Potassium Chloride Reacts With Silver Nitrate To Produce Solid Silver Chloride And Potassium Nitrate. KCl(Aq) + AgNO3(Aq) → AgCl(S) + KNO3(Aq) How Many Grams Of KCl Are Required To React Completely With 250 ML Of 0.030 M AgNO3? 2.63 G 13.18 0.1018 3.358 0.1128 0.559 8
The Correct Answer and Explanation is :
The balanced chemical equation for the reaction between potassium chloride (KCl) and silver nitrate (AgNO₃) is:
[ \text{KCl (aq)} + \text{AgNO₃ (aq)} \rightarrow \text{AgCl (s)} + \text{KNO₃ (aq)} ]
Step 1: Calculate the moles of AgNO₃
First, we need to find the moles of AgNO₃ in the solution. The molarity (M) of AgNO₃ is 0.030 M, and the volume of the solution is 250 mL, or 0.250 L.
Moles of AgNO₃ can be calculated using the formula:
[
\text{Moles of AgNO₃} = \text{Molarity} \times \text{Volume}
]
[
\text{Moles of AgNO₃} = 0.030 \, \text{M} \times 0.250 \, \text{L} = 0.0075 \, \text{mol}
]
Step 2: Use the stoichiometry of the reaction
From the balanced equation, we can see that the mole ratio of KCl to AgNO₃ is 1:1. This means that 1 mole of KCl reacts with 1 mole of AgNO₃. Therefore, the moles of KCl required to react with 0.0075 moles of AgNO₃ is also 0.0075 moles of KCl.
Step 3: Calculate the mass of KCl required
Now, we will convert the moles of KCl to grams. The molar mass of KCl is calculated as:
[
\text{Molar mass of KCl} = \text{K} + \text{Cl} = 39.1 \, \text{g/mol} + 35.45 \, \text{g/mol} = 74.55 \, \text{g/mol}
]
The mass of KCl required is:
[
\text{Mass of KCl} = \text{Moles of KCl} \times \text{Molar mass of KCl}
]
[
\text{Mass of KCl} = 0.0075 \, \text{mol} \times 74.55 \, \text{g/mol} = 0.559 \, \text{g}
]
Conclusion:
The mass of KCl required to react completely with 250 mL of 0.030 M AgNO₃ is 0.559 g.
Thus, the correct answer is 0.559 g.