The molar mass i.e mass of 1 mole of Silver nitrate (AgNO3) = 169.87 g/mol
Now the given concentration of AgNO3 solution = 2.50 M = 2.50 mols/ 1000 ml
Given volume of AgNO3 solution = 185 ml
Thus total number of moles of AgNO3 in the solution = concentration * volume
= 2.50 mols/ 1000 ml * 185 ml
= 0.4625 moles
Thus mass of 0.4625 mole of Silver nitrate (AgNO3) = number of moles * molar mass
= 0.4625 moles * 169.87 g/mol
= 78.56 g
Hence the mass of AgNO3 in the solution is 78.56 g
#5 vyme 14.55 a NAOH Take 3.0L SUTULUI. -TU UUU - 0,557 L soln 3.01 5....
CHM 1210 Final practice Name: Know electrolyte table, 5 solubility rules; 26 polyatomics (name/formula) Write 7 naturally occurring diatomic molecules (name; formula, phase , charge) Write rite out strong acids and weak acids by name; formula, phase ,charge Write out the molecular, complete, and net-ionic equations for the following reactions The mixing of Cobalt(IlI) chloride and silver nitrate The mixing of acetic acid and sodium hydroxide The mixing of hydrochloric acid and cakcium hydroxide The mixing of barium chloride and...