Answer:
The statement is FALSE.
Explanation:
It is known as the ion effect common to the displacement of an ionic equilibrium when the concentration of one of the ions that are involved in said equilibrium changes, due to the presence in the dissolution of a salt that is dissolved in it.
Given the reaction of the dissociation reaction of a weak electrolyte:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
The equilibrium constant of the reaction is:
![K_{ps}=\frac{[A^+][B^-]}{[AB]}](https://tex.z-dn.net/?f=K_%7Bps%7D%3D%5Cfrac%7B%5BA%5E%2B%5D%5BB%5E-%5D%7D%7B%5BAB%5D%7D)
Given the reaction of the dissociation reaction of a stong electrolyte:
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
If the electrolyte CB is added to the medium in which electrolyte AB is found, the medium will have a common ion B⁻:
AB (s) ⇔ A⁺(aq) + B⁻ (aq)
CB (s) ⇒ C⁺(aq) + B⁻ (aq)
By the Le Chatelier's principle, having more concentration of products, the balance will shift to the right.
Hence, the extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.
Explanation:
When pH of the solution is 11.
![pH=-\log[H^+]](https://tex.z-dn.net/?f=pH%3D-%5Clog%5BH%5E%2B%5D)
![11=-\log[H^+]](https://tex.z-dn.net/?f=11%3D-%5Clog%5BH%5E%2B%5D)
![[H^+]=1\times 10^{-11} M](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D1%5Ctimes%2010%5E%7B-11%7D%20M)
..(1)
At pH = 11, the concentration of 
ions is 
.
When the pH of the solution is 6.
![pH=-\log[H^+]'](https://tex.z-dn.net/?f=pH%3D-%5Clog%5BH%5E%2B%5D%27)
![6=-\log[H^+]'](https://tex.z-dn.net/?f=6%3D-%5Clog%5BH%5E%2B%5D%27)
![[H^+]'=1\times 10^{-6} M](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%27%3D1%5Ctimes%2010%5E%7B-6%7D%20M)
..(2)
At pH = 6, the concentration of ions is 
.
On dividing (1) by (2).
![\frac{[H^+]}{[H^+]'}=\frac{1\times 10^{-11} M}{1\times 10^{-6}}=1\times 10^{-5}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BH%5E%2B%5D%7D%7B%5BH%5E%2B%5D%27%7D%3D%5Cfrac%7B1%5Ctimes%2010%5E%7B-11%7D%20M%7D%7B1%5Ctimes%2010%5E%7B-6%7D%7D%3D1%5Ctimes%2010%5E%7B-5%7D%20)
The ratio of hydrogen ions in solution of pH equal to 11 to the solution of pH equal to 6 is 
.
Difference between the ions at both pH:
This means that Hydrogen ions in a solution at pH = 7 has 
ions fewer than in a solution at a pH = 6
Answer:
7.5 g
Explanation:
There is some info missing. I think this is the original question.
<em>Ammonium phosphate ((NH₄)₃PO₄) is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H₃PO₄) with ammonia (NH₃). What mass of ammonium phosphate is produced by the reaction of 4.9 g of phosphoric acid? Be sure your answer has the correct number of significant digits.</em>
<em />
Step 1: Write the balanced equation
H₃PO₄ + 3 NH₃ ⇒ (NH₄)₃PO₄
Step 2: Calculate the moles corresponding to 4.9 g of phosphoric acid
The molar mass of phosphoric acid is 98.00 g/mol.
Step 3: Calculate the moles of ammonium phosphate produced from 0.050 moles of phosphoric acid
The molar ratio of H₃PO₄ to (NH₄)₃PO₄ is 1:1. The moles of (NH₄)₃PO₄ produced are 1/1 × 0.050 mol = 0.050 mol.
Step 4: Calculate the mass corresponding to 0.050 moles of ammonium phosphate
The molar mass of ammonium phosphate is 149.09 g/mol.
Answer:
The molality of the glycerol solution is 2.960×10^-2 mol/kg
Explanation:
Number of moles of glycerol = Molarity × volume of solution = 2.950×10^-2 M × 1 L = 2.950×10^-2 moles
Mass of water = density × volume = 0.9982 g/mL × 998.7 mL = 996.90 g = 996.90/1000 = 0.9969 kg
Molality = number of moles of glycerol/mass of water in kg = 2.950×10^-2/0.9969 = 2.960×10^-2 mol/kg
Yes I can do in organic chem
