Predict whether or not a precipitate forms upon mixing 175.0 mLmL of a 0.0055 MKClMKCl solution with 145.0 mLmL of a 0.0015 MM AgNO3AgNO3 solution. Identify the precipitate, if any.

Answer : The precipitate is, AgCl.

Explanation :

The balanced chemical reaction will be:

First we have to calculate the molarity of ion.

where,

are the initial molarity and volume of KCl.

are the final molarity and volume of ion.

We are given:

Putting values in above equation, we get:

Now we have to calculate the molarity of ion.

where,

are the initial molarity and volume of .

are the final molarity and volume of ion.

We are given:

Putting values in above equation, we get:

Now we have to calculate the value of reaction quotient.

The expression for reaction quotient will be :

Now put all the given values in this expression, we get

The given solubility constant value is,

As, then the reaction is reactant favored that means formation of precipitation.

Thus, the precipitate is, AgCl.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer