Ask Question
26 February, 22:06

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.

+1
Answers (1)
  1. 26 February, 22:10
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “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. ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers