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Chapter 19: Q19.16P (page 873)

Find the pH of a buffer that consists of 0.95M HBrO and 0.68M KBrO ( ${pK}_{a}$ of HBrO=8.64).

Short Answer

Expert verified

The pH value of the given buffer solution is 8.49.

Step by step solution

01

Ionic Equilibrium

An ionic equilibrium refers to an equilibrium that exists in the solution of weak electrolytes between unionized molecules and ions.

02

The pH of the buffer solution

Write the 0.95 MHBrOdissociation equation first.

${HBrO +H}_{2} O ⇌ {BrO}^{-} {+H}_{3} O^{+} .$

Then, write the 0.68 MKBrOdissociation equation.

$KBrO \to {BrO}^{-} {+K}^{+} .$

We now have the initial hypobromus acid and hypobromite concentrations.

$HBrO = 0.95 M. {BrO}^{-} = 0.68 M.$

To find the pH, we may utilize the Henderson-Hasselbalch equation.

$pH = pKa + log \frac{[{BrO}^{-}]}{[HBrO]} = 8.64 + log \frac{0.68 M}{0.95 M} = 8.49.$

Therefore, the pH value of the given buffer solution is 8.49.

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Most popular questions from this chapter

Because of the toxicity of mercury compounds, mercury $(I)$ chloride is used in antibacterial salves. The mercury $(I)$ ionrole="math" localid="1663276416837" ${(Hg}_{2}^{2 +})$ consists of two boundsions.

(a) What is the empirical formula of mercury $(I)$ chloride?

(b) Calculate ${(Hg}_{2}^{2 +})$ in a saturated solution of mercury $(I)$ chloride $(K_{sp} = 1.5 \times 10^{- 18})$ .

(c) A seawater sample contains $0.20 lb$ of $NaCL$ per gallon. Find ${[Hg}_{2}^{2 +}]$ if the seawater is saturated with mercury role="math" localid="1663276630148" $(I)$ chloride.

(d) How many grams of mercury $(I)$ chloride is needed to saturate $4900 {km}^{3}$ of pure water (the volume of Lake Michigan)?

(e) How many grams of mercury $(I)$ chloride is needed to saturate $4900 {km}^{3}$ of seawater?

Find the pH of the equivalence point(s) and the volume (mL) of $0 .0372 M NaOH$ needed to reach it in titrations of

(a)role="math" localid="1663315329302" $42.2 mL$ of $0.0520 {M CH}_{3} COOH$ .

(b) $28.9 mL$ of $0.0850 {M H}_{2} {SO}_{3}$ (two equivalence points)

Some kidney stones form by the precipitation of calcium oxalate monohydrate $({CaC}_{2} O_{4} \times H_{2} O, K_{sp} = 2.3 \times 10^{- 9})$ . Theof urine varies from $5.5$ to $7.0$ , and the average $[{Ca}^{2 +}]$ in urine is $2.6 \times 10^{- 3} M$ .

(a) If the [oxalic acid] in urine is $3.0 \times 10^{- 13} M$ , will kidney stones form atrole="math" localid="1663267818783" $pH = 5.5$ ?

(b)at $pH = 7.0$ ?

(c) Vegetarians have a urineabove $7$ . Are they more or less likely to form kidney stones?

An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers. Find the pHof (a) $0.100 M HClO$ and $0.100 M NaClO$ ; (b) $0.100 M HClO$ and $0.150 M NaClO$ ; (c) $0.150 M HClO$ and $0.100 M NaClO$ ; (d) $1.0 L$ of the solution in part (a) after $0.0050$ mol of $NaOH$ has been added.?

$NaCl$ is purified by adding $HCl$ to a saturated solution of $NaCl (317 g / L)$ . When $28.5 mL$ of $8.65 M HCl$ is added to $0.100 L$ of saturated solution, what mass (g) of pure $NaCl$ precipitates?

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