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Chapter 6: Q37P (page 143)

Calculate the pHof pure water at (a) $25 掳 C$ and (b) $100 掳 C$ .

Short Answer

Expert verified

The pH value at $25 掳 C$ is 6.998

The pH value at $100 掳 C$ is 6.132

Step by step solution

01

Formula used

The pH of the solution can be calculated as:

$pH = - \log [H^{+}]$

The formula of the ionic product of water is:

$K_{w} = [H^{+}] [{OH}^{-}]$

Where,

$K_{w} = 1.0 脳 10^{- 14}$

02

Calculate the pH value at 25°C

(a)

Firstly calculate the pH value at $25 掳 C$

$K_{w} = [H^{+}] [{OH}^{-}] = 1.0 脳 10^{- 14}$

Let the concentration of $[H^{+}] = [{OH}^{鈥�}] = x$

$x^{2} = 1.0 脳 10^{- 14} x = [H^{+}] = 1.005 脳 10^{7} pH = - \log (1.005 脳 10^{- 7}) = 6.998 鈮� 7$

(b)

Calculate the pH value at $100 掳 C$

At $K_{w} = 5.43 脳 10^{- 14}$

$K_{w} = [H^{+}] [{OH}^{-}] = 5.43 脳 10^{- 13}$

Let the concentration of $[H^{+}] = [{OH}^{鈥�}] = x$

x^{2} = 5.43 脳 10^{- 13} x = [H^{+}] = 7.368 脳 10^{7} pH = - \log (7.368 脳 10^{- 7}) pH = 6.132

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Most popular questions from this chapter

$K_{a}$ for chloroacetic acid is $1.36 脳 10^{- 3} .$ Find $K_{b}$ for chloroacetate ion.

Given the following equilibria, calculate the concentration of

each zinc species in a solution saturated with $Zn {(OH)}_{2} (s)$ and containing $[{OH}^{-}]$

at a fixed concentration of $3.2 脳 10^{27} M$ .

$Zn {(OH)}_{2} (s) Ksp = 3 脳 10^{- 16} Zn {(OH)}^{+} 尾_{1} = 1 脳 10^{4} Zn {(OH)}_{2} (aq) 尾_{2} = 2 脳 10^{10} Zn {(OH)}_{3}^{-} 尾_{3} = 8 脳 10^{13} Zn {(OH)}_{4}^{2 -} 尾_{3} = 3 脳 10^{15}$

A solution contains $0.010 M {Ba}^{2 +}$ and $0.010 M {Ag}^{2}$ . Can 99.90% of either ion be precipitated by chromate ${CrO}_{4}^{2 -}$ without precipitating the other metal ion?

Find $[{Cu}^{2 +}]$ in a solution saturated with ${Cu}_{4} {(OH)}_{6} ({so}_{4})$ if $[{OH}^{-}]$ is fixed at $1.0 脳 10^{- 6} M$ . Note that ${Cu}_{4} {(OH)}_{6} ({so}_{4})$ gives 1mol of ${SO}_{4}^{2 -}$ 4 mol for of ${Cu}^{2 +}$ .

${Cu}_{4} {(OH)}_{6} ({so}_{4}) (s) 鈬� 4 C u^{2 +} + 6 O H^{-} + S O_{4}^{2 -} K_{s p} = 2.3 脳 10^{- 69}$

(a) Using only $K_{sp}$ from Table 6-3, calculate how many moles

of $Ca (OH)_{2}$ will dissolve in 1.00 L of water.

(b) How will the solubility calculated in part (a) be affected by the $K_{1}$ reaction in Table 6-3?

See all solutions

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