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Chapter 9: Q6TY (page 200)

Find the pH if only 6.30 instead of 12.0 mL HCl were added

Short Answer

Expert verified

The of Hydrochloric acid was 8.51 if the volume is 6.0ml

Step by step solution

01

Define the Henderson-Hasselbalch Equation.

The relationship between acid pH and pKa in aqueous solutions is described by the Henderson-Hasselbalch equation (acid dissociation constant). This equation can be used to forecast the pH of a buffer solution when the concentrations of such acid as well as its conjugate base, or the base and the related conjugate acid, are determined.

02

Calculate the pH of Hydrochloric acid.

Consider a basic reaction:

${BH}^{+} \overset{K_{a} = K_{w} / K_{b}}{饾啅} B + H^{+}, pH = {pK}_{a} + \log \frac{|B|}{[{BH}^{+}]}$

Where,

${pK}_{a} =$ acid dissociation constant for weak acid ${BH}^{+}$

Moles of $H^{+} = (0.006 L) (1.00 mol / L) = 0.006 molH +$

$Initial moles \begin{matrix} B & + & H^{+} & 鈫� {BH}^{+} \\ 0.1206 & 0.006 & 0.0296 \end{matrix}$

Final moles 0.0966 - 0.0356

$pH = {pK}_{a} + \log \frac{moles of B}{moles of {BH}^{+}}$

Now

$pH = 8.072 + \log \frac{0.0966}{0.0356} pH = 8.51$

Thus, the of Hydrochloric acid was 8.51 if the volume is 6.0ml.

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Most popular questions from this chapter

Find the pH of 0.050 M triethylammonium bromide.

How many milliliters of $0.246 {MHNO}_{3}$ should be added to $213 mL$ of $0.00666 M 2,$ -bipyridine to give a pH of $4.19$ ?

${Cr}^{3 +}$ is acidic by virtue of the hydrolysis reaction ${Cr}^{3 +} H_{2} O \overset{K_{aI}}{鈬�} Cr {(OH)}^{2 +} + H^{+}$ . [Further reactions produce $Cr {(OH)}_{2,}^{+} Cr {(OH)}_{3}$ and.] Find the value role="math" localid="1654864894349" $K_{aI}$ of in Figure 6-9. Considering only the $K_{aI}$ reaction, find pH value ofrole="math" localid="1654865110221" $0.010 MCr {({CIO}_{4})}_{3}$ What fraction of chromium is in the formrole="math" localid="1654865163335" $Cr {(OH)}^{2 +}$ ?

Find the pH of 0.050 M sodium butanoate (the sodium salt of

butanoic acid, also called butyric acid).

When is a weak acid weak and when is a weak acid strong? Show that the weak acid $99 %$ dissociatedrole="math" localid="1654854665468" $F = (0.0102) K_{a}$ will be 92%dissociated when dissolved in water if the formal concentration is one-tenth $(F = Ka / 10)$ of Show that the fraction of dissociation is 27%when $F = 10 Ka$ . At what formal concentration will the acid be 99%dissociatedCompare your answer with the left -hand curve in Figure 9-2

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