Dissolve 74.55g of KCL in some water then volume it up to 1 liter.
Dissolve 53 g sodium carbonate in 1 kg of water.
Dissolve 95,211 g anhydrous chloride in 1kg distilled water.
For 1 N CaCl2 ≡ 55.5 gms in 1 lit.
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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
1 meter
0.67 M
I'll straightly go to the equation. KCL molar mass is 74.5513 g/mol. To prepare 0.02 M KCL solution, *0.02 M is also known as 0.02 mol/litre. 74.5513 g/mol x 0.02 mol/litre x 1 litre = 1.4910 g *note that in the equation we can cancel the mol and litre leave out the gram alone. So we need only 1.4910 g of KCL in 1 litre. You can change the volume, depend on your convenience but must in litre unit.
MW 74.5, 1M solution requires 74.5g in 1L, 5M solution requires 74.5x5 = 372.5g in 1 L. You would need 93.1g KCL to make 250mL 5M solution
Dissolve 566.25g of KCl in 3L.
The answer is 6,71 g dried KCl.
Weigh 22.35 grams of KCl and Dissolve in 100 mL of Distilled Water
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
MW KCl = 74.6 g/mol2.39 gKCl * (1 mol KCL/74.6 g KCl)*(1 L solution/0.06 mol KCL) = 0.534 L
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!
I'll go straight to the equation, to prepare 0.5 M of KCl in 383 ml, simply calculate it this way, *Molar mass of KCl is 74.5513 g/mol *0.5 M is also known as 0.5 mol/Litre 74.5513 g/mol x 0.5 mol/litre x 0.383 Litre = 14.2766 g So, you need 14.2766 g of KCl to prepare 0.5 M in 383 ml solution.
1 meter
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
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
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 ------------------
moles KCL = ( M solution ) ( L of solution )moles KCl = ( 0.83 mol KCl / L ) ( 1.7 L ) = 1.41 moles KCl