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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:

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

Where,

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

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

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

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

A 0.10 M solution of a base is 2.0% hydrolzed $(α = 0.020)$ Find $K_{b}$

Find the pH of 0.050 M sodium butanoate (the sodium salt ofbutanoic acid, also called butyric acid).

Find the pH and fraction of association $(α)$ of a 0.100Msolution of the weak base B with $K_{b} = 1.00 \times 10^{- 5}$ .

Neglecting activity coefficients, calculate the pH of $5.0 \times 10^{- 8} {MHCIO}_{4}$ What fraction of $H^{+}$ is derived from dissociation of water?

Why doesn’t water produce $10^{- 7} M H^{+}$ , andwhen

is added?

See all solutions

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