Standerising NaOH: How to Do It & What Concentration of HCl

  • Thread starter Thread starter Bunting
  • Start date Start date
Click For Summary
SUMMARY

The discussion centers on the standardization of a 0.1 mol/dm³ sodium hydroxide (NaOH) solution using hydrochloric acid (HCl). Participants emphasize the importance of standardization due to the variability in NaOH composition and its tendency to absorb carbon dioxide (CO2) from the air, which alters its concentration over time. The necessity of understanding the concentration of HCl for accurate titration is also highlighted, as it directly impacts the results of the acid-base titration process.

PREREQUISITES
  • Understanding of acid-base titration techniques
  • Knowledge of molarity and solution preparation
  • Familiarity with the properties of NaOH and HCl
  • Basic laboratory safety protocols
NEXT STEPS
  • Research the process of standardizing NaOH with HCl using a primary standard
  • Learn about the preparation and use of standard solutions in titrations
  • Study the effects of CO2 absorption on NaOH concentration over time
  • Explore common laboratory practices for maintaining solution integrity
USEFUL FOR

Chemistry students, laboratory technicians, and educators involved in practical chemistry experiments, particularly those focusing on acid-base titrations and solution preparation.

Bunting
Messages
84
Reaction score
0
I am doing my chemistry practicle and my tecaher has told me that I need to standerise my 0.1moldm-3 solution of NaOH with HCl acid. But I don't know why or how, or what concentration of HCl. Does anyone have any ideas pls?
 
Chemistry news on Phys.org
Why? NaOH pellets have no definite composition --- you can't make up solutions by weight to better than a few percent uncertainty, and, once made up, it's a base, it absorbs CO2 from the air --- so, no matter how careful you are about keeping it closed, the concentration changes over time. This much information is not as well stressed during instruction as it should be. You get this much for free.

Since this is more in the category of a HW problem, now, you can tell us what you do know, how much instruction you've had, what lab manual you're working from, how much success you had with the acid-base titration exercises, and what you think is the place to start on this problem. 'Kay?
 

Similar threads

Hydrochloric Acid, NaOH, and English Ivy
  • · Replies 21 ·
Replies
21
Views
6K
Calculate the HCl concentration in H2O from the conductivity
  • · Replies 5 ·
Replies
5
Views
6K
Can Na2PdCl4 be used as a substitute for PdCl2 in electroless copper plating?
  • · Replies 1 ·
Replies
1
Views
3K
Ionization of Strong Acids: Does Concentration Matter?
  • · Replies 6 ·
Replies
6
Views
2K
Chemical water treatment: Acid base reaction
  • · Replies 2 ·
Replies
2
Views
3K
How to turn a weak acid into a strong acid
  • · Replies 35 ·
2
Replies
35
Views
7K
Why & How HCl is Used for Cleaning Materials
  • · Replies 3 ·
Replies
3
Views
2K
Chemistry A seemingly simple titration problem
  • · Replies 4 ·
Replies
4
Views
2K
Chemistry Titration of HCl with CaCO3, then excess HCl titrated with NaOH
  • · Replies 1 ·
Replies
1
Views
3K
What is the Boehm Back Titration end point?
  • · Replies 5 ·
Replies
5
Views
2K