mix 120ml of 0.320M silver nitrate with 40ml of 0.320M potasium chromate. What mass of silver chromate is produced?

I am stuck please help

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  1. Write the balanced reaction and determine the limiting reactant. That will tell you how many moles of silver chromate are produced. Convert that to grams using the molar mass.

    Hint: Potassium chromate is K2CrO4
    CrO4(-2) is divalent.

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  2. this is what I came up with


    molar mass of 2agno3 = 277.18
    molar mass of k2cro4 = 194.2
    molar mass of ag2cro4 = 331.08


    limiting reactant k2cro4


    is this anywhere near right?

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  3. Your answer is close to a factor of 10 off but I don't understand most of what you did.
    Here is how I would do it, following DrWLS' response.
    moles AgNO3 = M x L = 0.32 x 0.120 = 0.0384 moles.
    moles K2CrO4 = M x L = 0.32 x 0.040 = 0.0128 moles.
    How much AgNO3 must we have if K2CrO4 is the limiting reagent? We must have 0.0128 x 2 = 0.0256 and we have that much; therefore, K2CrO4 is the limiting reagent. (We can check it by asking how much K2CrO4 we must have if AgNO3 is the limiting reagent. We must have 0.0384 x 1/2 = 0.0192 moles K2CrO4 and we don't have that much; therefore, K2CrO4 is the limiting reagent.)
    So we will have 0.0128 moles Ag2CrO4 produced and that x molar mass 0.0128 x 331.73 = 4.246 grams Ag2CrO4 which rounds to 4.25 grams (I'm guessing we are allowed 3 significant figures although with 40 and 120 written as they are I can't tell). Check you work; perhaps you just made a decimal point error.

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  4. Thank you so much, now I understand ... I think :)

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