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Answer:
40:1 is the ratio of the magenta phenolphthalein concentration to the colorless phenolphthalein concentration.
Explanation:
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
![pH=pK_a+\log(\frac{[salt]}{[acid]})](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%28%5Cfrac%7B%5Bsalt%5D%7D%7B%5Bacid%5D%7D%29)
![pH=pK_a+\log(\frac{[magenta(Php)]}{[Php]})](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%28%5Cfrac%7B%5Bmagenta%28Php%29%5D%7D%7B%5BPhp%5D%7D%29)
We are given:
= negative logarithm of acid dissociation constant of phenolphthalein = 9.40
= concentration of magenta phenolphthalein
= concentration of colorless phenolphthalein
pH = 11
Putting values in above equation, we get:
![11=9.40+\log(\frac{[magenta(Php)]}{[Php]})](https://tex.z-dn.net/?f=11%3D9.40%2B%5Clog%28%5Cfrac%7B%5Bmagenta%28Php%29%5D%7D%7B%5BPhp%5D%7D%29)
![\log(\frac{[magenta(Php)]}{[Php]})=11-9.40=1.6](https://tex.z-dn.net/?f=%5Clog%28%5Cfrac%7B%5Bmagenta%28Php%29%5D%7D%7B%5BPhp%5D%7D%29%3D11-9.40%3D1.6)
![\frac{[magenta(Php)]}{[Php]}=10^{1.6}=39.81 :1 \approx 40:1](https://tex.z-dn.net/?f=%5Cfrac%7B%5Bmagenta%28Php%29%5D%7D%7B%5BPhp%5D%7D%3D10%5E%7B1.6%7D%3D39.81%20%3A1%20%5Capprox%2040%3A1)
40:1 is the ratio of the magenta phenolphthalein concentration to the colorless phenolphthalein concentration.
Molar solubility is the number of moles that are dissolved in 1 L solution.
when BaF₂ dissolves it dissociates into the following ions
BaF₂ --> Ba²⁺ + 2F⁻
if the molar solubility of BaF₂ is X, then molar solubility of Ba²⁺ is X and F⁻ is 2x
then the formula for the solubility product constant -ksp is;
ksp = [Ba²⁺][F⁻]²
ksp = X * (2X)²
ksp = 4X³
since ksp = 1.7 x 10⁻⁶
4X³ = 1.7 x 10⁻⁶
X = 0.0075 M
molar solubility of BaF₂ is 0.0075 M
Strong acids can dissolve the salts of weak acid. When we consider the different salts of silver:
Salts of silver with the conjugate bases of a weak acid are soluble in strong acidic solutions. Some of these salts are:
![2Ag^{+}(aq)+CO_{3}^{2-}(aq) --->Ag_{2}CO_{3}(s)](https://tex.z-dn.net/?f=2Ag%5E%7B%2B%7D%28aq%29%2BCO_%7B3%7D%5E%7B2-%7D%28aq%29%20---%3EAg_%7B2%7DCO_%7B3%7D%28s%29)
![Ag^{+}(aq)+C_{2}H_{3}O_{2}^{-}(aq)-->AgC_{2}H_{3}O_{2}(aq)](https://tex.z-dn.net/?f=Ag%5E%7B%2B%7D%28aq%29%2BC_%7B2%7DH_%7B3%7DO_%7B2%7D%5E%7B-%7D%28aq%29--%3EAgC_%7B2%7DH_%7B3%7DO_%7B2%7D%28aq%29)
![2Ag^{+}(aq)+SO_{3}^{2-}(aq) --->Ag_{2}SO_{3}(s)](https://tex.z-dn.net/?f=2Ag%5E%7B%2B%7D%28aq%29%2BSO_%7B3%7D%5E%7B2-%7D%28aq%29%20---%3EAg_%7B2%7DSO_%7B3%7D%28s%29)
Salts of silver with the conjugate bases of a strong acid are not affected by change in pH:
![Ag^{+}(aq)+Cl^{-}(aq) --->AgCl(s)](https://tex.z-dn.net/?f=Ag%5E%7B%2B%7D%28aq%29%2BCl%5E%7B-%7D%28aq%29%20---%3EAgCl%28s%29)
![2Ag^{+}(aq)+SO_{4}^{2-}(aq) --->Ag_{2}SO_{4}(s)](https://tex.z-dn.net/?f=2Ag%5E%7B%2B%7D%28aq%29%2BSO_%7B4%7D%5E%7B2-%7D%28aq%29%20---%3EAg_%7B2%7DSO_%7B4%7D%28s%29)
These two salts with Chloride and sulfate ions are not soluble in acidic solutions as the salts of silver with the conjugate bases of a strong acid are not soluble in acidic solutions, they remain unaffected by any change in pH.
So for salts of Ag and Ba with the conjugate bases of a weak acid, solubility is increased upon the addition of an acid. So, the interference from the ions of weak acids can be removed by decreasing the pH.