 380 g of KCl in 1 L (1000 g) of water. Since you are using 200 g of water, you would need 76 g of KCl to form a saturated solution.
What type of solution is it if 25g KCl are dissolved in 100g of water at 30 degrees celsius?
This would be considered a saturated solution if all 25g of KCl are completely dissolved in the 100g of water at 30 degrees Celsius.
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
Why saturated KCL in DNA extraction is used?
Saturated KCl precipitation is often used in DNA extraction for molluscan taxa. Molluscs produce a polysaccharide rich mucus that interferes with the reagents involved in DNA extraction. The KCl saturated solution is used right after the digestion step: about 1/4th of the volume of the digestion solution is added to the sample. Samples are then centrifugated at 14rpm for 15 minutes. The pellet formed will contain the polysaccharides and non digested tissue. The supernatant is extracted from the tube and used in the next steps of the DNA extraction.
What colour is KCl solution?
A potassium chloride (KCl) solution is colorless.
How many moles of KCl are contained in 1.7L of a 0.83M KCl solution?
moles KCL = ( M solution ) ( L of solution )moles KCl = ( 0.83 mol KCl / L ) ( 1.7 L ) = 1.41 moles KCl
How much KCL is required for 500mM KCL solution?
To prepare a 500mM KCl solution, you would need to dissolve 74.55 grams of KCl in enough solvent to make 1 liter of solution.
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 volume of 0.060 M KCl solution contains 2.39g of KCl?
To find the volume of the solution, first calculate the number of moles of KCl in 2.39g using its molar mass (74.55 g/mol). Then, use the molarity equation (Molarity = moles of solute / volume of solution in liters) to find the volume of the solution.
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 ------------------
