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
Molar mass of KCl = 39 g/mol (K) + 35.5 g/mol (Cl) = 74.5 g/mol. A 0.5 M solution is required (0.5 mol/L or 0.5 moles per litre). 0.5 moles of KCl is 0.5 mol x 74.5 g/mol = 37.25 g. Dissolving this 37.25 g of KCl in a litre of water would give a 0.5 M solution. If 1 L or 1000 mL of 0.5 M solution contains 0.5 moles then 1 mL of the same concentration solution would contain 0.5/1000 moles and 250 mL would contain 250 x 0.5/1000 moles = 0.125 moles. 0.125 moles of KCl is 0.125 mol x 74.5 g/mol = 9.31 g.
2.77 g KCl * x moles KCl/ 74.5 g/mol 0.0372 mol KCl * 1 mol K/ 1 mol Cl = 0.0372 mol K 0.0372 mol K * 6.02*10^23 2.24*10^22 atoms K
1. 4.8 g of KCL 2. 2.1 g of KCL
Minimum 102,6 g of KCl.
You have2KClO3 ==> 2KCl + 3O2 as the balanced equation 25 g KClO3 x 1 mole/123 g = 0.20 moles moles KCl formed = 0.20 moles KClO3 x 2 moles KCl/2 moles KClO3 = 0.20 moles KCl formed grams KCl = 0.20 moles x 74.5 g/mole = 14.9 g = 15 grams of KCl formed
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
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
For this you need the atomic (molecular) mass of KCl. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. KCl= 74.6 grams50.0 grams KCl / (74.6 grams) = .670 moles KCl
Molar mass of KCl = 39 g/mol (K) + 35.5 g/mol (Cl) = 74.5 g/mol. A 0.5 M solution is required (0.5 mol/L or 0.5 moles per litre). 0.5 moles of KCl is 0.5 mol x 74.5 g/mol = 37.25 g. Dissolving this 37.25 g of KCl in a litre of water would give a 0.5 M solution. If 1 L or 1000 mL of 0.5 M solution contains 0.5 moles then 1 mL of the same concentration solution would contain 0.5/1000 moles and 250 mL would contain 250 x 0.5/1000 moles = 0.125 moles. 0.125 moles of KCl is 0.125 mol x 74.5 g/mol = 9.31 g.
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 ------------------
2.77 g KCl * x moles KCl/ 74.5 g/mol 0.0372 mol KCl * 1 mol K/ 1 mol Cl = 0.0372 mol K 0.0372 mol K * 6.02*10^23 2.24*10^22 atoms K
0.1 N KCl is the same as 0.1 M KCl. This requires one to dissolve 0.1 moles per each liter of solution. The molar mass of KCl is 74.6 g/mol. So 0.1 moles = 7.46 gDissolve 7.46 g KCl in enough water to make 1 liter (1000 ml)Dissolve 3.73 g KCl in enough water to make 0.5 liter (500 ml)Dissolve 0.746 g KCl in enough water to make 0.1 liter (100 ml)etc., etc.
1. 4.8 g of KCL 2. 2.1 g of KCL
moles of KCl = 100 g x 1 mole/74.5 g = 1.34 molesvolume = 250 ml = 0.25 L molarity = moles/liter = 1.34 moles/0.25 L = 5.37 M Since KCl dissociates completely into K+ and Cl-, you have 5.37 M of each = total of 10.74 osmolar
This mass is 631,75 g K2O.
The answer is 6,71 g dried KCl.