What is the concentration of a solution formed by dissolving 10.0g of ammonium acetate in enough water to form 150.0mL of solution?

Could someone please explain and show me how to do this? I have the answer= .865M
But I am not sure exactly how?!

What's the definition?

M = mols/L solution.
How many mols do you have? 10.0/molar mass NH4C2H3O2 = ?
How many L do you have? 0.150

Done?

To calculate the concentration of a solution, you need to know the amount of solute (in grams) and the volume of the solution (in liters). In this case, you know that you have dissolved 10.0g of ammonium acetate and that the solution has a volume of 150.0mL.

To calculate the concentration of the solution, you need to convert the volume from milliliters (mL) to liters (L). Since 1L is equal to 1000mL, you divide the volume by 1000 to convert it to liters:

Volume = 150.0mL ÷ 1000 = 0.150L

Now you have the amount of solute (10.0g) and the volume of the solution (0.150 L), so you can use the formula for concentration (Molarity):

Concentration (M) = mol ÷ L

To find the number of moles, you need to know the molar mass of ammonium acetate. The molar mass is calculated by adding up the atomic masses of all the atoms in the compound.

The molecular formula of ammonium acetate is NH4C2H3O2, which consists of 4 hydrogen atoms (each with an atomic mass of 1 g/mol), 1 nitrogen atom (with an atomic mass of 14 g/mol), 2 carbon atoms (each with an atomic mass of 12 g/mol), and 3 oxygen atoms (each with an atomic mass of 16 g/mol).

Molar mass of NH4C2H3O2 = (4 * 1) + (1 * 14) + (2 * 12) + (3 * 16)
= 4 + 14 + 24 + 48
= 90 g/mol

Now, you can convert the mass of solute (10.0g) to moles by dividing it by the molar mass:

Moles of NH4C2H3O2 = 10.0g ÷ 90 g/mol = 0.1111 mol

Finally, you can calculate the concentration by dividing the number of moles by the volume in liters:

Concentration = 0.1111 mol NH4C2H3O2 ÷ 0.150 L = 0.7417 M

Therefore, the concentration of the solution formed by dissolving 10.0g of ammonium acetate in enough water to form 150.0mL of solution is approximately 0.7417 M.

To calculate the concentration of a solution, you need to know the amount of solute (in this case, ammonium acetate) and the volume of the solution.

The concentration of a solution is defined as the amount of solute per unit volume of the solution. It is usually expressed in moles per liter (M).

In this case, you are given the mass of ammonium acetate (10.0 g) and the volume of the solution (150.0 mL). To calculate the concentration, you need to follow these steps:

1. Convert the volume of the solution to liters. Since 1 L is equal to 1000 mL, you can convert 150.0 mL to liters by dividing by 1000:
Volume (in liters) = 150.0 mL / 1000 = 0.150 L

2. Convert the mass of ammonium acetate to moles. To do this, you need to know the molar mass of ammonium acetate, which is the sum of the atomic masses of all the elements in the compound. The formula for ammonium acetate (NH4C2H3O2) consists of one nitrogen (N), five hydrogens (H), two carbons (C), and three oxygens (O).

- Atomic masses:
N = 14.01 g/mol
H = 1.01 g/mol
C = 12.01 g/mol
O = 16.00 g/mol

- Molar mass of ammonium acetate:
Molar mass = (1 * 14.01) + (5 * 1.01) + (2 * 12.01) + (3 * 16.00)

- Calculate the molar mass:
Molar mass = 77.08 g/mol

Now, you can convert the mass of ammonium acetate to moles using its molar mass:
Moles of ammonium acetate = Mass / Molar mass = 10.0 g / 77.08 g/mol

3. Calculate the concentration by dividing the moles of ammonium acetate by the volume of the solution:
Concentration (in M) = Moles / Volume (in liters) = (10.0 g / 77.08 g/mol) / 0.150 L

Simplify the expression:
Concentration = 0.1296 mol/ L

Now, round the result to the appropriate significant figures:
Concentration = 0.130 M

Therefore, the concentration of the solution formed by dissolving 10.0 g of ammonium acetate in enough water to make 150.0 mL of solution is approximately 0.130 M.