A)What mass of silver chloride can be produced from 1.33 of a 0.207 solution of silver nitrate?
I got this one, its 39.4 g
B)The reaction described in Part A required 3.28 of potassium chloride. What is the concentration of this potassium chloride solution?
I keep getting 0.08 mol/L and that is not quite right! I am not sure what to do!
a. your numbers have no units.
b. is the reaction KCl+AgNO3?
Is that 3.28grams KCl? That is very little.
concentration= massKCl/(formulamassKCl*volumeinLiters)
I am quite certain your .08 is wrong, if no other reason, significant digits.
To find the concentration of the potassium chloride solution, you need to use the information provided in Part A and the balanced chemical equation for the reaction between silver nitrate and potassium chloride.
The balanced chemical equation for the reaction is:
AgNO3 + KCl -> AgCl + KNO3
From Part A, we know that 1.33 mol of a 0.207 M solution of silver nitrate is used in the reaction. This means that there are:
1.33 mol (0.207 mol/L) = 0.27531 L of silver nitrate solution
According to the balanced chemical equation, the stoichiometry between silver nitrate and potassium chloride is 1:1. This means that for every 1 mole of silver nitrate used, we need 1 mole of potassium chloride.
Since we know that 3.28 mol of potassium chloride was required, we can conclude that:
3.28 mol KCl solution = 3.28 M
Therefore, the concentration of the potassium chloride solution is 3.28 M, not 0.08 M as you initially calculated.