Standardization of NaOH Method 1 Fill a burette with the solution of NaOH(aq) of unknown concentration. Pipette 25.00 cm³ of the standard solution of 0.10 mol dm HCl(aq) onto a clean conical flask. Add a few drops of the indicator bromothymol blue solution to the conical flask and stand it on a white tile or white paper. Titrate the NaOH against the HCI, until the endpoint of the indicator is observed, and record the volume added from the burette. Repeat the titration until final values within 0.05 cm³ are obtained. Results Volume NaoH Titration 1 Titration 2 Titration 3 end volume / cm³ ± 0.05 24.7 24.8 24.6 start volume / cm t 0.05 titre / cm +0.10 24.7 24.8 24.6 average titre / cm³ ±0.10 = 24.7 Also, record your qualitative data.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
- Calculate the concerntration of NaOH in the solution provided.
Step by step
Solved in 3 steps
