Dissolve 74,5513 g dried KCl in 1 L distilled water, at 20 oC.
The answer is of course 0,9 M.
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
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
Weigh 22.35 grams of KCl and Dissolve in 100 mL of Distilled Water
To prepare a 2 M solution of KCl in 1 liter of water, you would need to dissolve 149.5 grams of KCl. This is because the molar mass of KCl is approximately 74.5 g/mol, and 2 moles of KCl are needed to prepare a 2 M solution in 1 liter of water.
To make a 3 M solution of KCl, you would need to dissolve 149.5 grams of KCl (potassium chloride) in enough water to make 1 liter of solution. Weigh out the desired amount of KCl, add it to a suitable container, and then add water while stirring until the KCl is completely dissolved.
To calculate the volume needed, you can use the formula for dilution: M1V1 = M2V2. You have M1 = 12.0 M, V1 (unknown), M2 = 0.50 M, and V2 = 300.0 ml. By rearranging the formula and solving for V1, you'll find that V1 = 2.5 ml of 12.0 M KCl solution is required to make 300.0 ml of 0.50 M KCl 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!
To make a 1.0 M solution of KCl in 500 ml, you would need to weigh out 74.55 g of KCl (molar mass of KCl is 74.55 g/mol) and dissolve it in enough water to make a final volume of 500 ml. Remember to use a volumetric flask to accurately measure the final volume.
The answer is of course 0,9 M.
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 ------------------
A volumetric flask or beaker would be suitable for making a 1.0 M KCl solution. Make sure to measure accurately to achieve the desired concentration.
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. Identify (a) through (d) as reactants or products. Type your answers in the spaces provided: (a) (b) (c) (d) KOH + HCl KCl + H2O
To calculate the grams of KCl needed, first calculate the moles of KCl required using the molarity formula. Then, convert moles to grams using the molar mass of KCl, which is approximately 74.55 g/mol.
The cell constant is the ratio of the distance between the electrodes to the cross-sectional area of the cell. It is typically determined experimentally and given in units of cm^-1. For a 0.1 M KCl solution, the cell constant could be around 1 cm^-1, while for a 0.01 M KCl solution, the cell constant could be around 10 cm^-1.