What is the molarity of 1.70 of silver trioxonitrate(v) in 500cm
Your school SUBJECT appears to be CHEMISTRY.
figure the number of moles of the silver compound.
Since 500cm^3 is 0.5 liters, the molarity is twice the # of moles.
To calculate the molarity of a solution, you need to know the moles of solute (silver trioxonitrate(V)) and the volume of the solution (in liters). Here's how you can find the molarity:
1. Convert the volume of the solution from cm³ to liters. Since 1 cm³ is equal to 0.001 L, divide the volume by 1000.
In this case, 500 cm³ is equal to 500/1000 = 0.5 L.
2. Determine the number of moles of silver trioxonitrate(V) (AgNO₃). The given mass of AgNO₃ (1.70) is in grams, and to find moles, you need to divide the mass by the molar mass of AgNO₃.
The molar mass of AgNO₃ can be calculated by summing the atomic masses of silver (Ag), nitrogen (N), and oxygen (O) in the compound:
AgNO₃ = (1 * Ag) + (1 * N) + (3 * O)
= (1 * 107.8682 g/mol) + (1 * 14.0067 g/mol) + (3 * 15.9994 g/mol)
= 169.87 g/mol
To convert the mass of AgNO₃ to moles, divide the given mass by the molar mass:
Moles of AgNO₃ = 1.70 g / 169.87 g/mol
3. Substitute the calculated values into the molarity formula: Molarity (M) = moles/volume
Molarity = Moles of AgNO₃ / Volume of solution (in liters)
Molarity = (1.70 g / 169.87 g/mol) / 0.5 L
4. Calculate the molarity using the equation and round off the answer to an appropriate number of significant figures.
The final result will be the molarity of silver trioxonitrate(V) in the solution.