22.50 mL of the Fe²+ solution required 12.50 mL of 0.255 M K₂Cr₂O, to reach the end point. Calculate the concentration of the Fe²+ solution. 0.127 [Fe²+] = Incorrect M
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.
Seeking an answer for the second part, [Fe2+].
![A Fe²+ solution is titrated with a K₂Cr₂O solution according to the unbalanced reaction below.
Cr₂O² (aq) + Fe²+ (aq)
Cr³+ (aq) + Fe³+ (aq)
Select net ionic equation that shows the above reaction balanced in acidic solution.
Cr₂O² (aq) + 6 Fe²+ (aq) + 14 H+ (aq) -
2 Cr₂O²¯(aq) + Fe²+ (aq) → 4 Cr³ + (aq)
Cr₂O²¯(aq) + Fe²+ (aq) + 14 H+ (aq)
2 Cr³+ (aq) + 6 Fe³+ (aq) + 7 H₂O(1)
+ Fe³+ (aq) + 70₂(g)
2 Cr³+ (aq) + Fe³+ (aq) + 7 H₂O(1)
Cr₂O²¯(aq) + 6 Fe²+ (aq) + 7 H₂O(1) → 2 Cr³ + (aq) + 6 Fe³ + (aq) + 14 OH¯(aq)
22.50 mL of the Fe²+ solution required 12.50 mL of 0.255 M K₂Cr₂O, to reach the end point.
Calculate the concentration of the Fe²+ solution.
0.127
[Fe²+] =
Incorrect
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