how does the concentration of a 100 mL solution of 10 g of Cu(OH)2 equals to .02M?
To determine the concentration of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters). In this case, you are given that you have 10 g of Cu(OH)2 dissolved in 100 mL of solution.
First, convert the mass of Cu(OH)2 into moles. The molar mass of Cu(OH)2 can be calculated by adding the atomic masses of Cu, O, and H:
Cu: 63.55 g/mol
O: 16.00 g/mol (there are two oxygen atoms)
H: 1.01 g/mol (there are two hydrogen atoms)
Molar mass of Cu(OH)2 = (63.55 g/mol) + (2 × 16.00 g/mol) + (2 × 1.01 g/mol) = 97.55 g/mol
Now, calculate the number of moles of Cu(OH)2:
moles of Cu(OH)2 = mass / molar mass = 10 g / 97.55 g/mol ≈ 0.1023 mol
Next, convert the volume of the solution from milliliters to liters:
volume of solution = 100 mL = 100/1000 L = 0.1 L
Finally, calculate the concentration (Molarity) of the solution by dividing the moles of Cu(OH)2 by the volume of the solution in liters:
concentration (Molarity) = moles of solute / volume of solution
= 0.1023 mol / 0.1 L = 1.023 M
Therefore, the concentration of the 100 mL solution of 10 g of Cu(OH)2 is approximately 1.023 M (not 0.02 M).
To determine the concentration of a solution, you need to know the moles of solute (Cu(OH)2 in this case) and the volume of the solution.
Step 1: Calculate the moles of Cu(OH)2 using its molar mass.
The molar mass of Cu(OH)2 can be calculated by adding up the atomic masses of its constituent elements:
Molar mass of Cu(OH)2 = (atomic mass of Cu) + (2 x atomic mass of O) + (2 x atomic mass of H)
= (63.55 g/mol) + (2 x 16.00 g/mol) + (2 x 1.01 g/mol)
= 63.55 g/mol + 32.00 g/mol + 2.02 g/mol
= 97.57 g/mol
The moles of Cu(OH)2 can be calculated using the given mass and molar mass using the formula:
Moles = Mass / Molar mass
= 10 g / 97.57 g/mol
≈ 0.10244 mol
Step 2: Convert the volume of the solution to liters.
The given volume is 100 mL, which needs to be converted to liters by dividing by 1000:
Volume = 100 mL / 1000
= 0.1 L
Step 3: Calculate the concentration (molarity) of the solution using the formula:
Concentration (molarity) = Moles / Volume
= 0.10244 mol / 0.1 L
= 1.0244 M
Therefore, the concentration of a 100 mL solution containing 10 g of Cu(OH)2 is approximately 1.0244 M, not 0.02 M as mentioned in the question.
To determine the concentration (in moles per liter, or M) of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
In this case, you have a 100 mL solution containing 10 g of Cu(OH)2. The first step is to convert the mass of Cu(OH)2 to moles. To do this, you need to know the molar mass of Cu(OH)2, which can be calculated using the atomic masses of the elements involved.
The molar mass of Cu(OH)2 can be determined by adding the atomic masses of copper (Cu), oxygen (O), and hydrogen (H). According to the periodic table, the atomic masses are approximately:
Cu = 63.55 g/mol
O = 16.00 g/mol (there are two oxygen atoms)
H = 1.01 g/mol (there are two hydrogen atoms)
So, the molar mass of Cu(OH)2 is:
Cu: 63.55 g/mol
O: (16.00 g/mol) x 2 = 32.00 g/mol
H: (1.01 g/mol) x 2 = 2.02 g/mol
Total molar mass of Cu(OH)2 = 63.55 + 32.00 + 2.02 = 97.57 g/mol
Now, you can calculate the number of moles of Cu(OH)2 in the solution using the formula:
moles = mass / molar mass
moles = 10 g / 97.57 g/mol
moles ≈ 0.1024 mol
Next, you need to convert the volume of the solution from milliliters (mL) to liters (L). Since 1 L is equal to 1000 mL, the volume of the solution is:
volume = 100 mL / 1000 mL/L = 0.1 L
Finally, the concentration (in M) is calculated by dividing the number of moles of solute by the volume of the solution:
concentration (M) = moles / volume
concentration (M) = 0.1024 mol / 0.1 L
concentration (M) ≈ 1.024 M
Therefore, the concentration of the 100 mL solution containing 10 g of Cu(OH)2 is approximately 1.024 M, not 0.02 M.