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Chapter 8: Q8 TY (page 171)

Write two mass balances for a 1.0Lsolution containing 0.100molof sodium acetate.

Short Answer

Expert verified

The mass balances are $[{Na}^{+}] = 0.100 M$ and $[{CH}_{3} {CO}_{2}^{-}] + [{CH}_{3} {CO}_{2} H] = 0.100 M$ .

Step by step solution

01

Concept used.

Mass balance:

All species in a solution containing a certain atom (or group of atoms) must be equal to the amount of that atom (or group) given to the solution.

02

Step 2: Calculate the two mass balances.

By definition, mass balance of the solution is given by

For sodium ion:

$[{Na}^{+}] = 0.100 M$

For acetate ion:

$[{CH}_{3} {CO}_{2}^{-}] + [{CH}_{3} {CO}_{2} H] = 0.100 M (dissociated product) (undissociated product) (amount of acetic acid put into the solution)$

Therefore, mass balance equation for 1.0L solution of $0.100 molNa + {CH}_{3} {CO}_{2}^{-}$ was given.

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Most popular questions from this chapter

Ammonia Equilibrium treated by solver. We now use the solve spreadsheet introduced in Figure 8 - 9 for ${TIN}_{3}$ solubility to find the concentration of species in 0.01 M ammonia solution, neglecting activity coefficient. In the systematic treatment of equilibrium of ${NH}_{3}$ hydrolysis, we have four unknowns $([{NH}_{3}], [{NH}_{4}^{+}], [H^{+}], [{OH}^{-}])$ and two equilibrium (8-13) , (8-14). Therefore we will estimate the concentration of 4unknowns - 2equilibirum = 2species, for which I choose localid="1663566766281" ${NH}^{+} and {OH}^{-}$ . Setup the spreadsheet shown below, in which the estimate localid="1663566820791" ${pNH}_{4}^{+} = 3 . {pOH}^{-}$ = 3 appears in B6andB7 . (Estimates comes from the $K_{b}$ equilibrium 8-17 with $[{NH}_{4}^{+}] = [{OH}^{-}] = \sqrt{K_{b} [{NH}_{3}]} \approx \sqrt{10^{- 4.755} [0.01]} \Rightarrow {pNH}_{4}^{+} = {pOH}^{-} \approx 3$ . Estimate donot have to be very good for Solver to work. The formula in cell C8 is $[{NH}_{3}] = [{NH}_{4}^{+}]$ .

$[{OH}^{-}] / K_{b}$ and the formula in the cell C9 is $[H^{+}] = K_{w} / [{OH}^{-}]$ . The mass balance $b_{1}$ appears in cell F6 and the charge balance $b_{2}$ appears in cell F7 . Cell F8 has the sum $b_{1}^{2} + b_{2}^{2}$ . As described for ${TIN}_{3}$ on page 176, open the solver window and set the Solver Option. Then use the Solver to set the target cell F8 Equal to Min by changing cells B6 : B7 . What are the concentrations of the species? What fraction of ammonia $(= [{NH}_{4}^{+}] / [{NH}_{4}^{+}] + [{NH}_{3}])$ is hydrolyzed. Your answer should agree with those from Goal Seek in Figure 8-8

By interpolation, find $γ$ for $H^{+}$ when $μ = 0.06 M$ .

Write the charge balance for a solution containing $H^{+}, {OH}^{-}, {Ca}^{2 +}, {HCO}_{3}^{-}, {CO}_{3}^{2 -}, Ca {({HCO}_{3})}^{+}, Ca {(OH)}^{+}, K^{+} and {ClO}_{4}^{-}$

Using activities, calculate the pH and concentration of $H^{+}$ in 0.050MLiBr at $25 ° C$ .

Find the activity coefficient of $H^{+}$ in a solution containing $0.010 M HCI$ plus $0.040 M {KCIO}_{4}$ . What is the pH of the solution?

See all solutions

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