complete the following double displacement reaction and indicate the states:
KCl+AgNO3=
From the information available how are you supposed to know if these are in solution or not?
KCl(aq) + AgNO3(aq) ==> AgCl(s) + KNO3(aq)
OR
KCl(s) + AgNO3(s) ==> no reaction
To complete the double displacement reaction between KCl and AgNO3, we need to determine the products. The general rule for double displacement reactions is that the positive ions (cations) of each compound switch places.
KCl + AgNO3 → KNO3 + AgCl
Now, let's indicate the states of each compound:
KCl (potassium chloride) is a solid (s)
AgNO3 (silver nitrate) is a solid (s)
KNO3 (potassium nitrate) is a solid (s)
AgCl (silver chloride) is a solid (s)
Therefore, the balanced equation with states is:
KCl (s) + AgNO3 (s) → KNO3 (s) + AgCl (s)
To complete the double displacement reaction between KCl and AgNO3, we need to determine the products and their states.
First, let's write the balanced equation:
KCl + AgNO3 → KNO3 + AgCl
In this reaction, the potassium chloride (KCl) reacts with silver nitrate (AgNO3) to produce potassium nitrate (KNO3) and silver chloride (AgCl).
Now, let's indicate the states of the reactants and products:
KCl (aq) + AgNO3 (aq) → KNO3 (aq) + AgCl (s)
The letters in parentheses indicate the states of the substances. In this case:
- (aq) represents a substance dissolved in water (aqueous)
- (s) represents a solid precipitate formed
KCl and AgNO3 are both soluble in water, so they are both in the aqueous state (aq). However, when potassium chloride and silver nitrate react, they form silver chloride, which is insoluble in water. Therefore, silver chloride appears as a solid precipitate (s) in the balanced equation.
So, the complete double displacement reaction is:
KCl (aq) + AgNO3 (aq) → KNO3 (aq) + AgCl (s)