How many grams of NaCL are required to prepare 100ML of solution of 1M NaCl?

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.

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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.

To determine the number of grams of NaCl required to prepare a 1M NaCl solution in 100 mL, you need to know the molar mass of NaCl.

The molar mass of NaCl is the sum of the atomic masses of sodium (Na) and chlorine (Cl). One sodium atom has a molar mass of approximately 22.99 grams, and one chlorine atom has a molar mass of approximately 35.45 grams. Therefore, the molar mass of NaCl is:

Molar mass of NaCl = Molar mass of Na + Molar mass of Cl
= 22.99 g/mol + 35.45 g/mol
= 58.44 g/mol

Now, we need to calculate the number of moles of NaCl required to prepare a 1M solution. The molarity (M) is defined as the number of moles of solute (in this case, NaCl) per liter of solution. Since you want to prepare a 100 mL solution, you need to convert the volume to liters.

1 L = 1000 mL

So, 100 mL is equivalent to 0.1 L.

Using the equation for molarity, we have:

Molarity (M) = Moles of solute / Volume of solution in liters

Rearranging the equation, we get:

Moles of solute = Molarity (M) * Volume of solution in liters

Substituting the given values:

Moles of solute = 1 mol/L * 0.1 L
= 0.1 mol

Finally, to find the grams of NaCl required, we can use the equation:

Grams = Moles of solute * Molar mass

Plugging in the values:

Grams = 0.1 mol * 58.44 g/mol
= 5.844 grams

Therefore, you would need approximately 5.844 grams of NaCl to prepare a 100 mL solution of 1M NaCl.

To determine the number of grams of NaCl required to prepare a 100 mL solution of 1M NaCl, you need to know the molar mass of NaCl and use the formula:

Number of moles = Volume (in liters) × Molarity

1. First, calculate the number of moles of NaCl required using the given molarity and volume.
Number of moles NaCl = 1 mol/L × 0.1 L

2. Convert the number of moles of NaCl to grams using its molar mass. The molar mass of NaCl is approximately 58.44 g/mol.
Mass of NaCl = Number of moles × Molar mass
= 0.1 mol × 58.44 g/mol

Therefore, to prepare a 100 mL solution of 1M NaCl, you would need approximately 5.84 grams of NaCl.