This is only one question!!! Using this reactions:1) Na2B4O5(OH)4⋅8 H2O (s) → 2 Na+ (aq) + B4O5(OH)42– (aq) + 8 H2O (l) and 2) B4O5(OH)42– (aq) + 2 H3O+ (aq) + H2O (l) → 4 H3BO3 (aq) Using Titration data and the volume of sample. Calculate concentration of Sodium ion in each of the 5 samples: K = [Na+]2[ B4O5(OH)42–] Molarity of HCL 0.2021 Data:40 mL Borox+0.80mL DI water mixed in Erlenmeyer flask, was placed into 1 L beaker and heated to 55C. Then cooled to 50,40.30, 20, and 10 degrees C. Samples Data: Sample Tubes at 50C, 40C, 30C, 20C, 10C 50 degree C = 9.4 ml 40 degree C= 8,60 ml 30C=9.3 ml 20C=9.1ml 10C=3.6 ml Titration data: Titrated with HCL and indicator Bromocresol Green 1) 50 degrees C Initial volume in the burette 0.0 and the color changed to green at 39.10 2) 40 degrees C Initial volume in the burette 0. 00 Color changed at 27.00 ml 3) 30 degrees C tube Initial volume in the burette 0.00 Color changed at 24.40 mL 4) 20 degrees C tube Initial volume in the burette 0.00 Color changed at 17.50 mL 5) 10 degrees C tube Initial volume in the burette is 0.00 Color changed at 2.90 mL
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.
This is only one question!!!
Using this reactions:1) Na2B4O5(OH)4⋅8 H2O (s) → 2 Na+ (aq) + B4O5(OH)42– (aq) + 8 H2O (l) and 2) B4O5(OH)42– (aq) + 2 H3O+ (aq) + H2O (l) → 4 H3BO3 (aq) Using Titration data and the volume of sample. Calculate concentration of Sodium ion in each of the 5 samples:
K = [Na+]2[ B4O5(OH)42–]
Molarity of HCL 0.2021
Data:40 mL Borox+0.80mL DI water mixed in Erlenmeyer flask, was placed into 1 L beaker and heated to 55C. Then cooled to 50,40.30, 20, and 10 degrees C.
Samples Data:
Sample Tubes at 50C, 40C, 30C, 20C, 10C
50 degree C = 9.4 ml
40 degree C= 8,60 ml
30C=9.3 ml
20C=9.1ml
10C=3.6 ml
Titration data:
Titrated with HCL and indicator Bromocresol Green
1) 50 degrees C
Initial volume in the burette 0.0 and the color changed to green at 39.10
2) 40 degrees C
Initial volume in the burette 0. 00
Color changed at 27.00 ml
3) 30 degrees C tube
Initial volume in the burette 0.00
Color changed at 24.40 mL
4) 20 degrees C tube
Initial volume in the burette 0.00
Color changed at 17.50 mL
5) 10 degrees C tube
Initial volume in the burette is 0.00
Color changed at 2.90 mL
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