Chemistry Molarity?

Question

Reacting 40mL of 0.200 M AgNO3 with 40mL of 0.200 M K2CrO4 results in what mass of solid form? Pls help. I totally don't get this!!

Answer 1

2 AgNO3 (aq) + K2CrO4 (aq) --> Ag2CrO4 (s) + 2KNO3 (aq)

1) first calculate the number of moles of each reactant.
.04 L x .2 mol/L = .008 mol AgNO3
.04 L x .2 mol/L = .008 mol K2CrO4

2) use mole ratio from balanced equation:
2 mol AgNO3 to 1 mol Ag2CrO4 so the most you could make would be .008 mol AgNO3 to .004 mol Ag2CrO4

3) change .004 mol Ag2CrO4 to grams using the molar mass

Answer 2

you may no longer artwork it out till you comprehend the concentration of the NaOH in moles in keeping with litre. assume it = M. Then 15.a million ml of the NaOH includes 15.1M/one thousand moles of NaOH. in view that a million mole of NaOH reacts with a million mole of CH3COOH there must be 15.1M/one thousand moles CH3COOH in 5 ml or (15.1M/one thousand) x one thousand/5 moles in keeping with litre