do number 11 please 10. lf you evaporated 250. mL of a 3.5 M solution of iron Fe

Question

do number 11 please

10. lf you evaporated 250. mL of a 3.5 M solution of iron Fe(NO)2, what mass of iron (II) nitrite would you recover? 11. A chemist has 4.0 g of silver nitrate (AgNO,) and needs to prepare 2.0 L of a 0.010 M solution. Will there be enough silver nitrate? If so, how much silver nitrate will be left over? 12. A chemist pours 500.00 mL of a 3.0000 molar solution of sodium hydroxide into a 2.000 liter volumetric flask and fills the flask up with water. What is the new molarity of the solution?

Explanation / Answer

Molarity of solution = 0.010M, volume= 2 L

Moles of AgNO3 = Molariry* volume =0.010*2=0.02 moles

Atomic weights (g/mole): Ag= 108, N= 14 and O=16

Molar mass of AgNo3= 108+14+3*16=170 g/mole

Mass of AgNO3 required to prepare 2L of 0.010= moles* molarity= 0.02*170= 3.4 gm

Gms of AgNO3 available= 4 gm, there is enough of AgNo3 to prepare 2L of 0.01M solution. Grams of AgNo3 available after prepation of solution = 4-3.4=0.6 gm

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