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Chapter 8: QDE (page 182)

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

Short Answer

Expert verified

The pH of the given solution is 6.99

Step by step solution

01

Define the formula for PH calculation.

The pH of a solution can be calculated as,

$p H = - l o g A_{H^{+}} = - l o g [H^{+}] 纬_{H^{+}}$

where,

$A_{H^{+}}$ - activity of hydrogne ion

$纬_{H^{+}}$ - activity coefficient of hydrogne ion.

02

Calculate the PH form the activity.

Given

0.050MLiBr at $25 掳 C$

At an ionic strength role="math" localid="1654765585845" $(渭)$ of and $纬_{OH} = 0.81$ .

role="math" localid="1654765776290" $[H^{+}] 纬_{H^{+}} [{OH}^{-}] 纬_{OH} = (x) (0.86) (x) (0.81) = 1.0 脳 10^{- 14} x = 1.2 脳 10^{- 7} M .$

The concentration of $H^{+}$ ion is $1.2 脳 10^{- 7} M$

Calculate the pH by using the concentration of $H^{+}$ ion

$pH = - \log [(1.2 脳 10^{- 7}) (0.86)] = 6.99$

Thus, theof the given solution is 6.99 .

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Most popular questions from this chapter

(a) Write the mass balance for ${CaCl}_{2}$ in water if the species are ${Ca}^{2 +}$ and ${CI}^{-}$ .

(b) Write the mass balance if the species are ${Ca}^{2 +}, {CI}^{-}, {CaCI}^{+}$ , and ${CaOH}^{+}$

(c) Write the charge balance for part (b).

Write the charge balance for a solution of $H_{2} {SO}_{4}$ in water if the $H_{2} {SO}_{4}$ ionizes $H_{2} {SO}^{-}_{4}$ to and ${SO}^{2 -}_{4}$

(a) Following the example of Mg(OH)₂ in Section 8-5, write the equations needed to find the solubility of Ca(OH)₂. Include activity coefficients where appropriate. Look up the equilibrium constants in Appendixes F and I.

(b) Suppose that the size of CaOH⁺= Ca(H₂O)₅(OH)⁺ is 500 pm. Including activity coefficients, compute the concentrations of all species, the fraction of hydrolysis (= [CaOH⁺]/{[Ca²⁺] + [CaOH⁺]}), and the solubility of Ca(OH)₂ in g/L. The Handbook of Chemistry and Physics lists the solubility of Ca(OH)₂ as 1.85 g/L at 0⁰C and 0.77 g/L at 100⁰C

Calculate the ionic strength of (a) 0.008 7 M KOH and (b) 0.000 2 $M - La {({IO}_{3})}_{3}$ (assuming complete disassociation at this low concentration and no hydrolysis reaction to make ${LaOH}^{2 +}$ ).

Including activity coefficient, find the concentration of ${Ba}^{2 +}$ in $0.100 M {({CH}_{3})}_{4} {NIO}_{3}$ solution saturated with $Ba {({IO}_{3})}_{2}$ .

See all solutions

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