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Chapter 9: Q6TY (page 200)

Find the pH if only 6.0 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 $H^{+} = (0.006 L) (1.00 mol / L) = 0.006 molH +$

$Initial moles \begin{matrix} B & + & H^{+} \to {BH}^{+} \\ 0.1206 & 0.006 & 0.0296 \end{matrix} Final moles 0.0966 - 0.0356$

Now $pH = {pK}_{a} + \log \frac{\log of B}{moles of {BH}^{+}} pH = 8.072 + \log \frac{0.0966}{0.0356}$

$pH = 8.51$

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 $K_{b}$

Interpreting spectral data. The graph shows the H-nuclear magnetic resonance chemical shift of the $H_{2}$ proton on pyridine as a function of $pH$ Chemical shift is related to the environment of a proton in a molecule. If the environment changes, the chemical shift changes. Suggest an explanation for why the chemical shift changesbetween low and high Estimate ${pK}_{2}$ for pyridinium ion $(C_{5} H_{5} {NH}^{+})$

Why does buffer capacity increase as a solution becomes very acidic (pH ≈ 1) or very basic (pH ≈ 13)?

Explain how you would use a spreadsheet such as Figure 8-9 to find the and concentrations of all species if you know the values of the equilibrium constants and the formal concentration $F$

Use the Goal Seek spreadsheet at the end of the chapter to find the pH of 1.00 L of solution containing 0.030 molHA $({pK}_{a} = 2.50)$ and What would the be with the approximations [HA]=0.030 and $[A^{-}]$ =0.015?

See all solutions

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