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Chapter 8: Q1 TY (page 163)

What is the ionic strength of $1 {mMCaCl}_{2}$ ?

Short Answer

Expert verified

The ionic strength of $1 {mMCaCl}_{2}$ is 3mM.

Step by step solution

01

Define the concept used

Ionic strength $(μ)$ :

The ionic strength $(μ)$ of the solution is given by

$μ = \frac{1}{2} (c_{1} z_{1}^{2} + c_{1} z_{1}^{2} + . . . . . . .) = \frac{1}{2} \sum_{} c_{i} z_{i}^{2}$

02

Step 2: Calculate the ionic strength of 1mMCaCl2

Using the ionic strength calculation formula, calculate the ionic strength.

$μ = \frac{1}{2} [[{Ca}^{2 +}] {(+ 2)}^{2} + 2 [{Cl}^{-}] {(- 1)}^{2}] = (\frac{1}{2} [(1) {(+ 2)}^{2} + 2 [1] {(- 1)}^{2}]) mM = (\frac{1}{2} [4 + 2]) mM = 3 mM$

The ionic strength of $1 {mMCaCl}_{2}$ is 3mM.

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Most popular questions from this chapter

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

Solubility with Activity: Find the concentration of the major species in a saturated aqueous solution of $LiF$ . Consider these reactions:

$LiF (s) ֏ {Li}^{+} + F^{-} K_{sp} = [{Li}^{+}] γ_{{Li}^{+}} [F^{-}] γ_{F^{-}} LiF (s) ֏ LiF (aq) K_{ionpair} = [LiF (aq)] γLiF (aq) F^{-} + H_{2} O ֏ HF + {OH}^{-} K_{b} = \frac{K_{w}}{K_{a}} (forHF) H_{2} O \overset{K_{w}}{֏} H^{+} + {OH}^{-} K_{w} = [H^{+}] γ_{H^{+}} [{OH}^{-}] γ_{{OH}^{-}}$

Look up the equilibrium constants in the appendixes and write their pK values. The ion pair reaction is the sum of localid="1654945209684" $LiF (s) ֏ {Li}^{+} + F^{-}$ from the Appendix ${FandLi}^{+} ֏ LiF (aq)$ from Appendix J. write the equilibrium constant expressions and the charge and mass balance.
Create a spreadsheet that uses activities to find the concentration of all species and the ionic strength. Use pH and pOH as independent variables to estimate. It does not work to choose pH and pLi because their concentration fixes that of the other through the relation $K_{sp} = [{Li}^{+}] γ_{{Li}^{+}} [F^{-}] γ_{F^{-}}$

Ammonia equilibrium solved with Goal Seek. Modify Figure $8 - 7$ to find the concentration of species in $0.05 M {NH}_{3}$ . The only change required is the value of F . How do the pH and fraction of ammonia hydrolysis role="math" localid="1654938461639" $(= \frac{[{NH}^{+}_{4}]}{[{NH}^{+}_{4}]} + [{NH}_{3}])$ change when the formal concentration of ${NH}_{3}$ increases from 0.01 to 0.05 M?

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

Write the charge and mass balances for dissolving ${CaF}_{2}$ in water if the reactions are

role="math" localid="1654770961556" ${CaF}_{2} (s) ٟ {Ca}^{2 +} + 2 F {Ca}^{2 +} + H_{2} O ٟ {CaOH}^{+} + H^{+} {Ca}^{2 +} F ؚ {CaF}^{+} {CaF}_{2} (s) ؚ {CaF}_{2} (aq) F + H^{+} ؚ HF (aq) HF (aq) + F ؚ {HF}_{2}$

See all solutions

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