1) How do I prepare 2M nitric acid from 65% concentrated nitric acid?
2) How do I prepare 17% ammonia from 25% concentrated ammonia?
Please show calculation steps. Thanks.
I would start the HNO3 by determining the molarity of the HNO3.
density = 1.42 g/mL x 1000 mL = 1420 grams.
It is 69% by mass; therefore, the amount of HNO3 in that 1420 g is 1420 x 0.69 = 979.8 grams. How many moles is that?
979.8/molar mass = about 15.5 M
Then mL x M = mL x M
mL x 15.5 M = 100 mL x M and I just made up the 100 mL number since you don't have a preference for the amount. Whatever volume you want goes in there.
The NH3 problem is done the same way.
Assuming it is w/w as is the case for most acids and conc ammonia, can you show me the steps using 69% HNO3 and 28% ammonia?
I have density of 69% HNO3 as 1.42g/ml & 28% ammonia as 0.88g/ml.
um
why was this made in 2010???
To prepare a specific concentration of a solution from a concentrated solution, you need to use the concept of dilution. Dilution involves adding a solvent (usually water) to the concentrated solution to decrease its concentration. Here's how you can prepare the desired solutions:
1) How to prepare 2M nitric acid from 65% concentrated nitric acid:
Step 1: Determine the volume of the concentrated solution needed to obtain the desired concentration. We'll assume you want to prepare 1 liter (1000mL) of 2M nitric acid.
Step 2: Calculate the moles of nitric acid required for the desired concentration.
Molarity (M) = Moles (mol) / Volume (L)
Using the above equation, rearrange it to solve for the moles of nitric acid:
Moles (mol) = Molarity (M) x Volume (L)
Given:
Molarity (M) = 2M
Volume (L) = 1L
Moles (mol) = 2M x 1L = 2 moles
Step 3: Calculate the volume of the concentrated nitric acid required.
The volume of the concentrated solution can be determined using the equation:
Volume (L) = Moles (mol) / Molarity (M)
Given:
Molarity (M) = 65% = 0.65M
Moles (mol) = 2 mol
Volume (L) = 2 mol / 0.65M = 3.08 L (3080 mL)
You need to take 3.08 liters (3080 mL) of the 65% solution and dilute it to 1 liter (1000 mL) to obtain a 2M nitric acid solution.
2) How to prepare 17% ammonia from 25% concentrated ammonia:
Step 1: Determine the volume of the concentrated solution needed to obtain the desired concentration. Let's assume you want to prepare 500 mL of 17% ammonia.
Step 2: Calculate the amount of ammonia in the desired solution.
Amount of ammonia (g) = Concentration (%) x Volume (mL) / 100
Given:
Concentration (%) = 25%
Volume (mL) = 500 mL
Amount of ammonia (g) = 25% x 500 mL / 100 = 125 g
Step 3: Calculate the volume of the concentrated ammonia solution required.
The volume of concentrated ammonia solution required can be calculated using the following equation:
Volume (mL) = Amount of ammonia (g) / Concentration (%)
Given:
Amount of ammonia (g) = 125 g
Concentration (%) = 25%
Volume (mL) = 125 g / 25% = 500 mL
To prepare a 17% ammonia solution, you need to take 500 mL of the 25% concentrated ammonia and dilute it to a total volume of 500 mL.
Is that 65% and 17% w/w or w/v?
Do you have a density listed.
I agree with the procedure.
My nitric (V) acid is 69.5% translating to a mass of 986.9 grams(pure acid).
Molarity of concentrated solution is 15.7M.
To prepare 2M HNO3 from it,measure 127.4cm³ of concentrated solution and top up to 1litre.