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Chapter 8: Q6 TY (page 169)

Find $[H^{+}]$ and the pH of $0.05 {MI}^{2} {NO}_{3}$ .

Short Answer

Expert verified

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

The pH is 6.99.

Step by step solution

01

Concept used.

pH of a solution:

The pH of a solution can be calculated by,

$pH =- {logA}_{H^{+}}$

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

With the help of above equation, the negative logarithm of activity of $H^{+}$ ion can be calculated.

02

Step 2: Calculate the value of [H+] and the pH of .

At an ionic strength $(渭)$ of $0.050 M, 纬_{H^{+}} = 0.86$ and $纬_{O H} = 0.81$ from the table 8 - 1.

role="math" localid="1663412820591" $K_{w} = [H^{+}] 纬_{H^{+}} [{OH}^{-}] 纬_{{OH}^{-}} = (x) (0.86) (x) (0.81) = 1.0 脳 10^{- 14} x = [H^{+}] = 1.2 脳 10^{- 7} M$

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

By using the concentration and activity coefficient of ion calculate the pH

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

The pH is 6.99.

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Most popular questions from this chapter

Write the equilibrium expression for ${Ca}^{2 +} + 2 {Cl}^{-} 鈫� {Cacl}_{2} (aq)$ with activity coefficients.

Write the charge balance for an aqueous solution of arsenic acid, $H_{3} {AsO}_{4}$ , in which the acid can disassociate to role="math" localid="1654936423245" $H_{3} {AsO}^{-}_{4}, H {AsO}_{4}^{2 -}, {andAsO}_{4}^{3 -}$ . Look up the structure of arsenic acid in Appendix G and write the structure of ${HAsO}^{2 -}_{4}$

15.Activity coefficient of a neutral molecule. We use the approximation

that the activity coefficient $(纬)$ of neutral molecules is 1.00.A more accurate relation is $濒辞驳纬 = 办渭$ , where $渭$ is ionic strengthand $k 鈮� 0.11$ for ${NH}_{3}$ and ${CO}_{2}$ and $k 鈮� 0.2$ for organic molecules.With activity coefficients for $HA, A^{-}$ ,and $H^{+}$ , predict the value ofthe quotient below for benzoic acid $^{(HA = C_{6} H_{5} {CO}_{2} H)}$ The observed quotient is $^{0.63 卤 0.03}$ .

Concentration quotient $= \frac{\frac{[H^{+}] [A^{-}]}{[HA]} (at 渭 = 0)}{\frac{[H^{+}] [A^{-}]}{[HA]} (at 渭 = 0.1 M)}$

Using activities, calculate the pH of a solution containing 0.010 M NaOH plus 0.012 0 M LiNO₃ . What would be the pH if you neglected activities?

Which statements are true In the ionic strength range $0_{I} 0.1 M,$

activity coefficients decrease with

a) increasing ionic strength

b) increasing ionic charge

c) decreasing hydrated radius

See all solutions

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