1. Calculate the mass of each compound required to make 25mL of the following solutions:
(a) 0.10 M Ni(NO3)2 • 6H2O
(b) 1.0 M NaClO4 • H2O
(c) 0.11 M trien (C6H18N4)
2. Calculate the concentrations of Ni2+ and trien in a solution prepared by mixing equal volumes of solutions 2(a) and 2(c).
***Note: Ni(trien) = nickel(II) triethylenetetramine
I don't know how to start this problem or what to do with the "• H2O" on the end. Do I include that in my calculations? More detailed explanation the better, thanks!
1a. mols needed = M x L
Then mols = grams/molar mass. You know molar mass and mols, solve for grams.
Same concepts for 2 but not worked same way.
So for part 2 I assume I add he volumes for 50mL? And then do I find just the moles of Ni2+? So one mole of Ni per 2 moles of NO3?
I just don't understand how to calculate the concentration of a single element using two different compounds.
To calculate the mass of each compound required to make the given solutions, you need to use the concentration (Molarity), volume, and molar mass of the compounds. The "• H2O" in the compound notation refers to the water of hydration, which means water molecules are associated with the compound.
Here's how you can calculate the mass of each compound for the given solutions:
(a) 0.10 M Ni(NO3)2 • 6H2O:
First, let's determine the molar mass of Ni(NO3)2 • 6H2O. It consists of one nickel atom (Ni), two nitrate ions (NO3), and six water molecules. The molar masses are:
- Nickel (Ni): Atomic mass of Ni = 58.69 g/mol
- Nitrate (NO3): Atomic mass of N = 14.01 g/mol, Atomic mass of O = 16.00 g/mol (There are three of them in the formula)
- Water (H2O): Atomic mass of H = 1.01 g/mol, Atomic mass of O = 16.00 g/mol (There are six of them in the formula)
Now, calculate the molar mass of Ni(NO3)2 • 6H2O:
Molar mass = (1 * Nickel mass) + (2 * Nitrate mass) + (6 * Water mass)
Using the atomic masses mentioned above and performing the calculations, you will find that the molar mass of Ni(NO3)2 • 6H2O is approximately 290.81 g/mol.
Next, calculate the mass (grams) of Ni(NO3)2 • 6H2O needed to make a 25 mL solution with a concentration of 0.10 M:
Mass (g) = Molarity (mol/L) * Volume (L) * Molar mass (g/mol)
Substituting the values into the equation, you get:
Mass (g) = 0.10 mol/L * 0.025 L * 290.81 g/mol
Performing the calculations, you will find that the mass of Ni(NO3)2 • 6H2O required is approximately 0.727 g.
(b) 1.0 M NaClO4 • H2O:
In this case, NaClO4 • H2O consists of one sodium ion (Na), one perchlorate ion (ClO4), and one water molecule. Determine the molar masses of NaClO4 • H2O, similar to the previous example.
Now, calculate the mass of NaClO4 • H2O needed to make a 25 mL solution with a concentration of 1.0 M:
Mass (g) = Molarity (mol/L) * Volume (L) * Molar mass (g/mol)
Performing the calculations, you will find the mass of NaClO4 • H2O required.
(c) 0.11 M trien (C6H18N4):
Trien (C6H18N4) is a simple compound with a well-defined formula. Determine its molar mass using the atomic masses of carbon (C), hydrogen (H), and nitrogen (N) atoms.
Calculate the mass of trien needed to make a 25 mL solution with a concentration of 0.11 M:
Mass (g) = Molarity (mol/L) * Volume (L) * Molar mass (g/mol)
Performing the calculations, you will find the mass of trien required.
To calculate the concentrations of Ni2+ and trien in a solution prepared by mixing equal volumes of solutions 2(a) and 2(c), you need to consider the stoichiometry of the reactions involved.
However, since you haven't provided the solutions 2(a) and 2(c), it is not possible to give you a detailed explanation or calculation for the concentrations of Ni2+ and trien. If you provide the necessary information, I can assist you further.