Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction.
(a) AgBr

Question

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. 
(a) AgBr

Accepted Answer

Hello everyone in this video. I want to determine if the scalability of C. U C L. Will increase an acidic solution. We also have to go ahead and provide the balance net ionic equation for one CCL dissolves to form a solution. So first let's start off with reading out the reaction. So we're starting off with of course R C U C L. Which is a solid. It's an equilibrium with its ions and that's C. U. Plus. So copper plus which is a quiz and chlorine minus one which is also acquis Alright so everything here does look to balance. We have one mole of each item here per side. So starting off with our C. U. Plus. So this is a plus one charge transition metal. Since it's a transition metal we have this being neutral and the first cl minus here it comes from H C. L. Which is a strong acid. So this is also neutral. So basically here we're adding a neutral atom with another neutral item which of course just means at the end we'll have an overall neutral molecule. The scalability of CCL two will not increase in an acidic solution. Again, the Celje bility of C U C L will not increase in an acidic solution. So the reaction here is the net ionic equation. And then this is our answer for the first problem which is asking if the scalability of CCL will increase or decrease in an acidic solution

Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) AgBr

Verified Solution

Key Concepts

Solubility and pH

Common Ion Effect

Net Ionic Equations