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Chapter 4: Problem 113

The mass percentage of chloride ion in a 25.00-mL sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took \(42.58 \mathrm{~mL}\) of \(0.2997 \mathrm{M}\) silver nitrate solution to reach the equivalence point in the titration. What is the mass percentage of chloride ion in the seawater if its density is \(1.025 \mathrm{~g} / \mathrm{mL} ?\)

Short Answer

Expert verified
The mass percentage of chloride ions in the seawater sample is approximately \(1.765 \% \).

Step by step solution

01

Write the balanced chemical equation

The balanced chemical equation of the reaction between silver nitrate (AgNO鈧�) and chloride ions (Cl鈦�) is as follows: \[AgNO_3(aq)+Cl^-(aq) \rightarrow AgCl(s)+NO_3^-(aq)\] Here, 1 mole of AgNO鈧� reacts with 1 mole of Cl鈦� to form 1 mole of AgCl as the precipitate.
02

Calculate the moles of silver nitrate used in titration

We are given the volume and concentration of the silver nitrate solution, so we can calculate the moles of AgNO鈧� used as follows: Moles of AgNO鈧� = Volume 脳 Concentration \[\text{Moles of AgNO鈧儅 = 42.58 \mathrm{~mL} 脳 0.2997 \frac{\mathrm{mol}}{\mathrm{L}} \times \frac{1 \mathrm{~L}}{1000 \mathrm{~mL}} = 0.012765 \mathrm{~mol}\]
03

Calculate the moles of chloride ions

From the balanced chemical equation, we know that 1 mole of AgNO鈧� reacts with 1 mole of Cl鈦�. So, the moles of Cl鈦� in the seawater sample would be equal to the moles of AgNO鈧� used in the titration. Moles of Cl鈦� = Moles of AgNO鈧� \[\text{Moles of Cl鈦粆 = 0.012765 \mathrm{~mol}\]
04

Calculate the mass of chloride ions

Now that we have the moles of Cl鈦�, we can find its mass using the molecular weight of chloride ions (MW of Cl = 35.45 g/mol). Mass of Cl鈦� = Moles of Cl鈦� 脳 Molecular weight \[\text{Mass of Cl鈦粆 = 0.012765 \mathrm{~mol} 脳 35.45 \frac{\mathrm{g}}{\mathrm{mol}} = 0.4524 \mathrm{~g}\]
05

Calculate the mass of the seawater sample

We are given the volume and density of the seawater sample. We can calculate the mass of the sample as follows: Mass of seawater = Volume 脳 Density \[\text{Mass of seawater} = 25.00 \mathrm{~mL} 脳 1.025 \frac{\mathrm{g}}{\mathrm{mL}} = 25.625 \mathrm{~g}\]
06

Calculate the mass percentage of chloride ions

Now we can calculate the mass percentage of chloride ions in the seawater sample using the mass of chloride ions and the mass of seawater: Mass percentage of Cl鈦� = (Mass of Cl鈦� / Mass of seawater) 脳 100 \[\text{Mass percentage of Cl鈦粆 = \frac{0.4524 \mathrm{~g}}{25.625 \mathrm{~g}} \times 100 = 1.765 \% \] So, the mass percentage of chloride ions in the seawater sample is approximately \(1.765 \% \).

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Most popular questions from this chapter

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows: \(2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) $$ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g) $$ Sodium bicarbonate is added untilthe fizzing due to the formation of \(\mathrm{CO}_{2}(\mathrm{~g})\) stops. If \(27 \mathrm{~mL}\) of \(6.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) was spilled, what is the minimum mass of \(\mathrm{NaHCO}_{3}\) that must be added to the spill to neutralize the acid?

Explain how a redox reaction involves electrons in the same way that an acid- base reaction involves protons. [Sections \(4.3\) and \(4.4]\)

Which of the following solutions is the most basic? (a) \(0.6 \mathrm{M} \mathrm{NH}_{3}\), (b) \(0.150 \mathrm{M} \mathrm{KOH}\), (c) \(0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\). Explain.

You know that an unlabeled bottle contains a solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2}\), or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\). A friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with \(\mathrm{NaCl}\) solutions. Explain how these two tests together would be sufficient to determine which salt is present in the solution.

In each of the following pairs, indicate which has the higher concentration of \(\mathrm{Cl}^{-}\) ion: (a) \(0.10 \mathrm{M} \mathrm{CaCl}_{2}\) or \(0.15 \mathrm{M} \mathrm{KCl}\) solution, (b) \(100 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{KCl}\) solution or \(400 \mathrm{~mL}\) of \(0.080 \mathrm{M} \mathrm{LiCl}\) solution, (c) \(0.050 \mathrm{M} \mathrm{HCl}\) solution or \(0.020 \mathrm{M} \mathrm{CdCl}_{2}\) solution.
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