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Chapter 4: Problem 112

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 M silver nitrate solution to reach the equivalence point in the titration. What is the mass percentage of chloride ion in 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 1.767%.

Step by step solution

01

Find the moles of chloride ions in the sample using the titration information.

Given that 42.58 mL of 0.2997 M silver nitrate solution was used to reach the equivalence point, the moles of silver nitrate (AgNO3) can be found using the formula: moles of AgNO3 = volume of AgNO3 (L) × molarity of AgNO3 (mol/L) Convert the volume from mL to L: \(42.58\,mL × \frac{1\,L}{1000\,mL} = 0.04258\,L \) Then, calculate the moles of AgNO3: \(moles\,of\,AgNO_3 = 0.04258\,L × 0.2997\,mol/L = 0.01277\,mol\) Since the reaction between AgNO3 and Cl- is a 1:1 ratio, the moles of Cl- are equal to the moles of AgNO3: moles of Cl- = moles of AgNO3 = 0.01277 mol
02

Calculate the mass of chloride ions in the sample.

Now that we have the moles of Cl-, let's find the mass using the molar mass of Cl- (35.45 g/mol): mass of Cl- = moles of Cl- × molar mass of Cl- mass of Cl- = 0.01277 mol × 35.45 g/mol = 0.453 g
03

Determine the mass of the seawater sample.

We are given that the density of the seawater is 1.025 g/mL, and the volume of the seawater sample is 25.00 mL. We can calculate the mass of the seawater sample using the formula: mass = volume × density mass = 25.00 mL × 1.025 g/mL = 25.63 g
04

Calculate the mass percentage of chloride ions in the seawater sample.

Now that we have both the mass of chloride ions and the mass of the seawater sample, we can find the mass percentage using the formula: mass percentage = (mass of Cl- / mass of seawater) × 100% mass percentage = (0.453 g / 25.63 g) × 100% = 1.767% The mass percentage of chloride ions in the seawater sample is approximately 1.767%.

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Most popular questions from this chapter

(a) A strontium hydroxide solution is prepared by dissolving 12.50 g of \(\operatorname{Sr}(\mathrm{OH})_{2}\) in water to make 50.00 \(\mathrm{mL}\) of solution. What is the molarity of this solution? (b) Next the strontium hydroxide solution prepared in part (a) is used to titrate a nitric acid solution of unknown concentration. Write a balanced chemical equation to represent the reaction between strontium hydroxide and nitric acid solutions. (c) If 23.9 mL of the strontium hydroxide solution was needed to neutralize a 37.5 mL aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?

Separate samples of a solution of an unknown salt are treated with dilute solutions of \(\mathrm{HBr}, \mathrm{H}_{2} \mathrm{SO}_{4},\) and \(\mathrm{NaOH} .\) A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: \(\mathrm{K}^{+}, \mathrm{Pb}^{2+}, \mathrm{Ba}^{2+}.\)

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCl in the stomach and each of the following substances used in various antacids: (a) \(\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s}),\) (b) \(\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})\), \((\mathbf{c}) \mathrm{MgCO}_{3}(s)\), \((\mathbf{d}) \mathrm{NaAl}\left(\mathrm{CO}_{3}\right)(\mathrm{OH})_{2}(s),\) (e) \(\mathrm{CaCO}_{3}(\mathrm{s}).\)

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) \(\mathrm{LiClO}_{4}\), (b) \(\mathrm{HClO}\), (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\) (propanol), \((\mathbf{d}) \mathrm{HClO}_{3}\) (e) \(\mathrm{CuSO}_{4}\), \((\mathbf{f}) \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) (sucrose).

Consider the following reagents: zinc, copper, mercury (density 13.6 \(\mathrm{g} / \mathrm{mL}\) , silver nitrate solution, nitric acid solution. (a) Given a 500 -mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?
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