Could I have an Example of Lab report: What is the best eway to remove silvert i
ID: 1036570 • Letter: C
Question
Could I have an Example of Lab report: What is the best eway to remove silvert ion (Ag+) from aqueous solution? This is my first part: Chemical reactions are usually recognized by a color change, the formation of a solid, the formation of bubbles, or a change in temperature. “What is the best way to remove silver ion from an aqueous solution?” Single displacement is the best way since it extracts pure silver ion and is in accordance to the guiding question. Many reactions occur in an aqueous environment. When a reactant or product has the physical state (aq) that substance is dissolved in water. An ionic compound in aqueous solution exists as individual ions in water. To determine if an ionic compound is soluble (it will dissolve in water) the solubility rules are used. In a single- displacement reaction, a more reactive metal element displaces another element from a compound, and a new element and compound are formed as the products. In a double- replacement/precipitation reaction, two ionic compounds in aqueous solution swap metals to form a precipitate , a solid formed when two ionic solutions are mixed. A limiting reagent, is the substance that completely used up when the chemical reaction is complete. The amount of product formed is limited by this reagent, since the reaction cannot continue without it.
Could you help me to have the total Lb complete?
Explanation / Answer
Best way to remove silver ion (Ag+ ) from an aqueous solution:
Add hydrochoric acid to the solution. Ag+ will react with HCl via a single displacement reaction and an insoluble precipitate of AgCl will appear. Filter out the precipitate. The filtrate is the aqueous solution that is free from Ag+ ion.
physical state (aq):
An ionic compound in aqueous solution exists as individual ions in water. We write the formulas the compound soulble in water followed by 'aq' in parenthesis.
Example: reaction between AgNO3 and NaCl
AgNO3 (aq) + NaCl (aq) = AgCl (s) + NaNO3 (aq)
Single- displacement reaction:
a more reactive metal element displaces another element from a compound, and a new element and compound are formed as the products.
Fe + CuSO4 = FeSO4 + Cu
Here, Fe displaces Cu as Fe is more reactive than Cu.
double- replacement/precipitation reaction:
wo ionic compounds in aqueous solution swap metals to form a precipitate , a solid formed when two ionic solutions are mixed.
Example: AgNO3 (aq) + NaCl (aq) = AgCl (s) + NaNO3 (aq)
Limiting reagent:
the substance that completely used up when the chemical reaction is complete.
Example: Mg + 2 HCl = MgCl2 + H2
If 1 mole Mg is allowed to react with 4 moles HCl, then Mg is the limiting reagent. Because 1 mole Mg reacts with maximum 2 moles HCl and rest 2 moles HCl remains unreacted. So, Mg reacts completely
Chemical reactions are usually recognized by a color change, the formation of a solid, the formation of bubbles, or a change in temperature.:
Colour change: PbCl2 (aq) + H2CrO4 (aq) = PbCrO4 (yellow precipitate) + 2 HCl (aq)
Formation of solid: AgNO3 (aq) + NaCl (aq) = AgCl (s) + NaNO3 (aq)
Formation of bubbles: Mg (s) + 2 HCl (aq) = MgCl2 (aq) + H2 (g) , H2 is bubbled out
Temperature change: CH4 (g) + 2O2 (g) = CO2 (g) +2 H2O (g), its an exothermic reaction and heat is released