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A 130.0 −mL sample of a solution that is 3.0×10−3 M in AgNO3 is mixed with a 230.0 −mL sample of a solution that is 0.14 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

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Hagrid
Given:

Volume of AgNO3 = 130 ml
Concentration of AgNO3 = 3.0x10^-3 M
Volume of NaCN = 230 ml
Concentration of NaCN = 0.14 M

Determine the moles of each reactant:

mol AgNO3 = 3.0x10^-3 mol/L * 0.130 L = 3.9x10^-4 moles
mol NaCN = 0.14 mol/L * 0.230 L = 0.0322 moles
Balanced Chemical Equation:

    AgNO3    +     NaCN ====> NaNO3 + AgCN 
I   3.9x10^-4        0.0322              0            0
C      -x                     -x                   x            x
E  3.9x10^-4 - x   0.0322 -x           x           x

solve for x 

the value of x will be the number of moles of AgCN and NaNO3 at equilibrium. 

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