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What is the concentration of K plus ions in a 0.025 M K2CO3 solution assuming complete dissociation?
Wiki User
∙ 6y ago
K2CO3 ==> 2K^+ + CO3^2-0.025 M K2CO3 = 2 x 0.025 M K^+ = 0.05 M concentration of K+ ions.
Wiki User
∙ 6y ago
Wiki User
∙ 13y ago3*0.785 = 2.355 M
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What is the molar concentration of Br- ions in a 0.225 M aqueous solution of FeBr3 assuming complete dissociation?
There are 0.225 mol dm-3 FeBr3 molecules. For each FeBr3 that fully dissociates, we get 3 Br- (and one F3+). It is fully dissociated. So 0.225 x 3 = 0.675 mol dm-3.
Why degree of dissociation of electrolyte increase with dilution?
these electrolytes will dissociate a lot less compared to the dissociation of strong electrolytes. This is due to the fact that they don't completely ionize in a moderately solution.
What is the total molar concentration of ions in a 0.350 M solution of the strong electrolyte Na2SO4 assuming complete dissociation?
1 mol Na2SO4 will dissociate to 2 mol Na+ and 1 mol SO42- Therefore 0.350 M Na2SO4 will dissociate to 0.350*2 = 0.700 mol Na+ and 0.350*1 = 0.350 mol SO42- Therefore the total concentration of ions is 0.700 mol + 0.350 mol = 1.050 mol.
Why does the molar conductivity of weak acid decrease as the concentration increases?
For a weak acid (or base), as the concentration increases, the % ionization/dissociation decreases. This leads to fewer ions in solution, and hence the molar conductivity decreases.
PH of acetic acid in 250M solution?
get the moles of hydrogen ions present in the solution by writing down the acid dissociation formula of the acid. Find the concentration of hydrogen ions present in the solution. Use -log[H+] to get the pH.
What describes a weak base in solution?
The dissociation is not complete.
What is the molar concentration of Br- ions in a 0.225 M aqueous solution of FeBr3 assuming complete dissociation?
There are 0.225 mol dm-3 FeBr3 molecules. For each FeBr3 that fully dissociates, we get 3 Br- (and one F3+). It is fully dissociated. So 0.225 x 3 = 0.675 mol dm-3.
Why degree of dissociation of electrolyte increase with dilution?
these electrolytes will dissociate a lot less compared to the dissociation of strong electrolytes. This is due to the fact that they don't completely ionize in a moderately solution.
What is the total molar concentration of ions in a 0.350 M solution of the strong electrolyte Na2SO4 assuming complete dissociation?
1 mol Na2SO4 will dissociate to 2 mol Na+ and 1 mol SO42- Therefore 0.350 M Na2SO4 will dissociate to 0.350*2 = 0.700 mol Na+ and 0.350*1 = 0.350 mol SO42- Therefore the total concentration of ions is 0.700 mol + 0.350 mol = 1.050 mol.
Why does the molar conductivity of weak acid decrease as the concentration increases?
For a weak acid (or base), as the concentration increases, the % ionization/dissociation decreases. This leads to fewer ions in solution, and hence the molar conductivity decreases.
PH of acetic acid in 250M solution?
get the moles of hydrogen ions present in the solution by writing down the acid dissociation formula of the acid. Find the concentration of hydrogen ions present in the solution. Use -log[H+] to get the pH.
What are examples of dissociation?
Dissociation of sodium chloride in water solution: NaCl -----------Na+ + Cl-
What process produce solute ions in a solution?
The Correct Answer is: Ionization and Dissociation.
What dictates how electrolytic an electrolyte is in solution?
This is the dissociation constant.
Ionic compounds produce ions in solution by?
Dissociation.
What is produced when a base dissolves in water?
A solution of the base in water. Like with acids you would get partial dissociation however. eg for NaOH, it would mostly split up into Na+ and OH-.
What has the author D D Perrin written?
D. D. Perrin has written: 'Ionisation constants of inorganic acids and bases in aqueous solution' -- subject(s): Bases (Chemistry), Dissociation, Inorganic acids, Tables 'Dissociation constants of organic bases in aqueous solution' -- subject(s): Ionization constants, Organic acids, Tables 'Dissociation constants of inorganic acids and bases in aqueous solution' -- subject(s): Bases (Chemistry), Dissociation, Inorganic acids, Tables 'Dissociation constants of organic bases in aqueous solution: supplement 1972' -- subject(s): Dissociation, Electrochemistry, Organic Chemistry, Tables
