500mg/l
I'm not sure abut the K2CrO4, but adding concentrated HCl to saturated NH4Cl you can form usually a white precipitate (with clearish suspension).
K2Cr2O7 + 6 KI + 7 H2So4 = Cr2(So4)3 + 4 K2So4 + 3 I2 + 7 H2O
KCrO4 does not exist it is K2CrO4 and is called Potassium Chromate. Potassium dichromate is K2Cr2O7
BaCl2+K2CrO4--------->BaCrO4+2KCl BaCrO4 is a yellow precipitate.
K2CrO4 Molarity (concentration) = moles of solute/Liters of solution (100 ml = 0.100 Liters ) Find moles K2CrO4 first. 3.50 grams = (1 mole K2CrO4/194.2 grams) = 0.01802 moles K2CrO4 ----------------------------------------------next Molarity = 0.01802 moles K2CrO4/0.100 Liters = 0.180 M K2CrO4 -------------------------
500mg/l
I'm not sure abut the K2CrO4, but adding concentrated HCl to saturated NH4Cl you can form usually a white precipitate (with clearish suspension).
inorganic
K2Cr2O7 + 6 KI + 7 H2So4 = Cr2(So4)3 + 4 K2So4 + 3 I2 + 7 H2O
KCrO4 does not exist it is K2CrO4 and is called Potassium Chromate. Potassium dichromate is K2Cr2O7
Chromate
Formula: K2CrO4
It depends on how much you have.
Formula: K2CrO4
Formula: K2CrO4
Formula: K2CrO4