If you mix 40.0 ml of a 0.200 m solution of k2cro4 with an aqueous solution of agno3, what mass of solid forms? (hint: most chromates are insoluble.)

 The mass  of solid formed  is 2.654  g

       calculation

step 1: write the balanced molecular  equation

=2AgNO3(aq)  + k2CrO4(aq)→ Ag2CrO4(s) + 2 KNO3(aq)

step 2:  calculate the moles of  K2CrO4

moles =  molarity  x volume in  liters

 molarity  = 0.200 M =  0.200   mol/L

volume  = 40 .0 ml  in  liters  = 40/1000 = 0.04 liters

moles is = 0.200 mol/l  x0.04 L =0.008  moles

Step 3:  use the  mole  ratio  to determine the   moles of solid formed( Ag2CrO4)

K2CrO4 :Ag2CrO4  is   1:1  therefore  the  moles of Ag2CrO4  is  also  

0.008 moles

step 4:  calculate the mass  of Ag2CrO4

mass  = moles  x   molar  mass

  from periodic table  the   molar mass   of Ag2Cro4  

=(107.87 x2) + 52 +(16  x4)  =331.74  g/mol

mass = 0.008 moles   x 331.74 = 2.654  g

it is b. absorbs thermal energy