A 1.85-g sample of a mixture of KCl and MgCl(subscript 2) is treated with excess AgNO(subscript 3) (aq). If 3.82 grams of AgCl(s) are obtained, then what is the percentage by mass of KCl in the original mixture.
Can someone tell me what the balanced chemical equation is for this reaction please?
Chloride comes from two sources.
AgNO3 + KCl ==> AgCl + KNO3 AND
2AgNO3 + MgCl2 --> 2AgCl + Mg(NO3)2
To solve this problem you must have two equations and solve them simultaneously.
Sure, here's the balanced chemical equation:
2AgNO3(aq) + MgCl2(aq) β 2AgCl(s) + Mg(NO3)2(aq)
Now for a little humor: Why did the chemist go broke? Because all his reactions were imbalanced! π
Sure! The balanced chemical equation for the reaction between AgNO3(aq) and a mixture of KCl and MgCl2 can be written as follows:
2AgNO3(aq) + KCl(aq) -> 2AgCl(s) + KNO3(aq)
In this equation, two moles of AgNO3 react with one mole of KCl to produce two moles of AgCl and one mole of KNO3.
To find the balanced chemical equation for the reaction between the mixture of KCl and MgCl(subscript 2) with AgNO(subscript 3), we need to understand the reaction taking place.
In this reaction, AgNO(subscript 3) reacts with the chloride ions (Cl-) present in the mixture of KCl and MgCl(subscript 2) to form AgCl(s) precipitate. The balanced chemical equation can be written as:
2AgNO(subscript 3) + KCl β 2AgCl(s) + KNO(subscript 3)
In this equation, 2 moles of AgNO(subscript 3) react with 1 mole of KCl to produce 2 moles of AgCl(s) and 1 mole of KNO(subscript 3).
It's important to note that in the given information, the amount of AgCl(s) formed from the reaction is given as 3.82 grams. This information will help us determine the percentage by mass of KCl in the mixture.
Now that we have the balanced chemical equation, we can proceed to calculate the percentage by mass of KCl.