Am I doing this right?
Find the concentration of the phosphate ion. 1.00 mL 210 micro molar. DI water added to 25 ml line.
1.00 mL phosphate solution * 1L/1000mL * 210 mol phosphate solution/1L solution * 1.0 *10^-6 mol/ 1 micromol * 1 mol PO4 3- / 1 mol solution = 2.1*10^-7
Then divide by .025 L = 8.40 * 10^-6
you diluted a 210 μM solution to 1/25 of its original
210 / 25 = 8.4
looks good
210e-6 molar of what? Phosophate ion?
seems to me if it 210e^-6 M, and you dilute it 25 times , then it is diluted 25 times.
or new concentration is 210e-6/25=8.40 * 10^-6 M
Thanks!
To determine the concentration of the phosphate ion, you followed the correct steps. Here's a breakdown of the calculations:
1. You started with 1.00 mL of a 210 micro molar phosphate solution.
2. To convert mL to L, you multiplied by the conversion factor 1 L / 1000 mL.
3. Next, you multiplied by the molarity of the phosphate solution, 210 mol phosphate solution / 1 L solution.
4. Since the concentration was given in micro molar (μM), you multiplied by the conversion factor 1.0 * 10^(-6) mol / 1 μmol to convert to moles.
5. Finally, to determine the concentration of the phosphate ion, you multiplied by the ratio of 1 mol PO4^(3-) (phosphate ion) to 1 mol of the solution.
By following these steps, you derived a concentration of 2.1 * 10^(-7) mol phosphate ion.
To calculate the final concentration after adding DI water to the 25 mL line, you divide the 2.1 * 10^(-7) mol by the final volume of the solution, which is 0.025 L. This gives you a final concentration of 8.40 * 10^(-6) mol phosphate ion.