Question #54da7

1. Assume the following data for the density of water and nitric acid.
   #HNO_3=1.42" g/ml"# #("concentrated"#)
   #H_2O=1.00" g/ml"# # ("at " 4^oC#)
2. Since the provided data are in grams, convert it to volume. Observe uniformity of units; i.e.,
   #V_(HNO_3)=(630cancel(g))/((1.42cancel(g))/(ml))=443.6620mL~~443.7mL#
   #V_(H_2O)=(6500cancel(g))/((1.00cancel(g))/(ml))=6500mL#
3. Find the volume of the solution. Note that volume solution is the summation of the volume of the solute and the solvent as shown below.
   #"Volume"_("solution")="volume solute"+"volume solvent"#

#"Volume"_("solution")=443.7mL+6500mL#

#"Volume"_("solution")=6943.7cancel(mL)xx(1L)/(1000cancel(mL))=6.9437L~~7.0000L#
4. Find the mole value of nitric acid #(etaHNO_3)# by taking the quotient of its #"mass"=630g# against its # "molar mass"=63.012" g/mol"#; so that,
#eta=(mHNO_3)/(MmHNO_3)#
#eta=(630g)/((63.012g)/(mol))#
#eta=9.998mol#
5. From the formula #"Molarity"(M)=("number of moles"(eta))/("Li solution"(V)#, find the concentration of the solution.
#M=eta/V#
#M=(9.998mol)/(7.0000L)#
#M=1.4283" mol/L"~~1.4283M#