<u>Answer:</u>
<u>For 1:</u> The molarity of
in this solution is 0.0592 M
<u>For 2:</u> The new molarity of
in this solution is ![2.07\times 10^{-3}M](https://tex.z-dn.net/?f=2.07%5Ctimes%2010%5E%7B-3%7DM)
<u>Explanation:</u>
To calculate the molarity of solution, we use the equation:
![\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%20of%20the%20solution%7D%3D%5Cfrac%7B%5Ctext%7BMass%20of%20solute%7D%5Ctimes%201000%7D%7B%5Ctext%7BMolar%20mass%20of%20solute%7D%5Ctimes%20%5Ctext%7BVolume%20of%20solution%20%28in%20L%29%7D%7D)
Given mass of KOH = 1.66 g
Molar mass of KOH = 56.1 g/mol
Volume of solution = 500.0 mL
Putting values in above equation, we get:
![\text{Molarity of solution}=\frac{1.66\times 1000}{56.1g/mol\times 500.0}\\\\\text{Molarity of solution}=0.0592M](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%20of%20solution%7D%3D%5Cfrac%7B1.66%5Ctimes%201000%7D%7B56.1g%2Fmol%5Ctimes%20500.0%7D%5C%5C%5C%5C%5Ctext%7BMolarity%20of%20solution%7D%3D0.0592M)
1 mole of KOH produces 1 mole of potassium ions and 1 mole of hydroxide ions
So, molarity of ![K^+\text{ ions}=0.0592M](https://tex.z-dn.net/?f=K%5E%2B%5Ctext%7B%20ions%7D%3D0.0592M)
Hence, the molarity of
in this solution is 0.0592 M
To calculate the molarity of the diluted solution, we use the equation:
![M_1V_1=M_2V_2](https://tex.z-dn.net/?f=M_1V_1%3DM_2V_2)
where,
are the molarity and volume of the concentrated KOH solution having ![K^+\text{ ions}](https://tex.z-dn.net/?f=K%5E%2B%5Ctext%7B%20ions%7D)
are the molarity and volume of diluted KOH solution having ![K^+\text{ ions}](https://tex.z-dn.net/?f=K%5E%2B%5Ctext%7B%20ions%7D)
We are given:
![M_1=0.0592M\\V_1=35.00mL\\M_2=?M\\V_2=1000mL](https://tex.z-dn.net/?f=M_1%3D0.0592M%5C%5CV_1%3D35.00mL%5C%5CM_2%3D%3FM%5C%5CV_2%3D1000mL)
Putting values in above equation, we get:
![0.0592\times 35.00=M_2\times 1000\\\\M_2=\frac{0.0592\times 35.0}{1000}=2.07\times 10^{-3}M](https://tex.z-dn.net/?f=0.0592%5Ctimes%2035.00%3DM_2%5Ctimes%201000%5C%5C%5C%5CM_2%3D%5Cfrac%7B0.0592%5Ctimes%2035.0%7D%7B1000%7D%3D2.07%5Ctimes%2010%5E%7B-3%7DM)
Hence, the new molarity of
in this solution is ![2.07\times 10^{-3}M](https://tex.z-dn.net/?f=2.07%5Ctimes%2010%5E%7B-3%7DM)