Calculate the molarity of KMNO4 solution needed to titrate 50.00 mL of a saturated solution of this oxalate salt. It should take 7.50 mL of KMnO4 solution to titrate the saturated oxalate solution.
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.
![**Solubility Product Constant**
**Identity of Oxalate Salt:** SrC2O4·H2O
**Solubility:**
0.00433 g SrC2O4·H2O / 100 g H2O
**Molar Mass Calculation:**
(SrC2O4·H2O):
- Sr: 87.62
- C: 12.01 x 2
- O: 16.00 x 4
- H2O: 18.01
Total molar mass = 193.65 g/mol
**Ksp from Solubility (Show your calculations below):**
\[ 5.00 \times 10^{-8} \]
Convert to moles:
\[
\frac{0.00433 \text{ g SrC2O4·H2O}}{193.65 \text{ g/mol}} = 2.2359 \times 10^{-5} \text{ mol}
\]
Calculate molarity:
\[
\frac{2.2359 \times 10^{-5} \text{ mol}}{0.1 \text{ L}} \times \frac{1000 \text{ mL}}{1 \text{ L}} = 2.2359 \times 10^{-4} \text{ M}
\]
Dissociation:
\[
\text{SrC2O4} \rightarrow \text{Sr}^{2+} + \text{C2O4}^{2-}
\]
Ksp:
\[
[\text{Sr}^{2+}] [\text{C2O4}^{2-}]
\]
Concentration of both Sr and C2O4 ions:
\[ 2.2359 \times 10^{-4} \, \text{M} \]
Ksp:
\[
\begin{align*}
2.2359 \times 10^{-4} \, \text{M} \times 2.2359 \times 10^{-4} \, \text{M} & = 4.9966 \times 10^{-8} \\
Ksp & = 5.00 \times 10^{-8}
\end{align*}
\]
**Calculate the molarity of KMnO4 solution needed to titrate 50.00 mL of a saturated solution](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa59a73bf-87c2-48f6-829d-0178c9223cc0%2Ffcaeac64-bcb0-49ae-8c1b-534878cfb9ba%2Fjml27he_processed.jpeg&w=3840&q=75)
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