The molecular weight of NaCl is 58.44 g/mol.
To prepare 1M NaCl solution in 100mL volume, we need 58.44 g/L or 5.844 g/100mL.
Therefore, 100mL of 1M NaCl solution requires 5.844 grams of NaCl.
How many grams of NaCL are required to prepare 100ML of solution of 1M NaCl?
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To understand the answer in more detail, let's break down the question and the calculations involved.
The question is asking how many grams of NaCl are required to prepare 100 mL of a solution with a concentration of 1M NaCl. To answer this question, we need to know the definition of molarity.
Molarity is defined as the number of moles of a solute dissolved in one liter of a solution. In this case, we want to prepare a 1M solution of NaCl in a volume of 100 mL, which is equivalent to 0.1 L.
To find out how many moles of NaCl are needed for a 1M solution, we need to know the molar mass of NaCl, which is the sum of the atomic masses of sodium and chlorine. Sodium has a molar mass of 22.99 g/mol, and chlorine has a molar mass of 35.45 g/mol. Therefore, the molar mass of NaCl is:
Molar mass of NaCl = 22.99 g/mol + 35.45 g/mol = 58.44 g/mol
Now we can use the molar mass of NaCl to calculate the amount of NaCl we need for a 1M solution in 0.1 L (100 mL) of water. The equation to calculate the number of moles of solute is:
moles of solute = molarity x volume (in liters)
Since we want a 1M solution in 0.1 L (100 mL) of water, we have:
moles of NaCl = 1 mol/L x 0.1 L = 0.1 mol NaCl
Finally, we can use Avogadro's number (6.02 x 10^23) to convert moles to number of NaCl molecules or atoms, or we can use the molar mass of NaCl to convert moles to grams:
mass of NaCl = moles of NaCl x molar mass of NaCl
mass of NaCl = 0.1 mol x 58.44 g/mol = 5.844 g
Therefore, 100 mL of a 1M NaCl solution requires 5.844 grams of NaCl.
The question is asking how many grams of NaCl are required to prepare 100 mL of a solution with a concentration of 1M NaCl. To answer this question, we need to know the definition of molarity.
Molarity is defined as the number of moles of a solute dissolved in one liter of a solution. In this case, we want to prepare a 1M solution of NaCl in a volume of 100 mL, which is equivalent to 0.1 L.
To find out how many moles of NaCl are needed for a 1M solution, we need to know the molar mass of NaCl, which is the sum of the atomic masses of sodium and chlorine. Sodium has a molar mass of 22.99 g/mol, and chlorine has a molar mass of 35.45 g/mol. Therefore, the molar mass of NaCl is:
Molar mass of NaCl = 22.99 g/mol + 35.45 g/mol = 58.44 g/mol
Now we can use the molar mass of NaCl to calculate the amount of NaCl we need for a 1M solution in 0.1 L (100 mL) of water. The equation to calculate the number of moles of solute is:
moles of solute = molarity x volume (in liters)
Since we want a 1M solution in 0.1 L (100 mL) of water, we have:
moles of NaCl = 1 mol/L x 0.1 L = 0.1 mol NaCl
Finally, we can use Avogadro's number (6.02 x 10^23) to convert moles to number of NaCl molecules or atoms, or we can use the molar mass of NaCl to convert moles to grams:
mass of NaCl = moles of NaCl x molar mass of NaCl
mass of NaCl = 0.1 mol x 58.44 g/mol = 5.844 g
Therefore, 100 mL of a 1M NaCl solution requires 5.844 grams of NaCl.
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