To determine the mass of solid formed, we can use the concept of stoichiometry and the balanced chemical equation for the reaction between K2CrO4 and AgNO3:
2 K2CrO4 + 3 AgNO3 -> Ag2CrO4 + 2 KNO3
From the balanced equation, we can see that for every 2 moles of K2CrO4, we produce 1 mole of Ag2CrO4.
First, let's calculate the number of moles of K2CrO4 and AgNO3 in the given solutions:
Number of moles of K2CrO4 = (volume of solution in L) * (molarity of solution in mol/L)
= (40.0 mL / 1000 mL/L) * 0.200 mol/L
= 0.008 mol
Number of moles of AgNO3 = (volume of solution in L) * (molarity of solution in mol/L)
= (40.0 mL / 1000 mL/L) * 0.200 mol/L
= 0.008 mol
From the stoichiometry of the balanced equation, we know that the number of moles of Ag2CrO4 formed is half the number of moles of K2CrO4 used:
Number of moles of Ag2CrO4 formed = 0.008 mol / 2
= 0.004 mol
To find the mass of Ag2CrO4 formed, we need to convert the number of moles to grams using the molar mass of Ag2CrO4:
Molar mass of Ag2CrO4 = (2 * atomic mass of Ag) + atomic mass of Cr + (4 * atomic mass of O)
= (2 * 107.87 g/mol) + 52.00 g/mol + (4 * 16.00 g/mol)
= 331.74 g/mol
Mass of Ag2CrO4 formed = (number of moles of Ag2CrO4) * (molar mass of Ag2CrO4)
= 0.004 mol * 331.74 g/mol
= 1.327 g
Therefore, the mass of solid formed is 1.327 g. None of the provided answer choices match this result, so the correct answer cannot be determined from the given options.
If you mix 40.0 mL of a 0.200 M solution of K2CrO4 is reacted with 40.0 mL of a 0.200 M solution of AgNO3, what mass of solid forms?
Group of answer choices
1.79 g
2.65 g
0.896 g
1.33 g
none of these
1 answer