What is the mass if solute dissolved in the indicated volume of each of the following solutions?


(b) 4.25 L of 0.450 M KIO4g

(c) 60.0 mL of 0.310 M ZnSO4g


(d) 60.0 mL of 0.310 M Ni(NO3)2g

Molarity=moles/volume=mass/(volume* molmass)

mass=molarity*molmass*volume

I am very confused. I tried several practice problems and am not getting them correct.

Why not post one of them and let us find the error. This way we're running in circles.

To find the mass of solute dissolved in each solution, we need to use the molarity (M) and volume (V) of the solution. The formula to calculate the mass of solute is:

Mass of Solute = Molarity x Volume x Molar Mass

Step-by-step instructions to find the mass of solute for each solution are as follows:

(b) 4.25 L of 0.450 M KIO4:

1. Obtain the molarity (0.450 M) and volume (4.25 L) of the solution.
2. Look up the molar mass of KIO4. The molar mass of K is 39.10 g/mol, I is 126.90 g/mol, and O is 16.00 g/mol.
3. Calculate the mass of KIO4 using the formula: Mass of Solute = Molarity x Volume x Molar Mass.
Mass of KIO4 = 0.450 M x 4.25 L x (39.10 g/mol + 4 x 16.00 g/mol).
Mass of KIO4 = 0.450 M x 4.25 L x (39.10 g/mol + 64.00 g/mol).
Mass of KIO4 = 0.450 M x 4.25 L x 103.10 g/mol.
Mass of KIO4 = 196.45375 g.

Therefore, the mass of solute in 4.25 L of 0.450 M KIO4 is 196.45375 grams.

(c) 60.0 mL of 0.310 M ZnSO4:

1. Convert the volume from milliliters (mL) to liters (L). There are 1000 mL in 1 L, so 60.0 mL is equal to 60.0/1000 L = 0.0600 L.
2. Obtain the molarity (0.310 M) and volume (0.0600 L) of the solution.
3. Look up the molar mass of ZnSO4. The molar mass of Zn is 65.38 g/mol, S is 32.07 g/mol, and O is 16.00 g/mol.
4. Calculate the mass of ZnSO4 using the formula: Mass of Solute = Molarity x Volume x Molar Mass.
Mass of ZnSO4 = 0.310 M x 0.0600 L x (65.38 g/mol + 32.07 g/mol + 4 x 16.00 g/mol).
Mass of ZnSO4 = 0.310 M x 0.0600 L x (65.38 g/mol + 32.07 g/mol + 64.00 g/mol).
Mass of ZnSO4 = 0.310 M x 0.0600 L x 161.45 g/mol.
Mass of ZnSO4 = 3.5889 g.

Therefore, the mass of solute in 60.0 mL of 0.310 M ZnSO4 is 3.5889 grams.

(d) 60.0 mL of 0.310 M Ni(NO3)2:

The process to find the mass of solute in this solution is similar to the calculation in part (c), but using the molar mass of Ni(NO3)2 instead. Calculate the mass of Ni(NO3)2 as follows:

1. Convert the volume from milliliters (mL) to liters (L). There are 1000 mL in 1 L, so 60.0 mL is equal to 60.0/1000 L = 0.0600 L.
2. Obtain the molarity (0.310 M) and volume (0.0600 L) of the solution.
3. Look up the molar mass of Ni(NO3)2. The molar mass of Ni is 58.69 g/mol, N is 14.01 g/mol, and O is 16.00 g/mol.
4. Calculate the mass of Ni(NO3)2 using the formula: Mass of Solute = Molarity x Volume x Molar Mass.
Mass of Ni(NO3)2 = 0.310 M x 0.0600 L x (58.69 g/mol + 2 x 14.01 g/mol + 6 x 16.00 g/mol).
Mass of Ni(NO3)2 = 0.310 M x 0.0600 L x (58.69 g/mol + 28.02 g/mol + 96.00 g/mol).
Mass of Ni(NO3)2 = 0.310 M x 0.0600 L x 182.71 g/mol.
Mass of Ni(NO3)2 = 3.2360 g.

Therefore, the mass of solute in 60.0 mL of 0.310 M Ni(NO3)2 is 3.2360 grams.