# chemistry

posted by .

Calculate the volume of a 9.00 M HNO3 stock solution that must be used to prepare 450 mL 0f a 1.80 M HNO3 solution.

• chemistry -

M x V = M x V (good for dilution problems only).

• chemistry -

so which ones do i times together?

• chemistry -

molarity of concd HNO3 x mL concd HNO3 = molarity of the diluted solution x mL of the diluted solution.

• chemistry -

so is just 9.00x 450x1.80??

• chemistry -

9.00 x 450x 1.80?

• chemistry -

Where is the equal sign?
I would do it this way.
9.00 M x ??mL = 1.80 M x 450 mL
and solve for ?? mL.
Isn't that what my instructions said?
M concd soln x mL concn soln = M dilute soln x mL dilute soln.

• chemistry -

9.00x?mL=810

how do i find the missing number

• chemistry -

You solve for ? mL. This is an ordinary equation.
9.00 x unknown mL = 810.
Solve for unknown mL.

• chemistry -

ok so to find it...do i subtract them..or divide?

• chemistry -

You divide. It has taken me most of the night but I think I know what your problem is. It isn't chemistry. It is arithmetic and algebra. You apparently don't know how to solve an equation.
When we had pH + pOH = 14 and we substituted to give
9.21 + pOH = 14, I had to tell you that pOH = 14 - 9.21 and you obtained the correct answer of 4.79.
For this problem, we have 9.00X = 810.
You solve for the unknown by
X = 810/9.00 = 90; therefore, you take 90 mL of the concd HNO3 (which is 9.00 M), make the total volume to 450 mL, and you end up with 450 mL of 1.80 M HNO3. I recommend that you find a tutor who can help you with algebraic manipulations.

## Similar Questions

1. ### Chemistry

You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3?
2. ### Chemistry

You wish to prepare 0.18 M HNO3 from a stock solution of nitric acid that is 18.9 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.18 M HNO3?
3. ### chemistry

To what volume should you dilute 48mL of a 13M stock HNO3 solution to obtain a 0.122 HNO3 solution?
4. ### CHEMISTRY

HOW YOU PREPARE 30.0ML OF 0.800M HNO3 FROM A STOCK SOLUTION OF 4.OOM HNO3?
5. ### Chemistry

1. calculate the volume of concentrated HNO3 (68%)that is needed to prepare stock solution 0.25M in 1000mL volumetric flask. (density HNO3 = 1.513 g/cm^3) 2. from above stock solution, determine volume needed to dilute to 500mL volumetric …
6. ### Chemistry

If you dilute 14.0mL of the stock solution to a final volume of 0.350L , what will be the concentration of the diluted solution?
7. ### CHEMISTRY !!! HELP !

Calculate the pH of the solution after the addition of the following amounts of 0.0617 M HNO3 to a 70.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. 1)Volume of HNO3 equal to the equivalence point 2)89.5mL of …
8. ### General Chemistry

An experiment calls for you to use 100 mL of 0.65 M HNO3 solution. All you have available is a bottle of 2.7 M HNO3. How many milliliters of the 2.7 M HNO3 solution do you need to prepare the desired solution?
9. ### chemistry

A stock solution of HNO3 is prepared and found to contain 11.1 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.
10. ### Chemistry

An 8 Molar (aqueous) solution contains H2O and HNO3. The solution has an S.G. of 1.24 at 25oC. HNO3 is a strong acid that completely dissociates in water. a) Calculate the mass of I Litre of solution. b) Calculate the mass concentration …

More Similar Questions