Calculate the number of moles of ag + in 5.00 ml of 2.00*10-3 m agno3 and the number of moles of cro2-4 in 5.00 ml of 3.10*10-3 m k2cro4.

Molarity = number of moles of solute / Volume of solution

the unit : mol / L

For AgNO₃ solution,

AgNO₃ (aq) →Ag⁺ (aq) + NO₃⁻ (aq)

since stoichiometric ratio between AgNO₃ (aq) and Ag⁺ (aq) is 1 : 1,

the molarity of Ag⁺ (aq) is 2.00*10⁻³ M

Hence moles of Ag⁺ (aq) in 5.00 mL = (2.00*10⁻³ mol / L) * 5.00 x 10⁻³ L

= 1.00 x 10⁻⁵ mol

For K₂CrO₄ solution,

K₂CrO₄ (aq) →2K⁺ (aq) + CrO₄²⁻ (aq)

since stoichiometric ratio between K₂CrO₄ (aq) and CrO₄²⁻ (aq) is 1 : 1,

the molarity of CrO₄²⁻ (aq) is 3.10*10⁻³ M

Hence moles of CrO₄²⁻ (aq) in 5.00 mL = (3.10*10⁻³ mol / L) * 5.00 x 10⁻³ L

= 1.55 x 10⁻⁵ mol