what mass of sodium phosphate is required to make 250mL of 0.10mol/L solution?
.1M=XXX grams/molmassNa3PO4*.25
solve for xxxx
how do i solve for XXXX
algebra
xxx= .1*molmassNa3PO4*.25
okay so if the molar mass of Na3PO4 is 164. a multiply that by 0.1 and then multiply that by o.25 ??
To calculate the mass of sodium phosphate required, we need to use the equation:
moles = concentration (mol/L) × volume (L)
First, let's write down the given values:
- Concentration (C) = 0.10 mol/L
- Volume (V) = 250 mL = 0.250 L
Now we can substitute these values into the equation:
moles = 0.10 mol/L × 0.250 L
By multiplying these values together, we find:
moles = 0.025 mol
To determine the mass of sodium phosphate, we need to know its molar mass, which is the mass of one mole of the compound. The molar mass of sodium phosphate (Na3PO4) can be calculated from the atomic masses of each element:
Na (sodium) = 22.99 g/mol
P (phosphorus) = 30.97 g/mol
O (oxygen) = 16.00 g/mol
So, the molar mass of Na3PO4 is:
3(Na) + 1(P) + 4(O)
= 3(22.99) + 30.97 + 4(16.00)
= 68.97 + 30.97 + 64.00
= 163.94 g/mol
To find the mass of sodium phosphate, we can use the equation:
mass (g) = moles × molar mass
Substituting the values, we get:
mass (g) = 0.025 mol × 163.94 g/mol
By multiplying these values, we find:
mass (g) = 4.0985 g
Therefore, to make a 250 mL solution with a concentration of 0.10 mol/L of sodium phosphate, you will need approximately 4.1 grams of sodium phosphate.