Preparing 0.1M Nitric Acid (1000ml, 65% Nitric Acid)

  • Thread starter Thread starter kaykay11
  • Start date Start date
  • Tags Tags
    Acid
Click For Summary

Discussion Overview

The discussion centers around the preparation of 1000ml of 0.1M Nitric acid using a 65% Nitric acid solution. Participants explore the calculations and steps necessary for dilution, including the use of specific gravity and molecular weight in their reasoning.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant asks how to prepare the solution, providing the concentration and specific properties of the nitric acid.
  • Another participant reiterates the goal of making 1000ml of 0.1M Nitric acid and lists relevant properties such as specific gravity and molecular weight.
  • A third participant suggests using the formula provided to substitute the values for the calculation.
  • A fourth participant proposes starting with the number of moles of HNO3 needed and then calculating the grams of pure HNO3, noting the source is not pure but a 65% solution, indicating further steps are required.

Areas of Agreement / Disagreement

The discussion remains unresolved, with participants offering different approaches and calculations without reaching a consensus on the method to be used.

Contextual Notes

Participants reference specific equations and properties but do not clarify all assumptions or dependencies in their calculations, leaving some steps and definitions potentially ambiguous.

kaykay11
Messages
2
Reaction score
0
how do I make 1000ml of 0.1M Nitric acid with 65% Nitric acide (specific gravity 1.42g) and Molecular weight 63g/mol
 
Physics news on Phys.org
Diluting acid with water

Homework Statement



To make 1000ml of 0.1M of Nitric acid with 65% Nitric acid.
Specific gravity= 1.42g/
Molecular weight= 63g/mol

Homework Equations


M = ((% x Specific gravity)/Molecular weight) x 10
cava = cfvf


The Attempt at a Solution

 


You presented a formula in your Relevant equations section. If you trust this formula then just substitute the values for the described information.
 
You could start with the number of moles of HNO3 you would want. If you know the moles of HNO3, then use formula weight to find number of grams of pure HNO3; but you know that your source is not pure, but instead is 65% w/w. so you have two more steps... can you derive them?
 

Similar threads

Titration Exam Question 1: Calculating Concentration of Undiluted Nitric Acid
  • · Replies 3 ·
Replies
3
Views
3K
Dissolving silver
  • · Replies 5 ·
Replies
5
Views
1K
Why Does Adding Nitric Acid to Copper and Carbon Dioxide Produce Brown Gas?
  • · Replies 14 ·
Replies
14
Views
3K
What is the percentage of Fool's Gold in the original sample?
  • · Replies 10 ·
Replies
10
Views
3K
How Do You Model the Changing Concentration of Nitric Acid in a Tank?
  • · Replies 3 ·
Replies
3
Views
1K
Determining pH using Henderson-Hasselbach equation?
  • · Replies 12 ·
Replies
12
Views
3K
Chemistry Are there typos in this snippet causing confusion?
  • · Replies 2 ·
Replies
2
Views
2K
Chemistry Book seems to say that we can have weak acid and weak conjugate base
  • · Replies 2 ·
Replies
2
Views
2K
Using nitric acid to dissolve brass
  • · Replies 8 ·
Replies
8
Views
4K
Chemistry How to calculate pH at equivalence point using this alternative?
  • · Replies 7 ·
Replies
7
Views
2K