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Chapter 16: Problem 30

In a titration experiment, \(20.4 \mathrm{~mL}\) of \(0.883 \mathrm{M}\) HCOOH neutralize \(19.3 \mathrm{~mL}\) of \(\mathrm{Ba}(\mathrm{OH})_{2} .\) What is the concentration of the \(\mathrm{Ba}(\mathrm{OH})_{2}\) solution?

Short Answer

Expert verified
The concentration of the \(Ba(OH)2\) solution is \(0.932 M\).

Step by step solution

01

Write down the balanced chemical equation

The balanced equation for the reaction is \(HCOOH + Ba(OH)2 -> BaCOOH + 2H2O\). Since the stoichiometry of the base and acid is 1:1, there is no need to adjust with it.
02

Convert milliliters to liters

The calculation has to be done by converting the given volumes to liters since the unit for molarity is mol/L. Therefore, the volume of HCOOH is \(20.4 mL = 20.4 \times 10^{-3} L\) and the volume of \(Ba(OH)2\) is \(19.3 mL = 19.3 \times 10^{-3} L\).
03

Calculate the concentration of Ba(OH)2

Apply the formula \(HCOOH's concentration \times HCOOH's volume = Ba(OH)2's concentration \times Ba(OH)2's volume\) or \(c1v1 = c2v2\), we can plug in the known values: \(0.883 mol/L \times 20.4 \times 10^{-3} L = c2 \times 19.3 \times 10^{-3} L\). Solving for \(c2\) gives us the concentration of the \(Ba(OH)2\) solution.

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of the following two buffer solutions: (a) \(2.0 \mathrm{M} \mathrm{CH}_{3} \mathrm{COONa} / 2.0 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\), (b) \(0.20 \mathrm{M} \mathrm{CH}_{3} \mathrm{COONa} / 0.20 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH} .\) Which is the more effective buffer? Why?

A \(100-\mathrm{mL} 0.100 \mathrm{M} \mathrm{CuSO}_{4}\) solution is mixed with a \(100-\mathrm{mL} 0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution. Calculate the concentrations of the ions in the combined solution.

In a titration experiment, \(12.5 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) neutralize \(50.0 \mathrm{~mL}\) of \(\mathrm{NaOH}\). What is the concentration of the \(\mathrm{NaOH}\) solution?

Use appropriate equations to account for the solubility of the amphoteric aluminum hydroxide \(\left.\left[\mathrm{Al}(\mathrm{OH})_{3}\right)\right]\) at low and high \(\mathrm{pHs}\)

Describe a simple test that would enable you to distinguish between \(\operatorname{AgNO}_{3}(s)\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(s)\)
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